Solution Chemistry

Please note that this unit is not complete yet.

1.	How many grams of CaCl2 are required to mix 100. mL of 2.00 M solution?
	A. 	11.1 g
	B. 	22.2 g
	C. 	111 g
	D. 	222 g

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


2.	How many grams of Mg(NO3)3 are required to mix 200. mL of 0.20 M solution?
	A. 	8.4 g
	B. 	42 g
	C. 	56 g
	D. 	210 g

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


3.	What mass of KCl is required to make 25.0 mL of a 0.250 M solution?

	A. 	0.466 g
	B. 	7.46 g
	C. 	74.6 g
	D. 	746 g

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


4.	What is the resulting molarity when 250. mL of 0.100 M NaBr solution is combined with 350. mL of 0.200 M NaBr solution?
	A. 	0.158 M
	B. 	0.180 M
	C. 	0.300 M
	D. 	0.150 M

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


5.	When Ba(NO3)2 is dissolved in water to form a 0.20 M solution, the concentration of each ion in the solution is
	A. 	[Ba+2]= 0.20 M and [NO3-]= 0.20 M
	B. 	[Ba+2]= 0.10 M and [NO3-]= 0.20 M
	C. 	[Ba+2]= 0.20 M and [NO3-]= 0.40 M
	D. 	[Ba+2]= 0.10 M and [NO3-]= 0.30 M

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 


6.	When Al(NO3)3 is dissolved in water to form a 0.30 M solution, the concentration of each ion in the solution is
	A. 	[Al+2]= 0.30 M and [NO3-]= 0.90 M
	B. 	[Al+2]= 0.10 M and [NO3-]= 0.30 M
	C. 	[Al+2]= 0.30 M and [NO3-]= 0.30 M
	D. 	[Al+2]= 0.30 M and [NO3-]= 0.10 M

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


7.	When Al2(SO4)3 is dissolved in water to form a 0.30 M solution, the concentration of each ion in the solution is
	A. 	[Al+2]= 0.30 M and [SO4-2]= 0.60 M
	B. 	[Al+2]= 0.30 M and [SO4-2]= 0.45 M
	C. 	[Al+2]= 0.30 M and [SO4-2]= 0.90 M
 	D. 	[Al+2]= 0.60 M and [SO4-2]= 0.90 M
 

  

     Depress mouse to view answer.
    	
 		Answer: 	D
 	
     
  
 
 
 8.	When SnCl4(s) is dissolved in water to form a 0.20 M solution, the concentration of each ion in the solution is
 	A. 	[Sn+4]= 0.20 M and [Cl-]= 0.80 M
 	B. 	[Sn+4]= 0.20 M and [Cl-]= 0.05 M
 	C. 	[Sn+4]= 0.20 M and [Cl-]= 0.20 M
 	D. 	[Sn+4]= 0.80 M and [Cl-]= 0.20 M
 

  

     Depress mouse to view answer.
    	
 		Answer: 	A
 	
     
  
 
 
 9.	The LEAST concentrated solution chosen from the following is
 
 	A. 	200 ml of 1.0 M CH3COOH(aq)
 	B. 	100 ml of 2.0 M CH3OH(aq)
 	C. 	20 ml of 1.5 M NaOH(aq)
 	D. 	150 ml of 0.75 M HNO3(aq)
 

  

     Depress mouse to view answer.
    	
 		Answer: 	D
 	
     
  
 
 
 10.	The LEAST concentrated solution chosen from the following is
 
 	A. 	200 ml of 0.10 M CH3COOH(aq)
 	B. 	100 ml of 0.20 M CH3OH(aq)
 	C. 	20 ml of 0.50 M NaOH(aq)
 	D. 	150 ml of 0.75 M HNO3(aq)
 

  

     Depress mouse to view answer.
    	
 		Answer: 	A
 	
     
  
 
 
 11.	The MOST concentrated solution chosen from the following is
 
 	A. 	25 ml of 0.10 M Fe(ClO)3(aq)
 	B. 	10 ml of 0.60 M ZnBr2(aq)
 	C. 	50 ml of 0.005 M KNO3(aq)
 	D. 	1500 ml of 0.05 M HCl(aq)
 

  

     Depress mouse to view answer.
    	
 		Answer: 	B
 	
     
  
 
 
 12.	The MOST concentrated solution chosen from the following is
 
 	A. 	25 ml of 1.00 M Fe(ClO)3(aq)
 	B. 	10 ml of 1.20 M ZnBr2(aq)
 	C. 	50 ml of 1.50 M KNO3(aq)
 	D. 	1500 ml of 0.50 M HCl(aq)
 

  

     Depress mouse to view answer.
    	
 		Answer: 	C
 	
     
  
 
 
 13.	What is the [CaI2] if 0.050 moles is dissolved to make 20.0  mL of solution?
 
 	A. 	40. M
 	B. 	25. M
 	C. 	2.5 M
 	D. 	0.40 M
 

  

     Depress mouse to view answer.
    	
 		Answer: 	C
 	
     
  
 
 
 14.	What is the molarity of 0.125 mol of NaBr dissolved in enough water to make a final solution volume of 325 mL?
 	A. 	2.60 M
 	B. 	0.385 M
 	C. 	0.0406 M
 	D. 	0.125 M
 

  

     Depress mouse to view answer.
    	
 		Answer: 	B
 	
     
  
 
 
 15.	What is the molarity if 2.50 mol of KCl is dissolved in enough water to make a final solution volume of 200. mL.
 	A. 	12.5 M
 	B. 	5.00 M
 	C. 	0.0125 M
 	D. 	80.0 M
 

  

     Depress mouse to view answer.
    	
 		Answer: 	A
 	
     
  
 
 
 16.	What is the molarity of 0.25 mol of KI is dissolved in enough water to make a final solution volume of 400. mL.
 	A. 	0.10 M
 	B. 	0.38 M
 	C. 	0.62 M
 	D. 	1.6 M
 

  

     Depress mouse to view answer.
    	
 		Answer: 	C
 	
     
  
 
 
 17.	What is the molarity of a solution made by dissolving 2.45 g of Al(OH)3 in enough water to make a solution volume of 200. mL?
 	A. 	6.37 M
 	B. 	2.56 M
 	C. 	0.00628 M
 	D. 	0.157 M
 

  

     Depress mouse to view answer.
    	
 		Answer: 	D
 	
     
  
 
 
 18.	What is the molarity of a solution made by dissolving 60.00 g of LiOH in enough water to make a solution volume of 750. mL?
 	A. 	0.080 M
 	B. 	0.532 M
 	C. 	1.88 M
 	D. 	3.34 M
 

  

     Depress mouse to view answer.
    	
 		Answer: 	D
 	
     
  
 
 
 19.	What is the molarity of a solution that has a concentration of 10.0 g/L of NaCl ?
 
 	A. 	0.171 M
 	B. 	0.446 M
 	C. 	5.85 M
 	D. 	10.0 M
 

  

     Depress mouse to view answer.
    	
 		Answer: 	A
 	
     
  
 
 
 20.	What is the molarity of a solution that has 0.86 moles of KCl dissolved in 1.2 L of solution?
 
 	A. 	0.72 M
 	B. 	0.86 M
 	C. 	1.0 M
 	D. 	1.4 M
 

  

     Depress mouse to view answer.
    	
 		Answer: 	A
 	
     
  
 
 
 21.	When 2.50 moles of a solute are dissoved in 1.00 L of water, 1.02 L of clear solution are produced.  The concentration is
 	A. 	0.400 M.
 	B. 	0.408 M.
 	C. 	2.45 M.
 	D. 	2.50 M.
 

  

     Depress mouse to view answer.
    	
 		Answer: 	C
 	
     
  
 
 
 22.	If 2.64 g of NaCl are dissolved in 2.68 L of water, then the concentration of the solution will be
 
 	A. 	0.0168 M
 	B. 	0.0451 M
 	C. 	less than 0.0168 M
 	D. 	more then 0.0168 M
 

  

     Depress mouse to view answer.
    	
 		Answer: 	C
 	
     
  
 
 
 23.	A 20.0 g sample of HF is dissolved in water to give 200 mL of solution.   The concentration of the solution is
 	A. 	1.0 M.
 	B. 	3.0 M.
 	C. 	0.10 M.
 	D. 	5.0 M.
 	E. 	10.0 M
 

  

     Depress mouse to view answer.
    	
 		Answer: 	D
 	
     
  
 
 
 24.	When 9.36 g Na0H is dissolved in enough water to make the total volume 965 mL, the concentration of the resulting solution is
 	A. 	0.970M.
 	B. 	0.242M.
 	C. 	2.42M.
 	D. 	0.234M.
 

  

     Depress mouse to view answer.
    	
 		Answer: 	B
 	
     
  
 
 
 25.	If 2.64 g of NaCl are dissolved in 2.0 L of water and then filled to make 2.68 L of solution, he concentration of the solution will be:
 	A. 	0.0168 M
 	B. 	0.0451 M
 	C. 	less then 0.0168 M
 	D. 	more than 0.0168 M
 

  

     Depress mouse to view answer.
    	
 		Answer: 	A
 	
     
  
 
 
 26.	What is the molarity of a solution that contains 4.0 g Na0H per 500. mL solution?
 
 	A. 	0.20M.
 	B. 	0.10M.
 	C. 	1.0M.
 	D. 	0.50M.
 

  

     Depress mouse to view answer.
    	
 		Answer: 	A
 	
     
  
 
 
 27.	How many moles of NaCl are contained in 25 mL of 0.60 M solution?
 
 	A. 	0.015 mol
 	B. 	0.041 mol
 	C. 	0.15 mol
 	D. 	24 mol mol
 

  

     Depress mouse to view answer.
    	
		Answer: 	A
	
    
 

 
 28.	How many moles of LiCl are contained in 250. mL of 0.40 M solution?
 
 	A. 	0.20 mol
 	B. 	0.10 mol
 	C. 	1.6 mol
 	D. 	0.020 mol

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 

 
 29.	How many moles of KBr are contained in 250. mL of 0.500 M solution?
 
 	A. 	0.500 mol
 	B. 	0.150 mol
 	C. 	0.125 mol
 	D. 	0.0250 mol

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 

 
 30.	How many moles of CsCl are contained in 750. mL of 0.50 M solution?
 
 	A. 	1.50 mol
 	B. 	0.250 mol
 	C. 	0.325 mol
 	D. 	0.375 mol

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 

 
 31.	How many moles of NaCl are contained in 75.0 mL of 0.10 M solution?
 
	 A. 	1.3 mol
 	B. 	0.75 mol
 	C. 	0.0075 mol
 	D. 	0.13 mol

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 

 
 32.	How many moles of NaNO3 are contained in 250 mL of 2.00 M solution?
 	A. 	0.20 mol
 	B. 	0.50 mol
 	C. 	0.80 mol
 	D. 	0.90 mol

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 

 
 33.	How many moles of LiNO3 are contained in 400 mL of 2.00 M solution?
 	A. 	0.20 mol
 	B. 	0.50 mol
 	C. 	0.80 mol
 	D. 	0.90 mol

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 

 
 34.	How many moles of Li2CO3 are contained in 450 mL of 2.00 M solution?
 	A. 	0.20 mol
 	B. 	0.50 mol
 	C. 	0.80 mol
 	D. 	0.90 mol

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 

 
 35.	How many moles of K2CO3 are contained in 100. mL of 2.0 M solution?
 	A. 	0.20 mol
 	B. 	0.50 mol
 	C. 	0.050 mol
 	D. 	20. mol

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 

 
 36.	Which solution, chosen from the following, has the most moles of solute?
 
 	A. 	250 ml of 0.30 M Fe(CH3COO)3(aq)
 	B. 	170 ml of 0.60 M ZnSO4(aq)
 	C. 	500 ml of 0.50 M KOH(aq)
 	D. 	1500 ml of 0.25 M HNO3(aq)

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 

 
 37.	Which solution, chosen from the following, has the most moles of solute?
 
 	A. 	250 ml of 4.0 M AgCH3COO(aq)
 	B. 	350 ml of 3.0 M Na2SO4(aq)
 	C. 	400 ml of 2.0 M LiOH(aq)
 	D. 	500 ml of 1.5 M Mg(NO3)2(aq)

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 

 
 38.	Which solution, chosen from the following, has the fewest moles of solute?
 
 	A. 	250 ml of 1.0 M AgNO3(aq)
 	B. 	80 ml of 3.0 M Na2S(aq)
 	C. 	400 ml of 0.80 M NaOH(aq)
 	D. 	500 ml of 0.50 M MgF2(aq)

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 

 
 39.	Which solution, chosen from the following, has the most moles of solute?
 
 	A. 	45 ml of 0.30 M AgCH3COO(aq)
 	B. 	75 ml of 0.20 M Na2SO4(aq)
 	C. 	50 ml of 0.25 M LiOH(aq)
 	D. 	25 ml of 0.50 M Mg(NO3)2(aq)

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 

 
 40.	Which solution, chosen from the following, has the most moles of solute?
 
 	A. 	25 ml of 0.30 M AgCH3COO(aq)
 	B. 	15 ml of 0.40 M Na2SO4(aq)
 	C. 	40 ml of 0.20 M LiOH(aq)
 	D. 	35 ml of 0.25 M Mg(NO3)2(aq)

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 

 
 41.	What volume of a 0.350 M solution of LiOH is required to obtain 0.125 mol of LiOH?
 
 	A. 	0.0438 L
 	B. 	0.0028 mL
 	C. 	0.357 L
 	D. 	0.357 mL

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 

 
 42.	What volume of a 0.200 M solution of H2SO4 contains 0.650 mol of H2SO4?
 	A. 	0.13 L
 	B. 	0.31 L
 	C. 	7.69 L
 	D. 	3.25 L

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 

 
 43.	What volume of a 0.100 M solution of LiOH would be required to obtain 2.50 g of LiOH?
 
 	A. 	25.0 L
 	B. 	1.04 L
 	C. 	0.250 L
 	D. 	2.39 L

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 

 
 44.	How many litres of 0.300 M AlF3 solution would be needed to obtain 2.50 mol of AlF3?
 	A. 	0.750 L
 	B. 	5.29 L
 	C. 	5.88 L
 	D. 	6.30 L
 	E. 	8.33 L

 

    Depress mouse to view answer.
   	
		Answer: 	E
	
    
 

 
 45.	What volume of a 0.0200 M solution of H2S is required to have 0.500 mol of H2S?
 	A. 	20.0 L
 	B. 	10.0 mL
 	C. 	40.0 mL
 	D. 	50.0 L

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 

 
 46.	What volume of a 0.500 M solution of KI would be required to obtain 20.0 g of KI?
 
 	A. 	0.241 L
 	B. 	4.15 L
 	C. 	0.482 L
 	D. 	2.07 L

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 

 
 47.	What volume of a 0.100 M solution of NiCl2 would be required to obtain 2.00 g of NiCl2?
 
 	A. 	0.077 L
 	B. 	0.154 L
 	C. 	2.50 L
 	D. 	6.49 L

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 

 
 48.	A chemical reaction requires 50.0 g of KCI; but, the KCl is only available in a 1.20 M solution.  What volume of this solution must be used to supply the necessary KCI?
 
 	A. 	0.558 L
 	B. 	0.804 L
 	C. 	1.24 L
 	D. 	1.79 L

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 

 
 49.	What volume of 0.50 M Na0H solution must you add to a reaction in order to supply 20.0 g of Na0H?
 	A. 	0.50 L
 	B. 	1.0 L
 	C. 	1.5 L
 	D. 	2.0 L

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 

 
 50.	Oil does not form an electrolytic solution because its 
 	A. 	molecules dissolve as whole molecules.
 	B. 	molecules dissociate into large ions.
 	C. 	molecucles are insoluble.
 	D. 	ions are too large to dissociate.

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 


51.	Sugar does not form an electrolytic solution because its 
	A. 	molecules dissolve as whole molecules.
	B. 	molecules dissociate into large ions.
	C. 	molecucles are insoluble.
	D. 	ions are too large to dissociate.

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


52.	An electrolytic solution is formed when 
	A. 	molecules dissolve into ions.
	B. 	molecules dissociate into ions.
	C. 	ionic crystals dissolve into molecules.
	D. 	ionic crystals dissociate into ions.

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


53.	An electric current passes through an electrolytic solution by the movement of
	A. 	electrons
	B. 	ions
	C. 	protons
	D. 	polar water molecules

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


54.	Which of the following statements about electrolytic solutions is FALSE?

	A. 	The overall net charge in the solution is either positive or negative.
	B. 	They conduct electricity.
	C. 	The solution is formed by dissolving an electrolyte in water.
	D. 	The solution contains ions.

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


55.	Which of the following statements about electrolytic solutions is FALSE?

	A. 	The overall net charge in the solution is balanced.
	B. 	They do not conduct electricity.
	C. 	The solution is formed by dissolving an electrolyte in water.
	D. 	The solution contains ions.

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


56.	Which of the following statements about electrolytic solutions is FALSE?

	A. 	The overall net charge in the solution is balanced.
	B. 	They conduct electricity.
	C. 	The solution is formed by dissolving a molecular compound in water.
	D. 	The solution contains ions.

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 


57.	Which of the following statements about electrolytic solutions is FALSE?

	A. 	The overall net charge in the solution is balanced.
	B. 	They conduct electricity.
	C. 	The solution is formed by dissolving an ionic compound in water.
	D. 	The solution contains dissolved molecules.

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


58.	Which of the following substances will form an electrolytic solution, when dissolved in water?
 
	A. 	CrCl3
	B. 	Cl2
	C. 	O3
	D. 	CH3OH

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


59.	Which of the following substances will form an electrolytic solution?
 
	A. 	N2
	B. 	Cl2O
	C. 	C6H12O6
	D. 	Ca(OH)2

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


60.	Which of the following substances will form an electrolytic solution?
 
	A. 	KNO3
	B. 	Br2O
	C. 	CH3F
	D. 	CH3OH

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


61.	Which of the following substances will form an electrolytic solution?
 
	A. 	Br2
	B. 	KCl
	C. 	C6H12O6
	D. 	CH3Cl

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


62.	Which of the following substances will form an electrolytic solution?
 
	A. 	CaBr2
	B. 	BrCl
	C. 	C6H12O6
	D. 	CH4

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


63.	Which of the following substances would be classified as a nonelectrolyte?
 
	A. 	FeF2
	B. 	LiCl
	C. 	SiO2
	D. 	NaNO3

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 


64.	Which of the following substances would be classified as a nonelectrolyte?
 
	A. 	Fe(NO3)3
	B. 	CuBr
	C. 	Na2SO3
	D. 	H2N2

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


65.	When dissolved in water, which of the following substances would not conduct electricity?
 
	A. 	Fe(NO3)3
	B. 	CuBr
	C. 	Na2SO3
	D. 	H2Te

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


66.	Which aqueous solution will probably be a good conductor of electricity?
	A. 	CH3OCH3(aq)
	B. 	P4(aq)
	C. 	I2O(aq)
	D. 	K2CO3(aq)

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


67.	Which aqueous solution will probably be a good conductor of electricity?
	A. 	CH3Cl(aq)
	B. 	Li3PO4(aq)
	C. 	N2O2(aq)
	D. 	CO(aq)

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


68.	Which of the following substances would be the best electrical conductor?  (given equal concentrations and volumes of solution)
	A. 	hexane
	B. 	sugar
	C. 	salt
	D. 	oil

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 


69.	50.0 ml of 1.0 M HCl is diluted to a volume of 500. ml. The new [HCl] is

	A. 	10. M
	B. 	2.0 M
	C. 	0.50 M
	D. 	0.10 M
	E. 	0.050 M

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


70.	20.0 ml of 2.0 M HNO3 is diluted to a volume of400. ml. The new [HNO3] is
	A. 	40. M
	B. 	1.0 M
	C. 	0.50 M
	D. 	0.10 M
	E. 	0.050 M

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


71.	200. ml of 5.0 M HNO3 is diluted to a volume of 1.0 litre. The new [HNO3] is
	A. 	25. M
	B. 	1.0 M
	C. 	0.50 M
	D. 	0.10 M
	E. 	0.050 M

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


72.	What volume of 10.0 M H2SO4 is required to make 500. mL of a 0.10 M solution?
	A. 	50.0 mL
	B. 	25.0 mL
	C. 	10.0 mL
	D. 	5.0 mL
	E. 	1.0 mL

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


73.	What volume of 1.00 M NaCl is required to make 500. mL of a 0.020 M solution?
	A. 	10. mL
	B. 	25. mL
	C. 	50. mL
	D. 	5.0 mL
	E. 	1.0 mL

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


74.	1.00 litre of 10. M HCl is diluted to a volume of 100. litres. The new [HCl] is

	A. 	10. M
	B. 	2.0 M
	C. 	1.0 M
	D. 	0.10 M
	E. 	0.050 M

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


75.	Which solution below will yield a 0.10 mol/L concentration when 100. mL of distilled water is added?

	A. 	50.0 mL of 0.30 M 
	B. 	150. mL of 0.10 M
	C. 	100. mL of 0.25 M
	D. 	25.0 mL of 0.75 M

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


76.	Which solution below will yield a 0.15 mol/L concentration when 100. mL of distilled water is added?

	A. 	50.0 mL of 0.30 M 
	B. 	150. mL of 0.20 M
	C. 	100. mL of 0.25 M
	D. 	25.0 mL of 0.75 M

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


77.	150. mL of a 2.0 M solution of ammonium phosphate is diluted to 0.50 M? The volume of water ADDED is
	A. 	750. mL
	B. 	600. mL
	C. 	450. mL
	D. 	250. mL

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 


78.	40.0 mL of a 6.00 M solution of ammonium phosphate is diluted to 0.500 M? The volume of water ADDED is
	A. 	600. mL
	B. 	480. mL
	C. 	440. mL
	D. 	400. mL

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 

79.	Which solution below will yield a 0.20 mol/L concentration when 100. mL of distilled water is added?

	A. 	50.0 mL of 0.30 M 
	B. 	150. mL of 0.20 M
	C. 	200. mL of 0.60 M
	D. 	25.0 mL of 0.75 M

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 


80.	How much of a 16.5 M stock solution of HCl would be required to make 100. mL of a 0.500 M solution?
	A. 	30.3 mL
	B. 	12.1 mL
	C. 	3.03 mL
	D. 	1.65 mL

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 


81.	How much of a 16.5 M stock solution of HCl would be required to make 250 mL of a 0.300 M solution?
	A. 	4.12 mL
	B. 	4.95 mL
	C. 	1.98 mL
	D. 	4.54 mL

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


82.	2.00 L of 12.0 M HCl is diluted with water to 6.00 L.  What is the concentration of the diluted solution?
	A. 	1.50 M
	B. 	2.00 M
	C. 	3.00 M
	D. 	4.00 M
	E. 	9.00 M

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


83.	What is the resulting molarity when 250 mL of 0.100 M NaBr solution is combined with 350 mL 
of 0.200 M NaBr solution?
	A. 	0.158 M
	B. 	0.180 M
	C. 	0.500 M
	D. 	0.142 M

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


84.	What is the resulting molarity when 150 mL of 0.350 M NaOH solution is combined with 100 mL
of 0.200 M NaOH solution?
	A. 	2.20 M
	B. 	0.290 M
	C. 	0.260 M
	D. 	0.600 M

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


85.	How much of a 12.0 M stock solution of HCl would be required to make 200. mL of a 0.500 M
solution?
	A. 	8.33 mL
	B. 	12.1 mL
	C. 	33.3 mL
	D. 	1.65 mL

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


86.	1.00 L of 12.0 M HC1 is diluted with water to 4.00 L.  What is the  concentration of the diluted solution?
	A. 	1.50 M
	B. 	2.00 M
	C. 	3.00 M
	D. 	4.00 M
	E. 	9.00 M

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 


87.	When 100. mL of 0.125M HCl is diluted to 250 mL, the resulting molarity  of HCl solution is

	A. 	0.025M.
	B. 	0.050M.
	C. 	0.625M.
	D. 	0.250M.

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


88.	How much water must you add to 1.5 L of a 0.80 M solution to make it a 0.50 M solution?

	A. 	0.3 L
	B. 	0.9 L
	C. 	1.2 L
	D. 	2.4 L

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


89.	A student has 0.25 L of a 2.0 M KCI solution.  How much water must be added to make it a 1.0 M solution?
	A. 	0.25 L
	B. 	0.50 L
	C. 	1.0 L
	D. 	2.0 L

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


90.	When a pure substance is added to water, the temperature of the water changes and a blue solution is formed that conducts electricity.  The statement describes which of the following changes?

	A. 	dissociation and dissolving
	B. 	dissolving but not dissociation
	C. 	dissociation but not dissolving
	D. 	neither dissociation or dissolving occurs

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


91.	When a pure substance is added to water, the temperature of the water increases and a  solution is formed that  does not conduct electricity.  The statement describes which of the following changes?

	A. 	dissociation and dissolving
	B. 	dissolving but not dissociation
	C. 	dissociation but not dissolving
	D. 	neither dissociation or dissolving occurs

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


92.	When a pure substance is added to water, a  heterogeneous mixture is formed that  does not conduct electricity.  The statement describes which of the following changes?

	A. 	dissociation and dissolving
	B. 	dissolving but not dissociation
	C. 	dissociation but not dissolving
	D. 	neither dissociation or dissolving occurs

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


93.	Which statement describes the changes that occur when salt is added to water?

	A. 	dissociation and dissolving
	B. 	dissolving but not dissociation
	C. 	dissociation but not dissolving
	D. 	neither dissociation or dissolving occurs

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


94.	Which statement describes the changes that occur when sugar is added to water?

	A. 	dissociation and dissolving
	B. 	dissolving but not dissociation
	C. 	dissociation but not dissolving
	D. 	neither dissociation or dissolving occurs

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


95.	Which statement describes the changes that occur when vegetable oil is added to water?

	A. 	dissociation and dissolving
	B. 	dissolving but not dissociation
	C. 	dissociation but not dissolving
	D. 	neither dissociation or dissolving occurs

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


96.	Which statement describes the changes that occur when water is added to alcohol?

	A. 	dissociation and dissolving
	B. 	dissolving but not dissociation
	C. 	dissociation but not dissolving
	D. 	neither dissociation or dissolving occurs

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


97.	Which of the following is true of neutralization reactions?

	A. 	A salt and a base are formed.
	B. 	Water is formed in an endothermic reaction.
	C. 	A salt and and acid are formed in an exothermic reaction.
	D. 	Water and a salt are formed.

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


98.	Potassium sulphate is a salt formed when sulphuric acid is used to neutralize

	A. 	potassium nitrate.
	B. 	sodium sulphate.
	C. 	sodium hydroxide.
	D. 	potassium hydroxide.

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


99.	A precipitate can generally be described as a substance which is

	A. 	common in rain.
	B. 	of low solubility.
	C. 	of low boiling point.
	D. 	a white solid.

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


100.	A beaker contains a mixture of AgNO3(aq), Cu(NO3)2(aq) and Fe(NO3)3(aq).  Some Na2SO4(aq) is added and a precipitate forms. The precipitate

	A. 	is Ag2SO4(s)
	B. 	is CuSO4(s)
	C. 	is Fe2(SO4)3(s)
	D. 	could be Ag2SO4(s) and/or Fe2(SO4)3(s)
	E. 	could be Fe2(SO4)3(s) and/or CuSO4(s)

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


101.	A beaker contains a mixture of AgNO3(aq), Ba(NO3)2(aq) and Fe(NO3)3(aq).  Some Na2SO4(aq) is added and a precipitate forms. The precipitate

	A. 	is Ag2SO4(s)
	B. 	is BaSO4(s)
	C. 	is Fe2(SO4)3(s)
	D. 	could be Ag2SO4(s) and/or Fe2(SO4)3(s)
	E. 	could be Ag2SO4(s) and/or BaSO4(s)

 

    Depress mouse to view answer.
   	
		Answer: 	E
	
    
 


102.	A beaker contains a mixture of AgNO3(aq), Ba(NO3)2(aq) and Fe(NO3)3(aq).  Some NaOH(aq) is added and a precipitate forms. The precipitate

	A. 	is AgOH(s)
	B. 	is Ba(OH)2v(s)
	C. 	is Fe(OH)3(s)
	D. 	could be AgOH(s) and/or Fe(OH)3(s)
	E. 	could be Ba(OH)2(s) and/or Fe(OH)3(s)

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


103.	A beaker contains a mixture of NaNO3(aq), Ba(NO3)2(aq) and Pb(NO3)2(aq).  Some KBr(aq) is added and a precipitate forms. The precipitate

	A. 	is NaBr(s)
	B. 	is BaBr2(s)
	C. 	is PbBr2(s)
	D. 	could be BaBr2(s) and/or PbBr2(s)
	E. 	could be NaBr(s) and/or PbBr2(s)

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 


104.	Three separate beakers contain solutions of (1) AgNO3(aq), (2) AlCl3(aq) and (3) Ni(NO3)2(aq).  Some Na2S(aq)  is added to each beaker. A precipitate will form in
	A. 	beaker (1) only.
	B. 	beaker (2) only.
	C. 	beaker (3) only.
	D. 	beakers (2) and (3).
	E. 	all of the beakers.

 

    Depress mouse to view answer.
   	
		Answer: 	E
	
    
 


105.	Which ion should be used to remove the cations Ca2+ and Mg2+ from "hard" water by precipitating
them in a double replacement reaction?
	A. 	CO32-
	B. 	Cl1-
	C. 	NO31-
	D. 	CH3COO1-

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


106.	Aqueous solutions of sodium sulfide and copper (II) chloride are mixed.  Which of the following is correct?
	A. 	NaCl will precipitate.
	B. 	No precipitate forms.
	C. 	Both NaCl and CuS precipitate.
	D. 	CuS will precipitate.

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 

107.	It required 9.76 mL of 0.500 M NaOH to titrate 10.0 mL of HCl.  What was the concentration of the HCl?
	A. 	0.500 M
	B. 	0.976 M
	C. 	1.00 M
	D. 	0.488 M

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


108.	Polar solvents dissolve:
	A. 	only polar solutes.
	B. 	polar and ionic solutes.
	C. 	polar, ionic and non-polar solutes.
	D. 	polar and non-polar solutes.
	E. 	only non-polar solutes.

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


109.	Non-polar solvents dissolve:
	A. 	only polar solutes.
	B. 	polar and ionic solutes.
	C. 	polar, ionic and non-polar solutes.
	D. 	polar and non-polar solutes.
	E. 	only non-polar solutes.

 

    Depress mouse to view answer.
   	
		Answer: 	E
	
    
 


110.	NaCl will dissolve in water because

	A. 	polar solutes dissolve in polar solvents.
	B. 	ionic solutes dissolve in polar solvents.
	C. 	polar solutes dissolve in non-polar solvents.
	D. 	ionic solutes dissolve in non-polar solvents.
	E. 	non-polar solutes dissolve in polar solvents.

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


111.	CaCl2 will dissolve in water because

	A. 	polar solutes dissolve in polar solvents.
	B. 	ionic solutes dissolve in polar solvents.
	C. 	polar solutes dissolve in non-polar solvents.
	D. 	ionic solutes dissolve in non-polar solvents.
	E. 	non-polar solutes dissolve in polar solvents.

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


112.	KNO3 will dissolve in water because

	A. 	polar solutes dissolve in polar solvents.
	B. 	ionic solutes dissolve in polar solvents.
	C. 	polar solutes dissolve in non-polar solvents.
	D. 	ionic solutes dissolve in non-polar solvents.
	E. 	non-polar solutes dissolve in polar solvents.

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


113.	Mg(OH)2 will dissolve in water because

	A. 	polar solutes dissolve in polar solvents.
	B. 	ionic solutes dissolve in polar solvents.
	C. 	polar solutes dissolve in non-polar solvents.
	D. 	ionic solutes dissolve in non-polar solvents.
	E. 	non-polar solutes dissolve in polar solvents.

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


114.	CH3OH will dissolve in water because

	A. 	polar solutes dissolve in polar solvents.
	B. 	ionic solutes dissolve in polar solvents.
	C. 	polar solutes dissolve in non-polar solvents.
	D. 	ionic solutes dissolve in non-polar solvents.
	E. 	non-polar solutes dissolve in polar solvents.

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


115.	C6H12O6 (sugar) will dissolve in water because

	A. 	polar solutes dissolve in polar solvents.
	B. 	ionic solutes dissolve in polar solvents.
	C. 	polar solutes dissolve in non-polar solvents.
	D. 	ionic solutes dissolve in non-polar solvents.
	E. 	non-polar solutes dissolve in polar solvents.

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


116.	CH3OCH3 (ether) will dissolve in water because

	A. 	polar solutes dissolve in polar solvents.
	B. 	ionic solutes dissolve in polar solvents.
	C. 	polar solutes dissolve in non-polar solvents.
	D. 	ionic solutes dissolve in non-polar solvents.
	E. 	non-polar solutes dissolve in polar solvents.

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


117.	CH4 (methane gas) will dissolve in gasoline because

	A. 	polar solutes dissolve in polar solvents.
	B. 	ionic solutes dissolve in polar solvents.
	C. 	polar solutes dissolve in non-polar solvents.
	D. 	ionic solutes dissolve in non-polar solvents.
	E. 	non-polar solutes dissolve in non-polar solvents.

 

    Depress mouse to view answer.
   	
		Answer: 	E
	
    
 


118.	Oil will dissolve in gasoline because

	A. 	polar solutes dissolve in polar solvents.
	B. 	ionic solutes dissolve in polar solvents.
	C. 	polar solutes dissolve in non-polar solvents.
	D. 	ionic solutes dissolve in non-polar solvents.
	E. 	non-polar solutes dissolve in non-polar solvents.

 

    Depress mouse to view answer.
   	
		Answer: 	E
	
    
 


119.	C3H8 (propane) will dissolve in vegetable oil because

	A. 	polar solutes dissolve in polar solvents.
	B. 	ionic solutes dissolve in polar solvents.
	C. 	polar solutes dissolve in non-polar solvents.
	D. 	ionic solutes dissolve in non-polar solvents.
	E. 	non-polar solutes dissolve in non-polar solvents.

 

    Depress mouse to view answer.
   	
		Answer: 	E
	
    
 


120.	Substances that dissolve each other in all proportions are
 
	A. 	saturated.
	B. 	diluted
	C. 	aqueous
	D. 	miscible

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


121.	The notation not characterizing a solution is

	A. 	HCl(g)
	B. 	NaCl(aq)
	C. 	Br2(alcohol)
	D. 	CH3OH(ether)

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


122.	The notation not characterizing a solution is

	A. 	HCl(aq)
	B. 	NaCl(s)
	C. 	Br2(alcohol)
	D. 	CH3OH(ether)

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


123.	The notation not characterizing a solution is

	A. 	Cl2(alcohol)
	B. 	NaCl(aq)
	C. 	Br2(s)
	D. 	CH3OH(ether)

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 


124.	An aqueous solution means
	A. 	an acid has formed
	B. 	a solute has reacted
	C. 	dissociation has taken place
	D. 	the solvent is water

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


125.	A solution is an example of a
	A. 	homogeneous substance
	B. 	homogeneous mixture
	C. 	heterogeneous substance
	D. 	heterogeneous mixture

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


126.	The solvent in the solution Br2(alcohol) is

	A. 	bromine
	B. 	bromide
	C. 	alcohol
	D. 	water

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 


127.	The solute in the solution BaBr2(aq) is

	A. 	bromine
	B. 	barium
	C. 	barium bromide
	D. 	water

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 


128.	The solvent in the solution BaBr2(aq) is

	A. 	bromine
	B. 	barium
	C. 	barium bromide
	D. 	water

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


129.	The solvent in the solution C2H4Br2(ether) is

	A. 	C2H4
	B. 	Br2
	C. 	ether
	D. 	water

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 


130.	The solute in the solution C2H4Br2(ether) is

	A. 	C2H4
	B. 	C2H4Br2
	C. 	ether
	D. 	water

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


131.	A solution in an open beaker is left for a week on the shelf.  The resulting solution is now

	A. 	more concentrated.
	B. 	less concentrated.
	C. 	the same concentration as before.
	D. 	less saturated than before.

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


132.	A solution in an open beaker is heated for 20 minutes on a bunsen flame.  The resulting solution is now

	A. 	more concentrated.
	B. 	less concentrated.
	C. 	the same concentration as before.
	D. 	less saturated than before.

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


133.	A solution in an open beaker contains undissolved crystals in the bottom.   The solution is 

	A. 	saturated
	B. 	concentrated.
	C. 	dilute.
	D. 	supersaturated

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


134.	200 mL of a solution in an open beaker is left on a shelf for a week.  The  beaker contains undissolved crystals in the bottom.  The lab assistant adds water until the new volume is 300 mL and the crystals have disappeared.   After the addition of the water the solution is 

	A. 	still saturated
	B. 	less concentrated.
	C. 	the same concentration as before.
	D. 	more concentrated.

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


135.	A solution in an open beaker contains undissolved crystals in the bottom.  Water is added and about half of the crystals dissolve.  The solution is now

	A. 	unsaturated
	B. 	less concentrated.
	C. 	the same concentration as before.
	D. 	supersaturated

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 


136.	A solution in an open beaker contains undissolved crystals in the bottom.   The solution is heated gently, until the crystals disappear, and then allowed to cool.  The solution is

	A. 	saturated
	B. 	less concentrated.
	C. 	the same concentration as before.
	D. 	supersaturated

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


137.	200 mL of a solution in an open beaker is left on a shelf for a week.  The  beaker now contains undissolved crystals in the bottom.  The lab assistant adds water until the  volume is 200 mL.   The solution is now

	A. 	saturated
	B. 	less concentrated.
	C. 	the same concentration as before.
	D. 	more concentrated.

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 


138.	Which one of the following phrases best describes a solution?

	A. 	a homogeneous substance
	B. 	a heterogeneous liquid
	C. 	a heterogeneous mixture
	D. 	a homogeneous mixture

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


139.	When sodium chloride is completely dissolved in water, the result is properly classified as a

	A. 	colloid
	B. 	liquid
	C. 	plasma
	D. 	solution

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


140.	The main components of the solution known as sea water can correctly be described as

	A. 	water is the solvent and sodium chloride is the solute.
	B. 	water is the solute and sodium chloride is the solvent.
	C. 	water is the solvent and sodium chloride is the saturate.
	D. 	water is the solute and sodium chloride is the insolvent.

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


141.	In a solution containing 20% methanol and 80% ethanol

	A. 	both methanol and ethanol are the solvents.
	B. 	neither methanol nor ethanol can be considered a solute.
	C. 	methanol is the solute and ethanol is the solvent.
	D. 	methanol is the solvent and ethanol is the solute.

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 


142.	As a salt solution is heated in an open beaker for 15 minutes, it will be true that the number of moles of
	A. 	solvent will increase.
	B. 	solvent will not change.
	C. 	solute will not change.
	D. 	solute will decrease.

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 


143.	In a solution containing 60% alcohol and 40% water

	A. 	both alcohol and water are the solvents.
	B. 	both alcohol and water are the solutes.
	C. 	alcohol is the solute and water is the solvent.
	D. 	alcohol is the solvent and water is the solute.

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


144.	The concentration of a solution can properly be described as

	A. 	the strength of a solution.
	B. 	the corrosiveness of a solution.
	C. 	a measure of the ratio of moles of solute to volume of solution.
	D. 	a measure of the moles of solute.

 

    Depress mouse to view answer.
   	
		Answer: 	C
	
    
 


145.	The correct abbreviation for the phrase "concentration of" is

	A. 	conc.
	B. 	c.
	C. 	( )
	D. 	[ ]

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


146.	As a salt solution is heated in an open beaker for 15 minutes, it will become

	A. 	more dilute.
	B. 	more concentrated.
	C. 	less concentrated.
	D. 	less dense.

 

    Depress mouse to view answer.
   	
		Answer: 	B
	
    
 


147.	A dilute solution is best described as
	A. 	many moles of solvent and few moles of solute.
	B. 	many moles of solvent and many moles of solute.
	C. 	few moles of solvent and few moles of solute.
	D. 	few moles of solvent and many moles of solute.

 

    Depress mouse to view answer.
   	
		Answer: 	A
	
    
 


148.	The liquid contents of a flask labeled "barium iodate solution" were tested by addition of solid barium iodate.  None of the added solid dissolved.  Based on this observation, the solution is called

	A. 	dilute.
	B. 	concentrated.
	C. 	unsaturated.
	D. 	saturated.

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


149.	In chemistry, the preferred way to express concentration of solutions is

	A. 	grams of solute per liter of water.
	B. 	grams of water per liter of solution.
	C. 	moles of solute per liter of water.
	D. 	moles of solute per liter of solution.

 

    Depress mouse to view answer.
   	
		Answer: 	D
	
    
 


150.	An example of two miscible substances would be
 
	A. 	sugar and water
	B. 	salt and water
	C. 	alcohol and water
	D. 	oil and water

 

    Depress mouse to view answer.
   	
		Answer: 	C