Acids and Bases

Practice Test
      
  1.A molecular system that is a dynamic process with two opposing reactions balancing each other is a(n) ___________.  
  a.   chemical equilibrium  
  b.   nonspontaneous reaction  
  c.   spontaneous reaction  
  d.   unreacted set of chemicals.  
      
  2.

Compared to strong acids, weak acids produce __________ ions and conduct electricity __________ efficiently.
 
  a.   fewer, more  
  b.   more, less  
  c.   fewer, less  
  d.   more, more  
      
  3.Which of the following is the formula for nitric acid?

Formula Acid Name
H2SO3 Sulfurous acid
H2SO4 Sulfuric acid


 
  a.   HN  
  b.   HNO2  
  c.   HNO  
  d.   HNO3  
      
  4.What is the name given to a chemical produced in one elementary step and used up in a subsequent elementary step?  
  a.   elementary step  
  b.   reaction mechanism  
  c.   intermediate  
  d.   complex step  
      
  5.How many grams of MgF2 will dissolve in 150 mL of 0.100M NaF solution? Ksp for MgF2 is 6.4 x 10-9.  
  a.   1.0 x 10-5 g  
  b.   4.1 x 10-6 g  
  c.   6.4 x 10-7 g  
  d.   6.0 x 10-6 g  
      
  6.H2SO4 is a ____________.  
  a.   monoprotic acid  
  b.   monoprotic base  
  c.   diprotic base  
  d.   diprotic acid  
      
  7.What is the equilibrium constant expression for the following reaction?

2NH4NO3(s) → 2NH3(g) + 2NO(g) + H2(g) + 2O2(g)
 
  a.   Keq = [NH3]2[NO]2[H2][O2]2  
  b.   Keq = ([NH3]2[NO]2[H2][O2]2)/[NH4NO3]2  
  c.   Keq = ([NH3][NO][H2][O2])/[NH4NO3]  
  d.   Keq = [NH3][NO][H2][O2]  
      
  8.For the reaction, 2SO2(g) + O2(g) → 2SO3(g) + heat, at equilibrium, what will be the effect on the net amount of SO3 present if the temperature of the container is increased?  
  a.   The concentration of SO3 remains the same.  
  b.   The concentration of SO3 increases.  
  c.   This question cannot be answered without knowing the value of Keq.  
  d.   The concentration of SO3 decreases.  
      
  9.A 0.001M solution of HCl is ____________.  
  a.   a dilute acid solution  
  b.   a weak acid solution  
  c.   a concentrated acid solution  
  d.   neutral  
      
  10.For the reaction, 2SO2(g) + O2(g) → 2SO3(g) at equilibrium, what will be the effect on the net amount of SO3 present if the volume of the container is increased?  
  a.   The concentration of SO3 will increase.  
  b.   The concentration of SO3 will decrease.  
  c.   The concentration of SO3 will remain the same.  
  d.   This question cannot be answered without knowing the value of Keq.  
      
  11.What kind of ion is iodide (I-)?  
  a.   polyatomic anion  
  b.   polyatomic cation  
  c.   monatomic anion  
  d.   monatomic cation  
      
  12.A solution of pH = 2.1 would be described as __________.  
  a.   slightly acidic  
  b.   distinctly basic  
  c.   slightly basic  
  d.   distinctly acidic  
      
  13.What is the correct name for H2SO3 in an aqueous solution?  
  a.   hydrosulfuric acid  
  b.   hydrosulfic acid  
  c.   sulfuric acid  
  d.   sulfurous acid  
      
  14.Sulfate (SO42-) is a ____________.  
  a.   monatomic cation  
  b.   polyatomic anion  
  c.   monatomic anion  
  d.   polyatomic cation  
      
  15.What quantity is defined by the change in concentration of a component in a chemical reaction divided by the change in time of the reaction?  
  a.   rate order  
  b.   catalyst  
  c.   specific rate constant  
  d.   instantaneous rate  
      
  16.What is the net ionic equation for the neutralization reaction between HF and KOH?  
  a.   K+ + F- → KF  
  b.   HF + OH- → H2O + F-  
  c.   H+ + KOH → H2O + K+  
  d.   H+ + OH- → H2O  
      
  17.Neutralization is the chemical process in which ____________.  
  a.   sodium ions react with hydroxide ions to form sodium hydroxide  
  b.   hydrogen ions react with chloride ions to form hydrogen chloride  
  c.   hydrogen ions react with hydroxide ions to form water  
  d.   sodium ions react with chloride ions to form sodium chloride  
      
  18.The molar solubility for BaCO3 is 9.0 x 10-5M at 25°C. What is the solubility product constant, Ksp, for BaCO3?  
  a.   8.1 x 10-9  
  b.   4.0 x 10-15  
  c.   1.2 x 10-8  
  d.   5.3 x 10-12  
      
  19.Which of the following is a weak acid?  
  a.   HF  
  b.   HNO3  
  c.   HCl  
  d.   HClO4  
      
  20.Calculate the pH of a solution that has a [OH-] = 2.50 x 10-4M.  
  a.   -3.6  
  b.   3.6  
  c.   0.4  
  d.   10.4  

 
   
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