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Chemistry LibreTexts

14.E: Acids and Bases

1.  Fill in the following table:

[H+]

[OH]

pH

pOH

acid, base or neutral?

1.0 x 10-4 M

 

 

 

 

 

1.0 x 10-7 M

 

 

 

 

 

12.0

 

 

 

 

 

14.0

 

 

 

3.5

 

 

4.6 x 10-3 M

 

 

 

 

 

8.2 x 10-12 M

 

 

 

 

2.  For each of the following: classify as acid or base, strong or weak, or amphoteric, and then write a balanced equation for its ionization in water:

  1. HNO3              
  2. HF             
  3. F-              
  4. HSO3-                  
  5. KOH

 

3.  Find the pH of the following solutions:

  1. 0.010 moles HCl in 10.0 liters water.
  2. 6.0 g NaOH dissolved in 15.0 liters water.
  3. 5.0 ml 0.40 M HBr diluted to 20.0 liters with water.
  4. 0.10 M solution of benzoic acid.
  5. 0.20 M NaClO.
  6. 0.20 moles HCl plus 0.10 moles KOH dissolved in 1.0 liter water.

 

4.  The pH of a 0.10 M solution of H2CO3, carbonic acid, is 3.68.

  1. Write an expression for the ionization of the first proton from carbonic acid.
  2. Write an expression for Ka for carbonic acid.
  3. Find the Ka of carbonic acid.
  4. What is Kb for HCO3-?

 

5. 

  1. Why is the acetate ion, CH3COO-, a base according to the Bronsted-Lowry model? 
  2. What is the conjugate acid of CH3COO-?
  3. Write a balanced equation in which CH3COO- acts as a base.

 

6.  Write a balanced net ionic equation for the reaction between solutions of HNO2 and KOH.  Which 2 species are acting as acids?  as bases?

 

7.  List the following acids in order of increasing strength:  HCl, HC2H3O2, HCN, HF.  List the following bases in order of increasing strength:  Cl-, C2H3O2-, CN-, F-.

 

8.  For each of the following solutions, indicate whether it is acidic, basic or neutral:

  1. 0.10 M NaOH             
  2. 0.10 M NH4NO3        
  3. 0.10 M KCl      
  4. 0.10 M NaF

Extra Questions

1.  Calculate the pH of a 0.030 M NH4Cl solution.

 

2.  Calculate the pH of a 0.14 M solution of NaF.

 

3.  Find the pH of the following solution:  6.00 mL of 3.00 M HNO3 diluted to a volume of 18.0 liters with water.

 

4.  Write a balanced net ionic equation for the reaction between NH4+ and NaOH.  What are the conjugate acid/base pairs in this reaction?

 

5.  Which of the following has the highest pH?

  1. 0.10 M NaCl               
  2. 0.10 M HCl           
  3. 0.10 M NaOH       
  4. 0.10 M NaNO2