Acids and Bases - LCPS



Acids and Bases Worksheet

1. At the equivalence point in a titration, what is true of moles of acid vs. moles of base?

2. Label the following substances as strong electrolyte, weak electrolyte or non-electrolyte:

a. BaCl2 (aq) b. HF (aq) c. KOH (aq) d. C6H12O6 (aq) e. HNO3 (aq) f. PbCl2 (s)

3. In each of the following chemical equations, identify the conjugate acid-base pairs.

a. HSO4- + H2O ( SO42- + H3O+

b. CH3NH2 + HCl ( CH3NH3+ + Cl-

c. CH3COO- + H2O ( CH3COOH + OH-

Complete the equation for each of the following conjugate acid-conjugate base reactions.

4. HNO2 + H2O ( H3O+ + NO2-

5. HBrO4 + H2O ( H3O+ + BrO4-

6. Write the conjugate acid for each of the following:

a. HPO42- _________ c. HS- _________

b. NO2- _________ d. S2- _________

7. Write the conjugate base for each of the following:

a. HNO3 _________ c. H3O+ _________

b. HPO42- _________ d. H2CO3 _________

8. Calculate the [H+] in each of the following solutions, and indicate whether the solution is acidic, basic, or neutral.

a. [OH-] = 3.99 x 10-5 M b. [OH-] = 7.23 x 10-2 M

9. Calculate the [OH-] in each of the following solutions, and indicate whether the solution is acidic, basic, or neutral.

a. [H+] = 1.27 x 10-3 M b. [H+] = 3.87 x 10-5 M

10. For each pair of concentrations, tell which represents the more basic solution.

a. [H+] = 1.21 x 10-8 M or [OH-] = 0.10 M

b. [H+] = 0.00100 M or [OH-] = 1.78 x 10-13 M

c. [H+] = 4.23 x 10-6 M or [OH-] = 1.15 x 10-7 M

11. Calculate the pH corresponding to each of the hydrogen ion concentrations given below. Tell whether each solution is acidic, basic, or neutral.

a. [H+] = 0.00100 M b. [H+] = 9.18 x 10-11 M

12. Calculate the pH corresponding to each of the hydroxide ion concentrations given below. Tell whether each solution is acidic, basic, or neutral.

a. [OH-] = 4.22 x 10-3 M b. [OH-] = 0.000100 M

13. Calculate the pOH corresponding to each of the pH values listed, and indicate whether each solution is acidic, basic, or neutral.

a. pH = 6.49 b. pH = 11.21

14. Calculate the hydrogen ion concentration, in moles per liter, for solutions with each of the following pH values.

a. pH = 4.11 b. pH = 7.00

15. Calculate the hydrogen ion concentration, in moles per liter, for solutions with each of the following pOH values.

a. pOH = 3.91 b. pOH = 1.15

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