Honors Chapter 19 Acid/Base Problems 2013-2014
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What are the properties of acids?
What are the properties of bases?
What is a Brønsted-Lowry acid? What is a Brønsted-Lowry base?
Identify each of the following species as a Brønsted acid, base, or both: 𝑎. 𝑃𝑂!!! 𝑏. 𝐶𝑙𝐶𝑙𝑂!! 𝑐. 𝑁𝐻!! 𝑑. 𝐻𝐶𝑂!!
Write a balanced formula equation for the reaction that occurs between each of the following pairs of reactants
a. magnesium and nitric acid
b. aluminum and sulfuric acid
c. calcium carbonate and hydrobromic acid
d. magnesium carbonate and hydrochloric acid
Identify the acid, base, conjugate acid, and conjugate base in the following reactions
a. NH4+(aq) + OH-(aq) ⇆ NH3(aq) + H2O(l)
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CO32-(aq) + H2O(l) ⇆ HCO3-(aq) + OH-(aq)
HSO4-(aq) + H2O(l) ⇆ H3O+(aq) + SO42-(aq)
HCN(aq) + H2O(l) ⇆ H3O+(aq) + CN-(aq)
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What makes a strong acid/base?
What makes a weak acid/base?
Is acid/base strength the same as being concentrated/dilute?
Describe what it means to have a concentrated weak acid.
Describe what it means to have a dilute strong acid.
Write the ionization equation and acid ionization constant (Ka) expressions for the following acids
a. HF
b. HClO2
13. Write the ionization equations and base ionization constant (Kb) expressions for the following bases.
a. hexylamine (C6H13NH2)
b. carbonate ion (CO32-)
c. hydrogen sulfite ion (HSO3-)
14. Draw and label the pH scale.
15. The concentration of either the H+ ion or the OH- ion is given for three aqueous solutions at 298 K. For each solution,
calculate [H+] or [OH-] . State whether the solution is acidic, basic, or neutral
a. [H+] = 1.0 x 10-13 M
b. [OH-] = 3.4 x 10 –11 M
16. Calculate the pH of solutions having the following ion concentrations at 298K
a. [H+] = 1.0 x 10-2 M
b. [OH-] = 2.0 x 10-8 M
17. Calculate the pH and pOH of aqueous solution having the following ion concentrations
a. [OH-] = 1.0 x 10-6 M
b. [H+] = 0.025 M
c. [H+] = 4.67 x 10-4 M
18. The pH is given for these solutions. Calculate pOH, [H+] and [OH-] in each solution.
a. pH = 2.37
b. pH = 11.05
19. The pOH is given for these solutions. Calculate pH, [H+] and [OH-] in each solution.
a. pOH = 3.45
b. pOH = 12.67
20. Calculate the concentration (in Molarity) of a NaOH solution if 25.0 mL of the solution are needed to neutralize 17.4 mL of
a 0.312 M HCl solution.
21. What volume of a 0.500 M HCl solution is needed to neutralize each of the following:
a. 10.0 mL of a 0.300 M NaOH solution
b. 10.0 mL of a 0.200 M Ba(OH)2 solution