Exam 3B, Spring 2005

1. Complete and balance the following reactions:

a. H₃PO₄(aq) + Sr(OH)₂(s)

b. CH₃CH₂NH₂(aq) + H₂O(l)

c. Fe²⁺(aq) + EDTA^4–(aq)

d. Co(NO₃)₂(aq) + Na₂S(aq)

e. Hydrogen phosphate ion plus chlorite ion

f. V²⁺(aq) + H₂O(l)

g. Cu(CH₃CO₂)(aq) + HCl(aq)

2. Identify if the following ionic salts are acidic or basic in aqueous solution. Show the reaction that defines the acidity or basicity.

a. KHSO₄

b. Fe(NO₃)₃

c. Mg(IO₃)₂

3. A buffer is prepared to be 0.010 M in H₂S and 0.010 M in NaHS.

a. Calculate the pH of the solution, showing all of your work.

b. 1 mL of HCl(g) is added to 1 L of the buffer. Calculate the new pH.

4. Will the solubility in water increase, decrease, or stay the same for the following salts if they are added to a pH = 14 solution? Briefly explain your answer.

a. CaC₂O₄

b. Cr(OH)₃

5. Determine the solubility of lead(II) bromide in a buffer with pH = 11.0.

6. Calculate ΔH° and ΔS° for the reaction of solid silver nitrate with aqueous hydrochloric acid.

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