Acid Base review
1.
Aspirin is a monoprotic acid with a Ka of 3.27 x 10-4. It dissolves in water by the following:
HC9H7O4 + H2O ↔ C9H7O4- + H3O+
a.
What is the hydronium concentration of the solution at equilibrium if the initial
concentration of aspirin is 1.8 x 10-2 M
b. What is the hydroxide ion concentration at equilibrium
c. What is the pH of the solution at equilibrium
d. How many mL of 0.10 M NaOH would be required to neutralize 325 mg of aspirin
2.
Formic acid (HCO2H) is found in the saliva and bodies of fire ants. The Ka of the acid is 1.8 x 10-4.
a. If the pH of a 1.0 mL solution of formic acid is 2.5, what is the equilibrium concentration of
the solution.
b. What is the initial concentration of the solution
c. How many grams of sodium carbonate would be required to neutralize the solution if it
reacts in a 1:1 ratio
d. What is the % ionization of the acid
3.
You have at your disposal a 0.10 M solution of standard NaOH, and an unknown sample of
H2SO4.
a. What is the concentration of the sulfuric acid, if you titrate 10 mL of the acid with 25 mL of
the standard base?
b. What is the pH of the original sample of sulfuric acid
c. At what pH would you expect the equivalence point to happen for this titration