1. Consider two solutions: one of .5 M hydrobromic acid and one of .75 M sodium
hydroxide.
a) Find the pH of each solution.
b) Each solution has a volume of 2.5 Liters. Calculate the number of moles of
each solute in the corresponding solutions.
c) The two solutions are combined. Find a chemical equation representing the
reaction that occurs and balance it.
d) Find the pH of the new solution.
e) If the hydrobromic acid solution was replaced with a hydrofluoric acid
solution of the same molarity, would the calculations in part d) still be valid?
Explain.
2. Consider a .000095 M solution of sulfuric acid.
a) Draw a Lewis Structure for sulfuric acid. Indicate the atom(s) in the molecule
that make it acidic.
b) Find the pH of the solution.
c) The solution has 56.78 grams of sulfuric acid. How much water should be
added to the solution to dilute it to a pH of 4?
3. This question involves a strong-acid + strong-base titration. The acid and analyte
is a solution of .6 M hydrochloric acid. The base and titrant is a solution of .4 M
rubidium hydroxide.
a) Find the pH of the hydrochloric acid solution.
b) Find the pOH of the original rubidium hydroxide solution.
c) Write out a balanced chemical equation showing the reaction that will proceed
if the titration goes through.
d) The initial acidic solution has a volume of 100 milliliters. You have an excess
supply of the rubidium hydroxide solution. If the burette can expel a solution
at a maximum rate of 1.8 milliliters per second, how long will it take to
completely neutralize the acid?
e) Sketch the titration curve for this reaction.