Question

1. What is the concentration of a solution of NaOH if it takes 15.98 mL of a 0.15 M solution of HClO4 to neutralize a 10.00 mL sample of the base? Report your answer in molarity. 2. How many mL of 0.2 M HI is needed to neutralize 25 mL of 0.5 M KOH?

Answer 1

Consider the neutralization reaction,

`HClO_4 + OH^(-) rightleftharpoons H_2O + ClO_4^(-)`

One molar equivalent of perchloric acid will neutralize the hydroxide ions dissociated from that salt.

This is easily solved with a simple stoichiometric calculation with the preceding knowledge. Hence,

`15.98"mL" * (0.15"mol")/"L" * 1/(10.00"mL") approx 0.24"M"`

will be concentration of base acid to completely neutralize the reaction.

For your second question, it's just another stoichiometric calculation using the principles above as a foundation. Hence,

`25"mL" * (0.5"mol")/"L" "L"/(0.2"mol") approx 63"mL"`

of `0.2"M"` hydroioidic acid is required to completely neutralize those hydroxide ions that dissociate from that salt.