Please show me how to solve this problem, step by step.
0.50 molar solutions of the following weak acids HOCL and NaOCL are available. What volume in mL of a 1.00 molar NaOH solution should be added to 1.00 L of the above acid solution to create a buffer with a pH of 7.16?
Ka = 3.5 x 10-8, Pka = 7.46
For buffer questions, you have to know about frozen equilibria.
When a buffer is made, the equilibrium is frozen, at least the concentrations of the weak acid and conjugate base will not change.
So we use
Ka = [H+] x moles of b/moles of a
Where Ka is 3.5 x 10-8
moles of b/moles of a ...
This provides a step by step explanation for how to solve a buffer solution problem.