1. Suppose that you have 0.500 L of each of the following solutions, and an unlimited supply of water.

Question

(Note: C9H7NHBr is a salt containing the ions C9H7NH+ and Br− and C9H7N is quinoline, an organic
base with pKb = 6.24 at 298 K. If you like, you may represent C9H7NH+ as HB+ and C9H7N as B.)
0.104 mol L−1 C9H7NHBr (aq) 0.122 mol L−1 HBr(aq) 0.113 mol L−1 NaOH(aq)
(a) Provide simple instructions for preparing 1.00 L of a buffer solution having pH = 7.00 at
298 K. Focus on preparing the buffer that contains the highest possible concentrations of the active
components. Your instructions should include the volumes of the solutions required.
(b) What is the buffer capacity of the resulting solution? How does this compare with the
buffer capacity of pure water? (The buffer capacity is the number of moles of NaOH that must be
added to 1.0 L of solution to raise the pH by one unit.)

for this particular question do you start off by finding out the limiting reagent? But i am stuck on the part where you have to write the formula for this particular question, please any help would be appreciated

Answer 1

This is a buffer problem and you must use the Henderson-Hasselbalch equation,

The C9H7NHBr is the base.
HBr is the acid.