Chapter 16, Problem 16.90QP

Interpretation Introduction

Interpretation:

$\text{HA}$ and $\text{HB}$ are both weak acids although $\text{HB}$ is the stronger of the two. Will it take a larger volume of a 0.10 M $\text{NaOH}$ solution to neutralize 50.0 mL of 0.10 M $\text{HB}$ than would be needed to neutralize 50.0 mL of 0.10 M $\text{HA}$ has to be explained

Concept Information:

A chemical substance that gives hydrogen ions when dissolved in water is called as acid.  A chemical substance that gives hydroxide ions in solution is called as base.

Neutralisation reaction is a reaction in which acid and base react with reach other to form salt and water.

Irrespective of whether the strong base is reacting with a strong monoprotic acid or a weak monoprotic acid, the same number of moles of acid is required to react with a constant number of moles of base.

To Explain:

Whether a larger volume of a 0.10 M $\text{NaOH}$ solution is needed to neutralize 50.0 mL of 0.10 M $\text{HB}$ than would be needed to neutralize 50.0 mL of 0.10 M $\text{HA}$