Question

What volume of a 0.317 M HBR solution is required to neutralize 18.8mL of a 0.129 M KOH solution?

HBr + KOH ——> KBr + H2O

Answer 1

`\large \boxed{\text{7.65 mL}}`

Step-by-step explanation:

1. Balanced chemical equation.

`\rm HBr + KOH \longrightarrow KBr + H_(2)O`

2. Moles of NaOH

`\text{Moles of NaOH} =\text{ 18.8 mL NaOH} * \frac{\text{0.129 mmol NaOH }}{\text{1 mL NaOH }} = \text{2.425 mmol NaOH }`

3. Moles of HBr

The molar ratio is 1 mmol HBr:1 mmol NaOH

`\text{Moles of HBr}= \text{2.425 mmol NaOH} * \frac{\text{1 mmol HBr}}{\text{1 mmol NaOH}} =\text{2.425 mmol HBr}`

4. Volume of HBr

`V = \text{2.425 mmol HBr}* \frac{\text{1mL HBr}}{\text{0.317 mmol HBr}} = \textbf{7.65 mL HBr}\\\\\text{The reaction requires $\large \boxed{\textbf{7.65 mL HBr}}$}`