Question

A 11.0 mLmL sample of 0.30 MHBrMHBr solution is titrated with 0.16 MNaOHMNaOH. Part A What volume of NaOHNaOH is required to reach the equivalence point? Express the volume to two significant figures and include the appropriate units. nothingnothing

Answer 1

21 mL of NaOH is required.

Step-by-step explanation:

Balanced reaction:
`HBr+NaOH\rightarrow NaBr+H_(2)O`

Number of moles of HBr in 11.0 mL of 0.30 M HBr solution

=
`((0.30)/(1000)* 11.0)` moles = 0.0033 moles

Let's say V mL of 0.16 M NaOH solution is required to reach equivalence point.

So, number of moles of NaOH in V mL of 0.16 M NaOH solution

=
`((0.16)/(1000)* V)` moles = 0.00016V moles

According to balanced equation-

1 mol of HBr is neutralized by 1 mol of NaOH

So, 0.0033 moles of HBr are neutralized by 0.0033 moles of NaOH

Hence,
`0.00016V=0.0033`

`\Rightarrow V=(0.0033)/(0.00016)=21`

So, 21 mL of NaOH is required.