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

Answer:

21 mL of NaOH is required.

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

= $(\frac{0.30}{1000}\times 11.0)$ 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

= $(\frac{0.16}{1000}\times V)$ 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, $0.00016V=0.0033$

           $\Rightarrow V=\frac{0.0033}{0.00016}=21$

So, 21 mL of NaOH is required.