Question

A chemistry student weighs out 0.154 g of chloroacetic acid (HCH2CICO2) into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1400 M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the equivalence point.

Answer 1

11.6 mL of 0.1400 M of NaOH is required to reach equivalence point.

Step-by-step explanation:

Chloroacetic acid is an monoprotic acid.

Neutralization reaction:
`ClCH_(2)COOH+NaOH\rightleftharpoons ClCH_(2)COONa+H_(2)O`

So, 1 mol of chloroacetic acid is neutralized by 1 mol of NaOH.

Molar mass of chloroacetic acid = 94.5 g/mol

So, 0.154 g of chloroacetic acid =
`(0.154)/(94.5)` moles of chloroacetic acid

= 0.00163 moles of chloroacetic acid

Lets assume V mL of 0.1400 M of NaOH is required to reach equivalence point.

So, number of moles of NaOH needed to reach equivalence point

=
`(0.1400* V)/(1000)` moles

So,
`(0.1400* V)/(1000)=0.00163`

or, V = 11.6

Hence, 11.6 mL of 0.1400 M of NaOH is required to reach equivalence point.