Question

Equal volumes of 0.250 M acetic acid and water are combined; a 50.0 mL portion of this solution is titrated to the endpoint with 0.125 M NaOH. Calculate the volume of NaOH required to reach the endpoint.

Answer 1

Answer: The volume of NaOH required to reach the endpoint is 100 mL

Step-by-step explanation:

To calculate the volume of NaOH, we use the equation given by neutralization reaction:

`n_1M_1V_1=n_2M_2V_2`

where,

`n_1,M_1\text{ and }V_1` are the n-factor, molarity and volume of acid which is
`CH_3COOH`

`n_2,M_2\text{ and }V_2` are the n-factor, molarity and volume of base which is NaOH.

We are given:

`n_1=1\\M_1=0.250M\\V_1=50.0mL\\n_2=1\\M_2=0.125M\\V_2=?mL`

Putting values in above equation, we get:

`1* 0.250* 50.00=1* 0.125* V_2\\\\V_2=(1* 0.250* 50.0)/(1* 0.125)=100mL`

Hence, the volume of NaOH required to reach the endpoint is 100 mL