Question

A chemist titrates of a hypochlorous acid solution with solution at . Calculate the pH at equivalence. The of hypochlorous acid is . Round your answer to decimal places.

Answer 1

The question is incomplete, here is the complete question:

A chemist titrates 110.0 mL of a 0.2412 M hypochlorous acid (HCIO) solution with 0.0613 M NaOH solution at 25°C. Calculate the pH at equivalence. The pKa of hypochlorous acid is 7.50. Round your answer to 2 decimal places

Answer: The pH of the solution is 10.09

Step-by-step explanation:

To calculate the volume of base, 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
`HClO`

`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=0.2412M\\V_1=110.0mL\\n_2=1\\M_2=0.0613M\\V_2=?mL`

Putting values in above equation, we get:

`1* 0.2412* 110.0=1* 0.0613* V_2\\\\V_2=(1* 0.2412* 110.0)/(1* 0.0613)=432.8mL`

At equivalence, the number of moles of acid is equal to the number of moles of base. Also, the moles of salt which is NaClO will also be the same.

To calculate the number of moles for given molarity, we use the equation:

`\text{Molarity of the solution}=\frac{\text{Moles of solute}* 1000}{\text{Volume of solution (in mL)}}` .....(1)

• For HClO:

Molarity of HClO solution = 0.2412 M

Volume of solution = 110.0 mL

Putting values in equation 1, we get:

`0.2412M=\frac{\text{Moles of HClO}* 1000}{110}\\\\\text{Moles of HClO}=((0.2412* 110))/(1000)=0.026532mol`

• For NaClO:

Moles of NaClO = 0.026532 moles

Volume of solution = [432.8 + 110] mL = 542.8 mL

Putting values in above equation, we get:

`\text{Molarity of NaClO}=(0.026532* 1000)/(542.8)=0.0489M`

To calculate the pH of the solution, we use the equation:

`pH=7+(1)/(2)[pK_a+\log C]`

where,

`pK_a` = negative logarithm of weak acid which is hypochlorous acid = 7.50

C = concentration of the salt = 0.0489 M

Putting values in above equation, we get:

`pH=7+(1)/(2)[7.50+\log (0.0489)]\\\\pH=7+3.09=10.09`

Hence, the pH of the solution is 10.09