Question

What volume of a 0.00945-M solution of potassium hydroxicce would be required to titrae 50.00mL of a sample of acid rain with a H2SO4 concentration of 123 x 10-4 M

H2SO4 + 2KOH ? K2SO4 + 2H2O

Answer 1

Answer: The volume of HBr solution required is 130.16 mL

Step-by-step explanation:

To calculate the concentration 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
`H_2SO_4`

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

We are given:

`n_1=2\\M_1=123* 10^(-4)M=0.0123M\\V_1=50mL\\n_2=1\\M_2=0.00945M\\V_2=?mL`

Putting values in above equation, we get:

`2* 0.0123* 50=1* 0.00945* V_2\\\\V_2=130.16mL`

Hence, the volume of KOH solution required is 130.16 mL