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

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:

$n_1=2\\M_1=123\times 10^{-4}M=0.0123M\\V_1=50mL\\n_2=1\\M_2=0.00945M\\V_2=?mL$

Putting values in above equation, we get:

$2\times 0.0123\times 50=1\times 0.00945\times V_2\\\\V_2=130.16mL$

Hence, the volume of KOH solution required is 130.16 mL