Question

What volume (in mL) of 0.51 M H2SO4(aq) solution is necessary to completely react with 103 mL of 0.36 M KOH(aq)

Answer 1

Answer: 36.3 ml

Step-by-step explanation:

According to the neutralization law,

`n_1M_1V_1=n_2M_2V_2`

where,

`n_1` = basicity
`H_2SO_4` = 2

`M_1` = molarity of
`H_2SO_4` solution = 0.51 M

`V_1` = volume of
`H_2SO_4` solution = ?

`n_2` = acidity of
`KOH` = 1

`M_1` = molarity of
`KOH` solution = 0.36 M

`V_1` = volume of
`KOH` solution = 103 ml

Putting in the values we get:

`2* 0.51* V_1=1* 0.36* 103`

`V_1=36.3ml`

Therefore, volume of
`H_2SO_4` required is 36.3 ml