Question

when 100 ml Of M /10 H2SO4 is mixed with 500 ml of M/10 NaOH then nature of the resulting solution and normality of excess reaction left is

Answer 1

hope u get my solution

Answer 2

Answer: The resulting solution is basic in nature and normality of the excess reactant left is 0.05 N

Explanation: We are given the molarity of acid and we need to find the normality of the excess reactant, so the relation between normality and molarity is:

Normality = Molarity × Basicity ( For Acid)

Normality = Molarity × Acidity (For base)

We are given Molarity of $H_2SO_4=\frac{M}{10}$

Basicity of $H_2SO_4$ = 2

$\text{Normailty of }H_2SO_4=\frac{1}{10}\times 2=0.2N$

Acidity of NaOH = 1

$\text{Normailty of }NaOH=\frac{1}{10}\times 1=0.1N$

Mili equivalents can be calculated by:

$\text{Mili Equivalents}=Normailty\times Volume(\text{in mL})$     ....(1)

For Acid:

Normailty = 0.2 N

Volume = 100 mL

Mili equivalents = 0.2 × 100 = 20 meq

For Base:

Normality = 0.1 N

Volume = 500 mL

Mili equivalents = 0.1 × 500 = 50 meq

As the mili equivalents of base is more, hence the solution will be basic in nature.

Excess mili equivalents left are = 50 - 20 = 30 meq.

Volume of the solution = 100 + 500 = 600 mL

Normality can be calculated by equation 1, we get

$30=600\times Normality$

Normality = 0.05 N