When 100 ml of ( M /10) H 2 SO 4 is mixed with 500 ml of ( M /10) NaOH then nature of resulting solution and normality of excess of reactant left is

Question

When 100 ml of ( M /10) H 2 SO 4 is mixed with 500 ml of ( M /10) NaOH then nature of resulting solution and normality of excess of reactant left is (A) Acidic, ( N /5) (B) Basic, (N/5) (C) Basic, ( N /20) (D) Acidic, ( N /10)

Tardigrade Admin · Accepted Answer

[. because N = M × n , n factor of H 2 SO 4=2 ∴ meq of H 2 SO 4=(100 × (1/5))=20 meq

[because N factor is 1] ∴ meq of NaOH =(500 × (1/10))=50 meq For Neutralisation Reaction =( text larger meq - text smaller meq / text Total volume ) =(50-20/600)=(1/20) N NaOH [because larger meq of NaOH will remain] ∴ Solution will be basic

Q. When $100 m l$ of $\frac{M}{10} H_{2} S O_{4}$ is mixed with $500 m l$ of $\frac{M}{10} N a O H$ then nature of resulting solution and normality of excess of reactant left is

Acidic, $\frac{N}{5}$

Basic, $\frac{N}{5}$

Basic, $\frac{N}{20}$

Acidic, $\frac{N}{10}$

Q. When 100ml of 10M​H2​SO4​ is mixed with 500ml of 10M​NaOH then nature of resulting solution and normality of excess of reactant left is

Acidic, 5N​

Basic, 5N​

Basic, 20N​

Acidic, 10N​

Q. When $100 m l$ of $\frac{M}{10} H_{2} S O_{4}$ is mixed with $500 m l$ of $\frac{M}{10} N a O H$ then nature of resulting solution and normality of excess of reactant left is

Acidic, $\frac{N}{5}$

Basic, $\frac{N}{5}$

Basic, $\frac{N}{20}$

Acidic, $\frac{N}{10}$