Given that, Ka( HCN )=4.9 × 10-10, Ka( HNO 2)=4.5 × 10-4 Thus, which of the following reaction is favoured in forward direction?

Question

Given that, Ka( HCN )=4.9 × 10-10, Ka( HNO 2)=4.5 × 10-4 Thus, which of the following reaction is favoured in forward direction? (A) NO 2-( aq )+ HCl ( aq ) leftharpoons HNO 2( aq )+ CN -( aq ) (B) HNO 2( aq )+ CN -( aq ) leftharpoons NO 2-( aq )+ HCN ( aq ) (C) Both are favoured in forward direction (D) None is favoured in forward direction

Tardigrade Admin · Accepted Answer

Ka( HNO 2)> Ka( HCN ) Larger the value of Ka, stronger is the acid. Thus, HNO 2 is stronger acid than HCN . NO 2- is a weaker base than CN-. HNO 2 is better proton donor and CN- is better proton acceptor. Thus, (b) is favoured in forward side (in which weaker acid and weaker base are formed).

Q. Given that, $K_{a} (H CN) = 4.9 \times 1 0^{- 10}, K_{a} (H N O_{2}) = 4.5 \times 1 0^{- 4}$ Thus, which of the following reaction is favoured in forward direction?

$N O_{2}^{-} (a q) + H Cl (a q) ⇌ H N O_{2} (a q) + C N^{-} (a q)$

$H N O_{2} (a q) + C N^{-} (a q) ⇌ N O_{2}^{-} (a q) + H CN (a q)$

Both are favoured in forward direction

None is favoured in forward direction

Q. Given that, Ka​(HCN)=4.9×10−10,Ka​(HNO2​)=4.5×10−4 Thus, which of the following reaction is favoured in forward direction?

NO2−​(aq)+HCl(aq)⇌HNO2​(aq)+CN−(aq)

HNO2​(aq)+CN−(aq)⇌NO2−​(aq)+HCN(aq)

Both are favoured in forward direction

None is favoured in forward direction

Q. Given that, $K_{a} (H CN) = 4.9 \times 1 0^{- 10}, K_{a} (H N O_{2}) = 4.5 \times 1 0^{- 4}$ Thus, which of the following reaction is favoured in forward direction?

$N O_{2}^{-} (a q) + H Cl (a q) ⇌ H N O_{2} (a q) + C N^{-} (a q)$

$H N O_{2} (a q) + C N^{-} (a q) ⇌ N O_{2}^{-} (a q) + H CN (a q)$