In its $0.2\,\, M$ solution, an acid ionises to an extent of $60\%$. Its hydrogen ion concentration is.....$M$
In its $0.2\,\, M$ solution, an acid ionises to an extent of $60\%$. Its hydrogen ion concentration is.....$M$
- A
$0.6$
- B
$0.2$
- C
$0.12$
- D
None of these
Similar Questions
Given the two concentration of $HCN (K_a = 10^{-9})$ are $0.1\,M$ and $0.001\,M$ respectively. What will be the ratio of degree of dissociation ?
Given the two concentration of $HCN (K_a = 10^{-9})$ are $0.1\,M$ and $0.001\,M$ respectively. What will be the ratio of degree of dissociation ?
The ionization constant of $HF$, $HCOOH$ and $HCN$ at $298\, K$ are $6.8 \times 10^{-4}, 1.8 \times 10^{-4}$ and $4.8 \times 10^{-9}$ respectively. Calculate the ionization constants of the corresponding conjugate base.
The ionization constant of $HF$, $HCOOH$ and $HCN$ at $298\, K$ are $6.8 \times 10^{-4}, 1.8 \times 10^{-4}$ and $4.8 \times 10^{-9}$ respectively. Calculate the ionization constants of the corresponding conjugate base.
Calculate $pH$ of $0.02$ $mL$ $ClC{H_2}COOH$. Its ${K_a} = 1.36 \times {10^{ - 3}}$ calculate its $pK_{b}$,
Calculate $pH$ of $0.02$ $mL$ $ClC{H_2}COOH$. Its ${K_a} = 1.36 \times {10^{ - 3}}$ calculate its $pK_{b}$,
Derive the equation of ionization constants ${K_a}$ of weak acids $HX$.
Derive the equation of ionization constants ${K_a}$ of weak acids $HX$.
Derive ${K_a} \times {K_b} = {K_w}$ equation.
Derive ${K_a} \times {K_b} = {K_w}$ equation.