What is [{H^ + }] of a solution that is 0.01, | vedclass

Name: PDF Generator App | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(d) ${K_a} = \frac{{[{H^ + }]\,\,[C{N^ - }]}}{{[HC{N^ - }]}}$

$6.2 	imes {10^{ - 10}} = \frac{{[{H^ + }]\,\,[0.02]}}{{[0.01]}}$

$[{H^ + }] = \f

Vedclass · Accepted Answer

$3.1 	imes {10^{ - 10}}$

Vedclass · Answer

(d) ${K_a} = \frac{{[{H^ + }]\,\,[C{N^ - }]}}{{[HC{N^ - }]}}$

$6.2 	imes {10^{ - 10}} = \frac{{[{H^ + }]\,\,[0.02]}}{{[0.01]}}$

$[{H^ + }] = \frac{{6.2 	imes {{10}^{ - 10}} 	imes 0.01}}{{0.02}} = 3.1 	imes {10^{ - 10}}$

What is $[{H^ + }]$ of a solution that is $0.01\,M$ in $HCN$ and $0.02\,M$ in $NaCN$ $({K_a}$for $HCN = 6.2 \times {10^{ - 10}})$

Similar Questions

Ionisation constant of $CH_3COOH$ is $1.7 \times 10^{-5}$ and concentration of $H^+$ ions is $3.4 \times 10^{-4}$. Then find out initial concentration of $CH_3COOH$ Molecules

Explain ionization and ionization constant in di and polyprotic acid.

The $pH$ of $0.004 \,M$ hydrazine solution is $9.7 .$ Calculate its ionization constant $K_{ b }$ and $pK _{ b }$

The concentration of $[{H^ + }]$ and concentration of $[O{H^ - }]$ of a $ 0.1$ aqueous solution of $2\%$ ionised weak acid is [Ionic product of water $ = 1 \times {10^{ - 14}}]$

For a concentrated solution of a weak electrolyte ( $K _{ eq }=$ equilibrium constant) $A _2 B _3$ of concentration ' $c$ ', the degree of dissociation " $\alpha$ ' is