The pH of a 0.1 M solution of NH_{4}OH (havi | vedclass

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

Question

(C) For a weak base,the concentration of hydroxyl ions is given by $[OH^{-}] = \sqrt{K_{b} 	imes C}$.$[OH^{-}] = \sqrt{1.0 	imes 10^{-5} 	imes 0.1}

Vedclass · Accepted Answer

$11$

Vedclass · Answer

(C) For a weak base,the concentration of hydroxyl ions is given by $[OH^{-}] = \sqrt{K_{b} 	imes C}$.$[OH^{-}] = \sqrt{1.0 	imes 10^{-5} 	imes 0.1} = \sqrt{1.0 	imes 10^{-6}} = 1.0 	imes 10^{-3} \ M$.Using the ionic product of water,$K_{w} = [H^{+}] [OH^{-}] = 1.0 	imes 10^{-14}$.$[H^{+}] = \frac{K_{w}}{[OH^{-}]} = \frac{1.0 	imes 10^{-14}}{1.0 	imes 10^{-3}} = 1.0 	imes 10^{-11} \ M$.The $pH$ is calculated as $pH = -\log [H^{+}]$.$pH = -\log (1.0 	imes 10^{-11}) = 11$.

The $pH$ of a $0.1 \ M$ solution of $NH_{4}OH$ (having $K_{b} = 1.0 \times 10^{-5}$) is equal to

Similar Questions

$pH$ of $0.05 \ M$ aqueous solution of diethyl amine is $10$. The value of equilibrium constant $(K_b)$ is:

When a $1$ deci-normal solution of acetic acid is $1.3\%$ ionized,what is the value of the ionization constant $(K_a)$?

The $pH$ of a $1.0 \ M$ monobasic acid $HX$ is $2$. The van't Hoff factor for the aqueous solution of the acid will be ........

Calculate the dissociation constant of a weak monobasic acid if it is $0.05 \%$ dissociated in a $0.02 \ M$ solution.

The $pH$ of $0.1 \ M$ monobasic acid is $4.50$. Calculate the concentration of species $H^{+}$,$A^{-}$ and $HA$ at equilibrium. Also,determine the value of $K_{a}$ and $pK_{a}$ of the monobasic acid.

Vedclass Test Series

Exam Paper Generator

Online Exam Module