Ionization of Acids and Bases

The $\mathrm{pH}$ of $0.1 \mathrm{M}$ acetic acid solution is closest to [Dissociation constant of the acid, ${\mathrm{K}}_{\mathrm{a}}=1.8\times {10}^{-5}$]

Which of the following equation follows for base ionization constant is expressed in terms of concentration in molarity of various species in equilibrium.

Calculate the concentration of ${\mathrm{A}}^{-}$ ions in the solution of $0.01 \mathrm{M} \mathrm{HA}$.

$\left[{\mathrm{K}}_{\mathrm{a}}=4\times {10}^{-10}\right]$

Ionisation constant of  ${\mathrm{CH}}_3\mathrm{COOH}$ is $1.7\times {10}^{-5}$ and concentration of ${\mathrm{H}}^{+}$ ions is $3.4\times {10}^{-4}$. Then, the initial concentration of ${\mathrm{CH}}_3\mathrm{COOH}$ is 

Which of the following will occur if a $0.1 \mathrm{M}$ solution of a weak acid is diluted to $0.01 \mathrm{M}$ at constant temperature?

The ${\mathrm{K}}_{\mathrm{a}}$ values of formic acid and acetic acid are respectively $1.77\times {10}^{-4}$ and $1.75\times {10}^{-5}$. The ratio of acid strength of $0.1 \mathrm{N}$ acids is

Which of the following is a weak alkali?

The $\mathrm{pH}$ of an aqueous solution of ${10}^{-8}\mathrm{MHCl}$ is

${\mathrm{NH}}_3$ is dissolved in water.

${\mathrm{NH}}_3 + {\mathrm{H}}_2\mathrm{O} \leftrightharpoons {{\mathrm{NH}}_4}^{+}+{\mathrm{OH}}^{-}$

Its base dissociation constant is given by:

Select the weak base from the following:

The increasing order of base strength is

A $0.025 \mathrm{M}$ aqueous solution of a monobasic acid had a freezing point change of $(-0.060)°\mathrm{C}.$ What is the $\mathrm{pKa}$ for the acid? Given that molal depression constant ${\mathrm{K}}_{\mathrm{f}}$ of  ${\mathrm{H}}_2\mathrm{O}$ is $1.86 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}.$

$(\log 2=0.3, \log 3=0.5, \log 4=0.6)$

Arrange in decreasing order of acidity?

(P)  (Q)  (R)  (S) 

The correct order of increasing $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]$ in the following aqueous solution is 

What is the decreasing order of strength of bases? 
${\mathrm{OH}}^{-}, {\mathrm{NH}}_2^{-}, \mathrm{H}-\mathrm{C}\equiv {\mathrm{C}}^{-} \mathrm{and} {\mathrm{CH}}_3-{\mathrm{CH}}_2^{-}$

What will be the $\mathrm{pH}$ of a solution obtained by diluting $1 \mathrm{mL}$ of  $0.10 \mathrm{M}$ weak monoacidic base to $100 \mathrm{mL}$ at constant temperature if the dissocitaion constant of the base is $1\times {10}^{-5}$?

If $1.0 \mathrm{M}$ solution of a weak acid is diluted to $0.1 \mathrm{M}$ at constant temperature, then corresponding consequence is:

Calculate equilibrium constant for weak acid reaction with strong base if weak acid shows ${\mathrm{K}}_{\mathrm{a}}=0.0001$.

Initial pressure of ${\mathrm{AB}}_3\left(\mathrm{g}\right)$  is 800 mm and total pressure at equilibrium is 900 mm of Hg. Calculate the percentage of ${\mathrm{A}\mathrm{B}}_3$ dissociated in the following reaction:

$\mathrm{A}{\mathrm{B}}_3\left(\mathrm{g}\right)\rightleftharpoons \mathrm{A}{\mathrm{B}}_2\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{B}}_2\left(\mathrm{g}\right)$

 

$\text{HF}+{\text{H}}_2\text{O}\stackrel{}{\rightleftharpoons }{\text{H}}_3{\text{O}}^{+}+{\text{F}}^{-}; {\text{K}}_{\text{a}}$ 

${\text{F}}^{-}+{\text{H}}_2\text{O}\stackrel{}{\rightleftharpoons }\text{H}\text{F}+{\text{OH}}^{-}{\text{; K}}_{\text{b}}$. 

The correct relation is: