Ionization of Weak Acids and Weak Bases

Explain the reason for the smaller value of higher order ionization constants than the lower order ionization constant of polyacidic bases.

Define polyacidic bases and give some examples.

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 is a weak alkali?

Define the degree of dissociation of electrolytes.

What is common ion effect? Write an example.

${\mathrm{NH}}_3$ 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? 
${\mathrm{OH}}^{-}, {\mathrm{NH}}_2^{-}, \mathrm{H}-\mathrm{C}\equiv {\mathrm{C}}^{-} \mathrm{and} {\mathrm{CH}}_3-{\mathrm{CH}}_2^{-}$

The relation between $\mathrm{p}\text{H}, \mathrm{p}{\text{K}}_{\mathrm{a}}$ and concentration $\mathrm{c}$ of the solution of a weak acid can be written as _____.

(A) $\mathrm{pH}=\frac{1}{2}\left({\mathrm{pK}}_{\mathrm{a}}-\mathrm{logc}\right)$

(B) $\mathrm{pH}=\frac{1}{2}\left({\mathrm{pK}}_{\mathrm{a}}+\mathrm{logc}\right)$

(C) $\mathrm{pH}=\left({\mathrm{pK}}_{\mathrm{a}}-\mathrm{logc}\right)$

Enter the correct answer as A, B or C.

If ${\mathrm{K}}_{\mathrm{a}}$ is the ionization constant of a weak acid and ${\mathrm{K}}_{\mathrm{b}}$ is that of the conjugate base, then ${\mathrm{pK}}_{\mathrm{a}}+{\mathrm{pK}}_{\mathrm{b}}=2\mathrm{Y}$. If the value of ionic product of water is $1.0\times {10}^{-14}$ then the value of $\mathrm{Y}=$_____.

If the acid-base reaction $\mathrm{HA}\left(\mathrm{aq}\right)+{\mathrm{B}}^{-}\left(\mathrm{aq}\right)\rightleftharpoons \mathrm{HB}\left(\mathrm{aq}\right)+{\mathrm{A}}^{-}\left(\mathrm{aq}\right)$ has a ${\mathrm{K}}_{\mathrm{eq}}={10}^{-4}$ , then is the given statement  correct or incorrect?

 ${\mathrm{A}}^{-}$ is stronger base than ${\mathrm{B}}^{-}$.

If the acid-base reaction $\mathrm{HA}\left(\mathrm{aq}\right)+{\mathrm{B}}^{-}\left(\mathrm{aq}\right)\rightleftharpoons \mathrm{HB}\left(\mathrm{aq}\right)+{\mathrm{A}}^{-}\left(\mathrm{aq}\right)$ has a ${\mathrm{K}}_{\mathrm{eq}}={10}^{-4}$  then the given statement is correct or incorrect?

${\mathrm{B}}^{-}$ is stronger acid than ${\mathrm{A}}^{-}$.

If the acid-base reaction ${\mathrm{HA}}_{\left(\mathrm{aq}\right)}+{{\mathrm{B}}^{-}}_{\left(\mathrm{aq}\right)}\rightleftharpoons {\mathrm{HB}}_{\left(\mathrm{aq}\right)}+{{\mathrm{A}}^{-}}_{\left(\mathrm{aq}\right)}$ has a ${\mathrm{K}}_{\mathrm{eq}}={10}^{-4}$, which of the following statements are true?

(i)  $\mathrm{HA}$ is more acidic than $\mathrm{HB}$.

(ii) $\mathrm{HB}$ is more acidic than $\mathrm{HA}$.

(iii) $\mathrm{HA}$ and $\mathrm{HB}$ have the same acidity.

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 $1\times {10}^{-5}$?

$100 ml$ aqueous $0.1 molar$ $M{\left(CN\right)}_2$ ($80 \%$ ionized) solution is mixed with $100 ml$ of $0.05 molar$ $H_{2}S{O}_4$ solution ($80 \%$ ionized) are mixed. What is the $pH$ of the resultant solution at ${25}^{o}C$ ? $(K_{b}ofC{N}^{-}={10}^{-6})$