Hydrolysis of Salts and pH of their Solutions

Which of the following salts will give a basic solution on hydrolysis? 

Which of the following salts with a concentration $0.1\mathrm{M}$ will give a basic solution?

A weak acid is titrated with a weak base. Consider the following statements regarding the $\mathrm{pH}$ of the solution at the equivalence point:
(i) $\mathrm{pH}$ depends on the concentration of acid and base.
(ii) $\mathrm{pH}$ is independent of the concentration of acid and base
(iii) $\mathrm{pH}$ depends on the ${\mathrm{pK}}_{\mathrm{a}}$ of acid and ${\mathrm{pK}}_{\mathrm{b}}$ of base.
(iv) $\mathrm{pH}$ is independent of the ${\mathrm{pK}}_{\mathrm{a}}$ of acid and ${\mathrm{pK}}_{\mathrm{b}}$ of base.
The correct statements are:-

Solution A and B contains respectively $1$ and $2$ moles of ${\mathrm{CH}}_3{\mathrm{COONH}}_4$ in one litre. Then hydrolysis will be;

Which among the following produces a basic aqueous solution?

$2.5 \mathrm{mL}$ of $\frac{2}{5}\mathrm{M}$ weak monoacidic base $({\mathrm{K}}_{\mathrm{b}}=1\times {10}^{-12}$ at ${25}^{\circ }\mathrm{C})$ is titrated with $\frac{2}{15}\mathrm{M} \mathrm{HCl}$ in water at  $25°\mathrm{C}$.  The concentration of $\left[{\mathrm{H}}^{+}\right]$ at equivalence point is $({\mathrm{K}}_{\mathrm{w}} =1\times {10}^{-14}$ at ${25}^{\circ }\mathrm{C})$.

$\mathrm{pH}$, ionization constant ${\mathrm{K}}_{\mathrm{a}}$ and concentration $\mathrm{c}$ of the solution of the salt of a weak acid and strong base (like ${\text{CH}}_3\text{COONa}$) are related as_____.

(A) $\mathrm{pH}=7+\frac{1}{2}\left[{\mathrm{pK}}_{\mathrm{a}}+\mathrm{logc}\right]$

(B) $\mathrm{pH}=7-\frac{1}{2}\left[{\mathrm{pK}}_{\mathrm{a}}+\mathrm{logc}\right]$

(C) $\mathrm{pH}=7-\frac{1}{2}\left[{\mathrm{pK}}_{\mathrm{a}}-\mathrm{logc}\right]$

Enter the correct answer as A, B or C.

Out of which of the following salt , the degree of hydrolysis is independent of the concentration of salt solution - 

If the blood contains ${\mathrm{C}\mathrm{O}}_2$ and ${\mathrm{H}\mathrm{C}\mathrm{O}}_3^{-}$, what is the ratio of conjugate base $\left(HC{O_3}^{-}\right)$ to acid $\left({\mathrm{H}}_2{\mathrm{C}\mathrm{O}}_3\right)$ to maintain the $\mathrm{p}\mathrm{H}$ of the blood equal to 7.4 ?

[Given: $\mathrm{p}{\mathrm{K}}_{{\mathrm{a}}_1\mathrm{ }}$of ${\mathrm{H}}_2{\mathrm{C}\mathrm{O}}_3=\mathrm{6.4]}$

Which of the following pair cannot exist together in solution?

Choose the salt that will not undergo hydrolysis.

What is the $\mathrm{p}\mathrm{H}$ of $0.05\mathrm{ }\mathrm{M}\mathrm{ }{\left({\mathrm{CH}}_3\mathrm{COO}\right)}_2\mathrm{Ca}$?

$\mathrm{HA}$ is a weak acid and $\mathrm{BOH}$ is a weak base. The salt for which the extent of hydrolysis is independent of the concentration of the salt is:

The ionisation constant of $\mathrm{NH}_{4}^{+}$ in water is $5.6 \times 10^{-10} \mathrm{at}$ $25^{\circ} \mathrm{C} .$ The rate constant for the reaction of $\mathrm{NH}_{4}^{+}$ and $\mathrm{OH}^{-}$ to form $\mathrm{NH}_{3}$ and $\mathrm{H}_{2} \mathrm{O}$ at $25^{\circ} \mathrm{C}$ is $3.4 \times 10^{10}$ litre
$\mathrm{mol}^{-1} \mathrm{sec}^{-1} .$ If equilibrium constant of water at $25^{\circ} \mathrm{C}$ is $1.8 \times 10^{-16},$ then

What is the pH of $0.1 \mathrm{M} {\left({\mathrm{NH}}_4\right)}_2{\mathrm{SO}}_4$ solution ? (The hydrolysis constant of ${{\mathrm{NH}}_4}^{+}$ is $5.6\times {10}^{-10}$)

In an experiment 1.2g Mg was burnt in air so that a part of metal was oxidized to MgO and rest to Mg₃N₂ . The residue dissolved in 100 mL H₂O & NH₃ produced not allowed to escape. Assuming negligible solubility of Mg (OH)₂ determine the mass percentage of Mg converted into MgO, the pH of above solution = 11.35, ${\text{K}}_{\text{b}\left({\text{NH}}_3\right)}=2\times 10^{-5.}$

$\mathrm{A}\mathrm{l}\mathrm{C}{\mathrm{l}}_3$ fumes in air because of

Which of the following salts with a concentration $0.1\mathrm{M}$ will give a basic solution?

Which of the following salts will give a basic solution on hydrolysis? 

What is the concentration in $\mathrm{mol}/\mathrm{L}$ of ${\mathrm{CH}}_3\mathrm{COOH}\left(\mathrm{aq}.\right)$ in a solution prepared by dissolving $0.01$ mole of ${\mathrm{NH}}_4^{+}{\mathrm{CH}}_3{\mathrm{COO}}^{-}$ in $1 \mathrm{L} {\mathrm{H}}_2\mathrm{O}?$ Leave your answer in the form of $\mathrm{p}\times {10}^{-6}· \left[{\mathrm{K}}_{\mathrm{a}\left({\mathrm{CH}}_3\mathrm{COOH}\right)}=1.8\times {10}^{-5}; {\mathrm{K}}_{\mathrm{b}\left({\mathrm{NH}}_4\mathrm{OH}\right)}=1.8\times {10}^{-5}\right]$ Calculate the value of p.