Salt of Weak Acid and Weak Base

Q. The degree of hydrolysis of a salt of a weak acidand a weak base in its 0.1 M solution is found tobe 50%. If the molarity of the solution is 0.2 M, the percentage hydrolysis of the salt should be(2Y 50%(1) 100%(4) 75%(3) 25%ration Cimol ) and

Q. nh4cl is acid but any NH2 is base in liquid ammonia

Q. pH of ${10}^{-8}$ M HCl solution

1. $6.95$
2. $4.75$
3. $7$
4. $8$

Q. When 10 mL of 0.1 M acetic acid $(p{K}_a=5.0)$ is titrated against 10 mL of 0.1 M ammonia solution $(p{K}_b=5.0)$ the equivalence point occurs at pH of:

1. 5
2. 6
3. 7
4. 9

Q. Calculate the degree of hydrolysis $\left(h\right)$ of a salt of aniline and acetic acid in 0.1 M solution at ${25}^{\circ }C$
Given :
$K_a$ for $C{H}_{3}COOH$ is $1.8\times {10}^{-5}$
$K_b$ for aniline is $4.6\times {10}^{-10}$

1. 0.996
2. 0.235
3. 0.85
4. 0.523

Q. $\text{pOH}=7–0.5p{K}_a+0.5p{K}_b$ is true for an aqueous solution that has which pair of cations and anions amongst the following?

1. $C_6{H}_{5}N{H}_3^{+},C{H}_{3}CO{O}^{-}$
2. $N{H}_4^{+},F^{-}$
3. $N{a}^{+},C{H}_{3}CO{O}^{-}$
4. $N{H}_4^{+},C{l}^{-}$

Q. Given the $K_a$ for acetic acid is $1.77\times {10}^{-5}$ and $K_b$ for ammonium hydroxide is $1.82\times {10}^{-5}$.
Calculate the pH of an aqueous solution of ammonium acetate $\left(C{H}_{3}COON{H}_4\right)$ at ${25}^{\circ }C$.

1. 8.115
2. 7.01
3. 7.65
4. 8.05

Q. What will be the $pH$ of an aqueous solution of $0.1M$ ammonium formate ${25}^{o}C$?
$\text{Given :}p{K}_a\left(HCOOH\right)=3.8andp{K}_b\left(N{H}_{4}OH\right)=4.8$

1. 6
2. 6.5
3. 4.5
4. 5.5