Question 1: Palette 1/9

JEE Advanced 2023 MCQ

On decreasing the $p \mathrm{H}$ from 7 to 2 , the solubility of a sparingly soluble salt (MX) of a weak acid (HX) increased from $10^{-4} \mathrm{~mol} \mathrm{~L}^{-1}$ to $10^{-3} \mathrm{~mol} \mathrm{~L}^{-1}$. The $p \mathrm{~K}_{\mathrm{a}}$ of $\mathrm{HX}$ is

A

3

B

4

C

5

D

2

Question 2: Palette 2/9

JEE Advanced 2018 MCQ

Dilution processes of different aqueous solutions, with water, are given in LIST - I. The effects of dilution of the solutions on $\left[ {{H^ + }} \right]$ are given in LIST - II

(Note: Degree of dissociation (a) of weak acid and weak base is $<<1;$ degree of hydrolysis of salt $<<1;$ $\left[ {{H^ + }} \right]$ represents the concentration of ${H^ + }$ ions)

	LIST-I		LIST-II
P.	(10 mL of 0.1 M NaOH + 20 mL of 0.1 M acetic acid) diluted to 60 mL	1.	the value of [H+] does not change on dilution
Q.	(20 mL of 0.1 M NaOH + 20 mL of 0.1 M acetic acid) diluted to 80 mL	2.	the value of [H+] changes to half of its initial value on dilution
R.	(20 mL of 0.1 M HCL + 20 mL of 0.1 M ammonia solution) diluted to 80 mL	3.	the value of [H+] changes to two times of its initial value on dilution
S.	10 mL saturated solution of Ni(OH)2 in equilibrium with excess solid Ni(OH)2 is diluted to 20 mL (solid Ni(OH)2 is still present after dilution).	4.	the value of [H+] changes to ${1 \over {\sqrt 2 }}$ times of its initial value on dilution
		5.	the value of [H+] changes to $\sqrt 2 $ times of its initial value on dilution

Match each process given in LIST-I with one or more effect(s) in LIST-II. The correct option is :

A

$P - 4;Q - 2;R - 3;S - 1$

B

$P - 4;Q - 3;R - 2;S - 3$

C

$P - 1;Q - 4;R - 5;S - 3$

D

$P - 1;Q - 5;R - 4;S - 1$

Question 3: Palette 3/9

JEE Advanced 2015 MCQ

Paragraph
When 100 mL of 1.0 M HCl was mixed with 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7^o C was measured for the beaker and its contents (Expt. 1). Because the enthalpy of neutralization of a strong acid with a strong base is constant (-57.0 kJ/mol), this experiment could be used to measure the calorimeter constant. In a second experiment (Expt. 2) 100 mL of 2.0 M acetic acid (K_a = 2.0 $\times$ 10^-5) was mixed with 100 mL of 1.0 M NaOH (under identical conditions to Expt. 1) where a temperature rise of 5.6^o C was measured. (Consider heat capacity of all solutions as 4.2 J/gK and density of all solutions as 1.0 g m/L)
Question
Enthalpy of dissociation (in kJ/mol) of acetic acid obtained from the Expt. 2 is

A

1.0

B

10.0

C

24.5

D

51.4

Question 4: Palette 4/9

JEE Advanced 2015 MCQ

Paragraph
When 100 mL of 1.0 M KCl was mixed with 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7^o C was measured for the beaker and its contents (Expt. 1). Because the enthalpy of neutralization of a strong acid with a strong base is constant (-57.0 kJ/mol), this experiment could be used to measure the calorimeter constant. In a second experiment (Expt. 2) 100 mL of 2.0 M acetic acid (K_a = 2.0 $\times$ 10^-5) was mixed with 100 mL of 1.0 M NaOH (under identical conditions to Expt. 1) where a temperature rise of 5.6^o C was measured. (Consider heat capacity of all solutions as 4.2 J/gK and density of all solutions as 1.0 g m/L)
Question
The pH of the solution after Expt. 2 is

A

2.8

B

4.7

C

5.0

D

7.0

Question 5: Palette 5/9

JEE Advanced 2013 MCQ

The K_sp of Ag₂CrO₄ is 1.1 $\times$ 10^-12 at 298 K. The solubility (in mol/L) of Ag₂CrO₄ in a 0.1 M AgNO₃ solution is

A

1.1 $\times$ 10^-11

B

1.1 $\times$ 10^-10

C

1.1 $\times$ 10^-12

D

1.1 $\times$ 10^-9

Question 6: Palette 6/9

JEE Advanced 2013 MCQ

The initial rate of hydrolysis of methyl acetate (1M) by a weak acid (HA, 1M) is 1/100^th of that of a strong acid (HX, 1M), at 25^oC. The K_a of HA is

A

1 $\times$ 10^-4

B

1 $\times$ 10^-5

C

1 $\times$ 10^-6

D

1 $\times$ 10^-3

Question 7: Palette 7/9

JEE Advanced 2010 MSQ

Aqueous solution of HNO₃, KOH and CH₃COOH and CH₃COONa of identical concentrations are provided. The pairs of solutions which form a buffer upon mixing is(are)

A

HNO₃ and CH₃COOH

B

KOH and CH₃COONa

C

HNO₃ and CH₃COONa

D

CH₃COOH and CH₃COONa

Question 8: Palette 8/9

JEE Advanced 2008 MCQ

Solubility product constants (K$_{sp}$) of salts of types MX, MX$_2$ and M$_3$X at temperature T are 4.0 $\times$ 10$^{-8}$, 3.2 $\times$ 10$^{-14}$ and 2.7 $\times$ 10$^{-15}$, respectively. Solubilities (mol dm$^{-3}$) of the salts at temperature 'T' are in the order:

A

MX > MX$_2$ > M$_3$X

B

M$_3$X > MX$_2$ > MX

C

MX$_2$ > M$_3$X > MX

D

MX > M$_3$X > MX$_2$

Question 9: Palette 9/9

JEE Advanced 2008 MCQ

2.5 mL of $\frac{2}{5}$M weak monoacidic base (K$_b$ = 1 $\times$ 10$^{-12}$ at 25$^\circ$C) is titrated with $\frac{2}{15}$M HCl in water at 25$^\circ$C. The concentration of H$^+$ at equivalence point is (K$_w$ = 1 $\times$ 10$^{-14}$ at 25$^\circ$C).

A

3.7 $\times$ 10$^{-13}$ M

B

3.2 $\times$ 10$^{-7}$ M

C

3.2 $\times$ 10$^{-2}$ M

D

2.7 $\times$ 10$^{-2}$ M