1
JEE Advanced 2020 Paper 2 Offline
Numerical
+4
-0
An acidified solution of 0.05 M Zn2+ is saturated with 0.1 M H2S. What is the minimum molar concentration (M) of H+ required to prevent the precipitation of ZnS?

Use Ksp(ZnS) = 1.25 $$\times$$ 10$$-$$22 and overall dissociation constant of

H2S, Knet = K1K2 = 1 $$\times$$ 10-21.
2
JEE Advanced 2020 Paper 1 Offline
Numerical
+4
-0
Consider the reaction,

A $$\rightleftharpoons$$ B

at 1000 K. At time t', the temperature of the system was increased to 2000 K and the system was allowed to reach equilibrium. Throughout this experiment the partial pressure of A was maintained at 1 bar. Given, below is the plot of the partial pressure of B with time. What is the ratio of the standard Gibbs energy of the reaction at 1000 K to that at 2000 K?

3
JEE Advanced 2019 Paper 1 Offline
Numerical
+3
-0
For the following reaction, the equilibrium constant Kc at 298 K is 1.6 $$\times$$ 1017.

Fe2+(aq) + S2-(aq) ⇌ FeS(s)

When equal volumes of

0.06 M Fe2+(aq) and 0.2 M S2$$-$$(aq)

solutions are mixed, the equilibrium concentration of Fe2+(aq) is found by Y $$\times$$ 10$$-$$17 M. The value of Y is .................
4
JEE Advanced 2018 Paper 1 Offline
Numerical
+3
-0
The solubility of a salt of weak acid $$(AB)$$ at $$pH\,$$ $$3$$ is $$Y \times {10^{ - 3}}$$ $$mol\,{L^{ - 1}}.$$ The value of $$Y$$ is ________________.

(Given that the value of solubility product of $$AB$$ $$\left( {{K_{sp}}} \right) = 2 \times {10^{ - 10}}$$ and the value of ionization constant of $$HB$$ $$\left( {{K_a}} \right) = 1 \times {10^{ - 8}}$$)