Equilibrium practice · Mixed difficulty

$\mathrm{H}_2 \mathrm{~S}$ is passed into $1 \mathrm{~dm}^3$ of a solution containing 0.1 mole of $\mathrm{Zn}^{2+}$ and 0.01 mole of the $\mathrm{Cu}^{2+}$ till the sulphide ion concentration reaches $8.1 \times 10^{-19}$ mole. Which one of the following statements is true? [ $K_{\mathrm{sp}}$ of Zns and CuS are $3 \times 10^{-22}$ and $8 \times 10^{-36}$, respectively].

Which of the following statement is correct?

pH of a $0.0001\;\mathrm{ }M\;\mathrm{ }HCl$ solution is

$\Delta G^{\circ}$ at $25^{\circ} \mathrm{C}$ for the reaction $\frac{1}{2} \mathrm{N}_2(\mathrm{g})+\frac{3}{2} \mathrm{H}_2(\mathrm{g}) \rightleftharpoons \mathrm{NH}_3(\mathrm{g})$ is $-16.5 \mathrm{~kJ} \mathrm{~mol}^{-1}.$ Hence, thermodynamic equilibrium constant is

$A\left( \mathrm{g} \right) + B\left( \mathrm{g} \right)\;\leftrightharpoons\;AB\left( \mathrm{g} \right)$ is a reversible reaction. At equilibrium 0.4 mole of $AB$ is formed when each $A$ and $B$ are taken one mole. How much of $A$ changes into $AB$?

Which among the following is an electron deficient compound?

Given below are two statements one is labelled as Assertion A and the other is labelled as Reason R:
Assertion A: The amphoteric nature of water is explained by using Lewis acid/base concept
Reason R: Water acts as an acid with $N{H_3}$ and as a base with ${H_2}S.$
In the light of the above statements choose the correct answer from the options given below:

Calculate the percentage ionization of $0.01 \mathrm{~M}$ acetic acid in $0.1 \mathrm{~M} {~HCl} {~K}_{{a}}$ of acetic acid is $1.8 \times 10^{-5}$

The equilibrium constants for the reaction,

$\begin{aligned} & \mathrm{Zn}(s)+\mathrm{Cu}^{2+}(a q) \rightleftharpoons \mathrm{Zn}^{2+}(a q)+\mathrm{Cu}(s) \text { and } \\ & \mathrm{Cu}(s)+2 \mathrm{Ag}^{+}(a q) \rightleftharpoons \mathrm{Cu}^{2+}(a q)+2 \mathrm{Ag}(s) \end{aligned}$

are $K_1$ and $K_2$ respectively. The equilibrium constant for the combined reaction is

If acetic acid is mixed with sodium acetate then ${\mathrm{H}^ + }$ ion concentration will

The following equilibrium constants were determined at $1120 {~K}$ :
$\begin{aligned} & 2 {CO}(g) \rightleftharpoons {C}({s})+{CO}_2({~g}) ; K_{p_1} =10^{-14} {~atm}^{-1} \\ & {CO}(g)+{Cl}_2(g) \rightleftharpoons {COCl}_2({~g}) ; K_{p_2} =6 \times 10^{-3} {~atm}^{-1} \end{aligned}$
What is the equilibrium constant $K_c$ for the following reaction at $1120 {~K}$ :
${C}({s})+{CO}_2({~g})+2 {Cl}_2({~g}) \rightleftharpoons 2 {COCl}_2({~g})$

One litre of an aqueous solution contain 0.15 moles of $C{H_3}COOH\left( {pka = 4.8} \right)$ and 1.5 mole of $C{H_3}COONa$ . The pH of solution is:

Assertion(A) ${BF}_3$ is a Lewis acid as well as Bronsted-Lowry acid.

Reason(R) Any species which can accept a lone pair of electrons is a Lewis acid and the species that can lose a proton is Bronsted-Lowry acid.

Maximum possible $\mathrm{pH}$ of a solution of slaked lime is $\left[\mathrm{K}_{\mathrm{SP}}\right.$ of $\left.\mathrm{Ca}(\mathrm{OH})_2=32 \times 10^{-6}\right]$:

The $\mathrm{pH}$ of $10^{-11} \mathrm{~M} {~HCl}$ at $25^{\circ} \mathrm{C}$ is

Given,
$\mathrm{H}_2 \mathrm{~S}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(l)\rightleftharpoons\mathrm{H}_3 \mathrm{O}^{+}(\mathrm{aq})+\mathrm{HS}^{-}(\mathrm{aq})$; $K=9.1 \times 10^{-8}$ and for
$\mathrm{FeS}(s)+\mathrm{H}_2 \mathrm{O}(l)\rightleftharpoons\mathrm{Fe}^{2+}(\mathrm{aq})+\mathrm{HS}^{-}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq}) ;$ $K=5 \times 10^{-19}$
Thus, molar solubility of $\mathrm{FeS}(s)$ in a buffer solution of $\mathrm{pH}=3.0$ in which $\left[\mathrm{H}_2 \mathrm{~S}\right]$ is fixed at $0.1 \mathrm{M}$, is

Solution of $0.1 \mathrm{~M} \mathrm{~NH}_4 \mathrm{OH}$ and $0.1 \mathrm{~M} \mathrm{~NH}_4 \mathrm{Cl}$ has $\mathrm{pH} ~9.25$, The $\mathrm{pK}_{\mathrm{b}}$ of $\mathrm{NH}_4 \mathrm{OH}$ is;

A vessel at 1000 K contains $\mathrm{C}{\mathrm{O}_2}$ with a pressure of 0.5 atm. Some of the $\mathrm{C}{\mathrm{O}_2}$ is converted into $\mathrm{CO}$ on the addition of graphite. If the total pressure at equilibrium is 0.8 atm, the value of ${K_p}$ is

Assertion(A) ${CaO}$ donates oxide, hence it is a base and ${CO}_2$ accepts an oxide, hence it is an acid. This is in accordance with Lux-Flood concept.

Reason(R) ${Cu}^{+}, {Ag}^{+}, {Au}^{+}$, etc., are soft acids while ${Li}^{+}, {Na}^{+}, {Ca}^{+}$, etc., are hard acids.

$\Delta G^{\circ}$ for the reaction $\mathrm{X}+\mathrm{Y} \rightleftharpoons \mathrm{C}$ is $-4.606 \mathrm{~kcal}$ at $1000 \mathrm{~K}.$ The equilibrium constant for the reverse mode of the reaction is

(A): In presence of dilute ${HCl}, {Zn}^{2+}$ is not precipitated by $S^{2-}$ ions

(R): The dissociation of ${H_2}S$ is suppressed by addition of dilute $HCl$.

The following reactions are known to occur in the body,

$\mathrm{C}{\mathrm{O}_2} + {\mathrm{H}_2}\mathrm{O}\leftrightharpoons{\mathrm{H}_2}\mathrm{C}{\mathrm{O}_3}\leftrightharpoons{\mathrm{H}^ + } + \mathrm{HCO}_3^ -$

If $\mathrm{C}{\mathrm{O}_2}$ escapes from the system, then:

The hydrolysis constant for $\mathrm{ZnCl}_2$ will be

Where, ${K}_{\mathrm{b}}$ is effective dissociation constant of base $\mathrm{Zn}^{++}$

Statement (S): Hydrolysis of salt is an exothermic phenomenon.

Explanation (E): It involves breaking up of water molecule of produce acid and base respectively.

Calculate the concentration of hydrogen ion in the acidic solution with $\mathrm{pH}=$ 4.3

At $1000 \mathrm{~K}$, pressure of $\mathrm{CO}_2$ in equilibrium with $\mathrm{CaCO}_3$ and $\mathrm{CaO}$ is equal to $2.105 \mathrm{~atm}$. The equilibrium constant for the reaction,
$\mathrm{C}(s)+\mathrm{CO}_2(g) \rightleftharpoons 2 \mathrm{CO}(g)$
is 1.9 at the same temperature when pressure are in atm. Solid $\mathrm{C}, \mathrm{CaO}$, and $\mathrm{CaCO}_3$ are mixed and allowed to come to equilibrium at $1000 \mathrm{~K}$ in a closed vessel. What is the pressure of $\mathrm{CO}(\mathrm{g})$ at equilibrium (in $\mathrm{atm}$ )?

Given the reaction between 2 gases represented by ${A_2}$ and ${B_2}$ to give the compound $A{B_{\left( \mathrm{g} \right)}}\mathrm{.}$
${A_{2\left( \mathrm{g} \right)}} + {B_{2\left( \mathrm{g} \right)}}\;\leftrightharpoons\;2A{B_{\left( \mathrm{g} \right)}}$
At equilibrium, the concentration
of ${A_2} = 3.0 \times {10^{ - 3}}\;\mathrm{M}$
of ${B_2} = 4.2 \times {10^{ - 3}}\;\mathrm{M}$
of $AB = 2.8 \times {10^{ - 3}}\;\mathrm{M}$
If the reaction takes place in a sealed vessel at $527^\circ C$, then the value of ${K_c}$ will be :

For the reaction ${N}_2(\mathrm{g})+{O}_2(\mathrm{g}) \rightleftharpoons 2 {NO}(\mathrm{g})$, the value of ${K}_{{C}}$ at $800^{\circ} \mathrm{C}$ is $0.1.$ What is the value of ${K}_{{P}}$ at this temperature?

On doubling ${P}$ and ${V}$ with constant temperature the equilibrium constant will

Which one of the following statements is not true?