Equilibrium practice · Mixed difficulty

$\mathrm{pH}$ at which a basic indicator with $K_b=1.0 \times 10^{-10}$ changes colour when the indicator is $10^{-2} \mathrm{M}$ is

In the manufacture of ammonia by Haber’s process,

${\mathrm{N}_2}\left( \mathrm{g} \right) + 3{\mathrm{H}_2}\;\leftrightharpoons\;2\mathrm{N}{\mathrm{H}_3}\left( \mathrm{g} \right) + 92.3\;\mathrm{kJ}$

Which of the following condition is unfavourable?

If ${HCl}$ is added into ${H}_2 {S}$ weak acid, then what will happen:

$4.0$ moles of argon and $5.0$ moles of $\mathrm{PCl}_5$ are introduced into an evacuated flask of 100 litre capacity at $610 \mathrm{~K}$. The system is allowed to equilibrate. At equilibrium, the total pressure of mixture was found to be $6.0 \mathrm{~atm}$. The $\mathrm{K}_p$ for the reaction is [Given : $R=0.082 \mathrm{~L}$ atm $\mathrm{K}^{-1} \mathrm{~mol}^{-1}$ ]

Which of the following will occur if a $0.1 \mathrm{~M}$ solution of a weak acid is diluted to $0.01 \mathrm{~M}$ at constant temperature?

A buffer mixture of acetic acid and potassium acetate has $\mathrm{pH} = 5.24.$ The ratio of $\left[ {\mathrm{C}{\mathrm{H}_3}\mathrm{CO}{\mathrm{O}^ - }} \right]/\left[ {\mathrm{C}{\mathrm{H}_3}\mathrm{COOH}} \right]$ in this buffer is, $\left( {\mathrm{p}{K_a} = 4.74} \right):$

Assertion (A): $\mathrm{N}_2 \mathrm{O}_4(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NO}_2(\mathrm{~g})$ is the example of homogeneous equilibrium.

Reason (R): For this reaction, $\mathrm{K}_{\mathrm{c}}$ has unit $\mathrm{L}$ $\mathrm{mol}$ and $\mathrm{K}_{\mathrm{p}}$ has unit bar.

A weak acid HX has the dissociation constant $1 \times {10^{ - 5}}\;M$. It forms a salt $\mathrm{Na}X$ on reaction with alkali. The degree of hydrolysis of $0.1\;M$ solution of $\mathrm{Na}X$ is

Water in equilibrium with air contains $4.4 \times 10^{-5} \%$ $\mathrm{CO}_2.$ The resulting carbonic acid $\left(\mathrm{H}_2 \mathrm{CO}_3\right)$ gives the solution a hydronium ion concentration of $2.0 \times 10^{-6} \mathrm{M}$ about 20 times greater than that of pure water. What is the $\mathrm{pH}$ of the solution at $298 \, \mathrm{K} ?\, (\log 4.4=0.64, \log 2=0.3)$

A reversible reaction is one which

In which reaction ammonia acts as an acid?

Assertion :- When an acid or a base is added to water at constant temperature the pH changes.

Reason :- This is due to change in ionic product of water.

If the $\mathrm{pH}$ value is 4.5 for a solution then what is the value of $\mathrm{H}^{+}$concentration ?

Consider the following statements.
I) The pH of a mixture containing 400 mL of $\;0.1\;M\;{H_2}S{O_4}$ and 400 mL of $\;0.1\;M\;NaOH$ will be approximately 1.3
II) Ionic product of water is temperature dependent.
III) A monobasic acid with ${K_a} = {10^{ - 5}}$ has a $pH = 5.$ The degree of dissociation of this acid is 50%.
IV) The Le-Chatelier’s principle is not applicable to common-ion effect.
The correct statements are

The ${K_C}$ for ${H_2}(g) + {I_2}(g)2HI(g)$ is 64, if the volume of the container is reduced to one-half of its
original volume, the value of equilibrium constant will be

The most favourable condition for the manufacture of $\mathrm{N}{\mathrm{H}_3}$ is

Assertion (A): When the concentration of any of the reactants or products in a reaction at equilibrium is changed, the composition of the equilibrium mixture changes, so as to minimize the effect of concentration changes.

Reason (R): It illustrates Le-Chatelier's principle on the effect of concentration change.

In a closed tube, $\mathrm{HI}(\mathrm{g})$ is heated at $440^{\circ} \mathrm{C}$ up to establishment of equilibrium. If it dissociates into $\mathrm{H}_2(\mathrm{g})$ and $\mathrm{I}_2(\mathrm{g})$ up to $22 \%,$ then the dissociation constant is

Statement (S): The dissociation constant of water at $60^{\circ} \mathrm{C}$ is $10^{-13}$.

Explanation (E): The $\mathrm{pH}$ of water is 6.5 and that it behaves as acid at $60^{\circ} \mathrm{C}$.

For the equilibrium $A B_{3(\mathrm{g})} \rightleftharpoons 1 / 2 A_{2(\mathrm{g})}+3 / 2 B_{2(\mathrm{g})},$ the value of the equilibrium constant is $3.0 \times 10^{-6}$ at 1000 K. Find $\mathrm{K}_{\mathrm{p}}$ for the reaction at this temperature (given $\mathrm{R}: 8.314 \mathrm{~JK}^{-1} \mathrm{~mol}^{-1})$