The ionization constant of phenol is $1.0 \times 10^{-10}$. What is the concentration of phenolate ion in 0.05 M solution of phenol? What will be its degree of ionization if the solution is also 0.01M in sodium phenolate?

Reaction between $N_2$ and $O_2$ takes place as follows:
$2N_2 (g) + O_2 (g) \rightleftharpoons 2N_2O (g)$
If a mixture of 0.482 mol $N_2$ and 0.933 mol of $O_2$ is placed in a 10 L reaction vessel and allowed to form $N_2O$ at a temperature for which $K_c= 2.0 \times 10^{-37}$, determine the composition of equilibrium mixture.

Which of the following reactions will get affected by increasing the pressure? Also, mention whether change will cause the reaction to go into forward or backward direction.
(iv) $2H_2 (g) + CO (g) \rightleftharpoons CH_3OH (g)$

Determine the solubilities of silver chromate, barium chromate, ferric hydroxide, lead chloride and mercurous iodide at 298K from their solubility product constants given in Table 6.9. Determine also the molarities of individual ions.

What will be the conjugate bases for the Brönsted acids: HF, $H_2SO_4$ and $HCO_3^{-}$?

The ionization constant of propanoic acid is $1.32 \times 10^{-5}$. Calculate the degree of ionization of the acid in its 0.05M solution and also its pH. What will be its degree of ionization if the solution is 0.01M in HCl also?

What is the equilibrium concentration of each of the substances in the equilibrium when the initial concentration of ICl was 0.78 M ?
$2ICl (g) \rightleftharpoons I_2 (g) + Cl_2 (g)$; $K_c = 0.14$

The ionization constant of HF, HCOOH and HCN at 298K are $6.8 \times 10^{-4}$, $1.8 \times 10^{-4}$ and $4.8 \times 10^{-9}$ respectively. Calculate the ionization constants of the corresponding conjugate base.

Describe the effect of:
d) removal of $CH_3OH$
on the equilibrium of the reaction:
$2H_2(g) + CO (g) \rightleftharpoons CH_3OH (g)$

Which of the following reactions will get affected by increasing the pressure? Also, mention whether change will cause the reaction to go into forward or backward direction.
(iii) $CO_2 (g) + C (s) \rightleftharpoons 2CO (g)$

At 700 K, equilibrium constant for the reaction:
$H_2 (g) + I_2 (g) \rightleftharpoons 2HI (g)$
is 54.8. If 0.5 mol $L^{-1}$ of $HI(g)$ is present at equilibrium at 700 K, what are the concentration of $H_2(g)$ and $I_2(g)$ assuming that we initially started with $HI(g)$ and allowed it to reach equilibrium at 700K?

The pH of 0.1M solution of cyanic acid (HCNO) is 2.34. Calculate the ionization constant of the acid and its degree of ionization in the solution.

What is the pH of 0.001M aniline solution? The ionization constant of aniline can be taken from Table 6.7. Calculate the degree of ionization of aniline in the solution. Also calculate the ionization constant of the conjugate acid of aniline.

At 450K, $K_p= 2.0 \times 10^{10}/bar$ for the given reaction at equilibrium.
$2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3 (g)$
What is $K_c$ at this temperature ?

A liquid is in equilibrium with its vapour in a sealed container at a fixed temperature. The volume of the container is suddenly increased.
c) What happens when equilibrium is restored finally and what will be the final vapour pressure?

One of the reaction that takes place in producing steel from iron ore is the reduction of iron(II) oxide by carbon monoxide to give iron metal and $CO_2$.
$FeO (s) + CO (g) \rightleftharpoons Fe (s) + CO_2 (g)$; $K_p = 0.265$ atm at 1050K
What are the equilibrium partial pressures of CO and $CO_2$ at 1050 K if the initial partial pressures are: $p_{CO}$= 1.4 atm and $p_{CO_2}$ = 0.80 atm?

If 0.561 g of KOH is dissolved in water to give 200 mL of solution at 298 K. Calculate the concentrations of potassium, hydrogen and hydroxyl ions. What is its pH?

Predict which of the following reaction will have appreciable concentration of reactants and products:
a) $Cl_2 (g) \rightleftharpoons 2Cl (g) \quad K_c = 5 \times 10^{-39}$

At 473 K, equilibrium constant $K_c$ for decomposition of phosphorus pentachloride, $PCl_5$ is $8.3 \times 10^{-3}$. If decomposition is depicted as,
$PCl_5 (g) \rightleftharpoons PCl_3 (g) + Cl_2 (g)$ $\Delta_r H^{\circ} = 124.0$ kJ $mol^{-1}$
a) write an expression for $K_c$ for the reaction.

What is $K_c$ for the following equilibrium when the equilibrium concentration of each substance is: $[SO_2]$= 0.60M, $[O_2]$ = 0.82M and $[SO_3]$ = 1.90M ?
$2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$