The ionization constant of chloroacetic acid is $1.35 \times 10^{-3}$. What will be the pH of 0.1M acid and its 0.1M sodium salt solution?

Classify the following species into Lewis acids and Lewis bases and show how these act as Lewis acid/base: (d) $BCl_3$.

Calculate the pH of the following solutions:
a) 2 g of TlOH dissolved in water to give 2 litre of solution.

Does the number of moles of reaction products increase, decrease or remain same when each of the following equilibria is subjected to a decrease in pressure by increasing the volume?
(c) $3Fe (s) + 4H_2O (g) \rightleftharpoons Fe_3O_4 (s) + 4H_2 (g)$

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

One mole of $H_2O$ and one mole of CO are taken in 10 L vessel and heated to 725 K. At equilibrium 40% of water (by mass) reacts with CO according to the equation,
$H_2O (g) + CO (g) \rightleftharpoons H_2 (g) + CO_2 (g)$
Calculate the equilibrium constant for the reaction.

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 $mol^{-1}$
c) what would be the effect on $K_c$ if (ii) pressure is increased

Classify the following species into Lewis acids and Lewis bases and show how these act as Lewis acid/base: (c) $H^{+}$

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 ?
$2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$

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 $mol^{-1}$
c) what would be the effect on $K_c$ if (i) more $PCl_5$ is added

Bromine monochloride, BrCl decomposes into bromine and chlorine and reaches the equilibrium:
$2BrCl (g) \rightleftharpoons Br_2 (g) + Cl_2 (g)$
for which $K_c= 32$ at 500 K. If initially pure BrCl is present at a concentration of $3.3 \times 10^{-3}$ mol $L^{-1}$, what is its molar concentration in the mixture at equilibrium?

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.

Predict if the solutions of the following salts are neutral, acidic or basic:
NaCl, KBr, NaCN, $NH_4NO_3$, $NaNO_2$ and KF

The concentration of sulphide ion in 0.1M HCl solution saturated with hydrogen sulphide is $1.0 \times 10^{-19}$ M. If 10 mL of this is added to 5 mL of 0.04 M solution of the following: $FeSO_4$, $MnCl_2$, $ZnCl_2$ and $CdCl_2$. in which of these solutions precipitation will take place?

The ionization constant of acetic acid is $1.74 \times 10^{-5}$. Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its pH.

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.

The solubility of $Sr(OH)_2$ at 298 K is 19.23 g/L of solution. Calculate the concentrations of strontium and hydroxyl ions and the pH of the solution.

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.
(i) $COCl_2 (g) \rightleftharpoons CO (g) + Cl_2 (g)$

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

Write the expression for the equilibrium constant, $K_c$ for each of the following reactions:
(v) $I_2 (s) + 5F_2 \rightleftharpoons 2IF_5$