The equilibrium expression, K_c= [CO₂] represents the reaction.

In a closed system
A(S) ⇌ 4 B(g) + 3 C(g)
If partial pressure of C is doubled, then partial pressure of B will be _____.

What effect does a catalyst have on the equilibrium position of a reaction?

A chemist dissolves an excess of BaSO₄ in pure water at 25°C if its K_sp = 1 x 10^-10 what is the concentration of barium in the water?

If in a mixture where Q = k is combined, then what happens?

Explain , why pure liquids and solids can be ignored while writing the equilibrium constant expression?

For an exothermic reaction, what happens to the equilibrium constant if temperature is increased?

Under the conditions is a substance precipitated from its solution?

Why solution of sugar in water does not conduct electricity whereas that of common salt  in water does?

The solubility product of silver bromide is 3.3 x 10^-13 Calculate its solubility.

For the following equilibrium, K_c = \(6.3\times { 10 }^{ 14 }\) at 1000 K  
\(NO(g)+{ O }_{ 3 }(g)\rightleftharpoons NO_{ 2 }(g)+{ O }_{ 2 }(g)\) Both the forward and reverse reactions in the equilibrium are elementary bimolecular reactions. What is K_c , for the reverse reaction?

Write conjugate acid and conjugate base of H₂O?

Give two characteristics of a buffer solution.

Calculate the percentage hydrolysis of sodium acetate in 0.1 M solution at 25^oC assuming the salt to be completely dissociated. K_a = 1.8 x 10^-5. 

The ionization constant of acetic acid is 1.74 × 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.

At 450 K, K_p = 2.0 x 10¹⁰ bar^-1 for the equilibrium reaction:
2SO₂ (g) + O₂ (g) ⇄ 2SO₃ (g)
What is K_c at this temperature?

K_p = 0.04 atm at 899 K for the equilibrium shown below. What is the equilibrium concentration of C₂H₆ when it is placed in a flask at 4.0 atm pressure and allowed to come to equilibrium?
C₂H₆ (g) ⇌ C₂H₄ (g) + H₂(g)

Write the equilibrium constant (K) expression for the following reactions.
(i) Cu₂+(aq) + 2 Ag (s) ⇌ Cu(s) + 2Ag+ (aq)
(ii) 4HCl (g) + O₂(g) ⇌ 2Cl₂ (g) + 2H₂O(g)

Calculate the pH of a buffer which is 0.1 M in acetic acid and 0.15 M in sodium acetate. Given that the ionisation costants of acetic acid is 1.75 x 10^-5. Also calculate the change in pH of the buffer if to 1L of the buffer 1 cc of 1 M NaOH are added.

(i) Point out the differences between ionic product and solubility product.
(ii) The solubility of AgCl in water at 298 K is 1.06 x 10^-5 mole per litre. Calculate its solubility product at this temperature.