Most Important Chemical Equilibrium Quiz Test Online

1) The solubility product (Ksp) is applicable only for substances whose molar concentrations are:

2)

3) In a saturated solution of AB, the molar concentration of A⁺ and B⁻ ions is 1 × 10⁻⁵ M. Find Ksp?

4) Units of equilibrium constant (Kc) for the following reaction:

A​+B​⇌2C

5) A buffer solution is a solution that resists the change in:

6) The pH of an ideal buffer solution is:

7) Which Henderson equation is correct?

8) Which of the following is a basic buffer solution?

9) If ionic product > Ksp, then the solution is:

10) A buffer solution contains equal concentrations of acid (X) and its conjugate base, where the Ka for X is 10⁻³. The pH of the buffer is:

11)

The ionization of BaSO₄ is suppressed by:

12)

If Na₂SO₄ is added to a solution of BaSO₄, BaSO₄ will precipitate due to:

13) The catalyst used in the Haber process is:

14) For an acidic buffer, pH>pKa if:

15) If the ionic product = Ksp, the solution is

16) When CO₂ gas is passed through a saturated solution of calcium carbonate (CaCO₃), the solubility of CaCO₃:

17)

If the temperature is decreased, what will happen to the formation of NH₃, given that the reaction is reversible and exothermic?

18) Buffer action can be explained by:

19) A basic buffer solution can be prepared by mixing:

20) For a sparingly soluble salt AB3, the solubility is "S" mol/dm³. The solubility product (Ksp) is given by:

1) For which of the following equilibrium reactions, K has no units?

2)

What will be the pH of an HCl solution with a concentration of 10⁻² M?

3) Which one of the following bases has the highest Kb value?

4)

The product of ion concentrations in a saturated solution of a sparingly soluble salt at 310 K, each raised to the power of its stoichiometric coefficient, is known as

5)

Which of the following factors influence a reversible chemical reaction based on Le Chatelier’s Principle?

6)

7)

Precipitation takes place when the ionic product of the ions in a solution is:

8) The pH of human blood is:

9)

In the equation Kp = Kc (RT)ⁿ, if Δn > 0, then:

10) What is the relationship between pH and pKa?

11)

Which of the following factors affect the equilibrium position?

12) What is the pH of 0.01 M HCl?

13)

Consider the following reversible reaction:

CH3CH2OH + CH3COOH ⇌ CH3COOCH2CH3 + H2O

The initial concentrations are:

• Ethanol (CH₃CH₂OH) = 1 mol

• Acetic acid (CH₃COOH) = 1 mol

• Ethyl acetate (CH₃COOCH₂CH₃) = 0 mol

• Water (H₂O) = 0 mol

At equilibrium, the concentrations are:

• CH₃CH₂OH = 0.333 mol

• CH₃COOH = 0.333 mol

• CH₃COOCH₂CH₃ = 0.666 mol

• H₂O = 0.666 mol

If 1 mole each of CH₃CH₂OH and CH₃COOH are added, what will be the new equilibrium concentrations?

14)

For maximum yield of NO₂, according to Le Chatelier’s Principle, the reaction:

Δ2NO + O₂ ⇌ 2NO₂        ΔH=−114 kJ/mol

should be carried out at:

15)

The equilibrium constant (Kc) for the reaction N₂(g) + O₂(g) ⇌ 2NO(g) is 4.0 x 10⁻⁴ at a certain temperature. What is the value of Kc for the reaction 2NO(g) ⇌ N₂(g) + O₂(g) at the same temperature?

16) At 25°C, the solubility product constant (Ksp) for the PbSO₄ system is:

17)

The Kc unit for the reaction:

A+3B⇌2C

18) Which of the following is the correct representation for Ksp of BaSO₄?

BaSO₄ ⇌Ba²⁺​ + SO₄²⁻​

19)

If the pKa of formic acid (HCOOH) is 3.75, the pH of an equimolar solution of formic acid and sodium formate is:

20) Human blood has pH of:

1) Ice and water are in equilibrium within a closed system. If the pressure is decreased, the equilibrium will shift:

2) A+B ⇌ C + Heat

As the forward reaction is exothermic, an increase in temperature shifts the equilibrium:

3) Which industrial process is represented by the reaction: N₂ + 3H₂ ⇌ 2NH₃?

4) Which statement is correct regarding the reaction:
2NOCl ⇌ 2NO + Cl₂

5) In a gaseous reaction where the number of moles of reactants and products are the same, the relationship between Kp and Kc is:

6) The pKa values of some acids at room temperature are given below. Which one is the strongest acid?

7) The purification of table salt (NaCl) by passing HCl gas through its saturated aqueous solution is an example of:

8) N2 + 3H2 ⇌ 2NH3 + Heat

The production of NH₃ will be highest at: