12th Chemistry Monthly Test - 3 (Ionic Equilibrium)

St. Britto Hr. Sec. School - Madurai

12th Chemistry Monthly Test - 3 (Ionic Equilibrium) -Aug 2020

Time : 2.30 Hours

Part - A

Generic 2 - Answer All Question

Magnesium is not precipitated from a solution of its salt by a mixture of NH₄OH and NH₄Cl. Explain.

Ksp of Ag2Cr04 is 1.1 X 10^-12. what is solubility of Ag₂CrO₄ in 0.1M K₂CrO₄.

Define pH.

BF₃ is termed as an add though it does not contain H⁺ ions. Explain.

When temperature is increased, will ionic product of water increase or decrease? Give reason to justify your answer.

The K_a value for HCN is 10^-9. What is the pH of 0.4 M HCN solution?

Solubility product of Ag₂Cr0₄ is 1 x 10^-12What is the solubility of Ag₂CrO₄ in 0.01 M AgNO₃ solution?

K_sp of Al(OH)₃ is 1 x 10^-15 M. At what pH does 1.0 x 10^-3M AI³⁺ precipitate on the addition of ouffer of NH₄Cl and NH₄OH solution?

Define solubility product.

Account for the acidic nature of HClO₄. In terms of Bronsted- Lowry theory, identify its conjugate base.

K_sp of AgCl is 1.8 x 10^-10. Calculate molar solubility in 1 M AgNO₃

Define ionic product of water. Give its value at room temperature.

Define neutralisation reaction.

The concentration of hydroxide ion in a water sample is found to be 2.5 x 10^-6 M. Identify the nature of the solution.

50 ml of 0.05 M HNO₃ is added to 50 ml of 0.025 M KOH. Calculate the pH of the resultant solution.

A saturated solution, prepared by dissolving CaF₂(s) in water, has [Ca²⁺] = 3.3 x 10^-4 M. What is the K_sp of CaF₂?

Calculate the extent of hydrolysis and the pH of 0.1 M ammonium acetate Given that K_a = K_b = 1.8 x 10^-5.

Calculate the pH of 0.04 M HNO₃ Solution.

Write the expression for the solubility product of Hg₂Cl₂.

Write the expression for the solubility product of Ca₃ (PO₄)₂

Give the Limitations of Arrhenius concept theory of acids and bases.

Will a precipitate be formed when 0.150 L of 0.1 M Pb(NO₃)₂ and 0.100 L of 0.2 M NaCl
are mixed? K_sp (PbCl₂) = 1.2 X 10^-5

Derive an expression for the hydrolysis constant and degree of hydrolysis of salt of strong acid and weak base.

A lab assistant prepared a solution by adding a calculated quantity of HC1 gas 25°C to get a solution with [H₃O⁺] = 4 x 10^-5 M. Is the solution neutral (or) acidic (or) basic.

Derive an expression for Ostwald’s dilution law.

Define Buffer solution.

Part - B

Generic 3 - Answer All Question

Based on Arrhenius concept, define acid and bases and give an example for each.

What do you mean by buffer action?

Define buffer Index.

What do you mean by auto ionisation of water?

For an aqueous solution of NH₄Cl, prove that \(\left[ H^{ + } \right] =\sqrt { { K }_{ a }.C } \)

What is Henderson equation?

Part - C

Generic 5 - Answer All Question

Explain buffer action in an acidic buffer.

Derive Henderson - Hasselbalch equation.

Derive the relationship between pH and pOH.

On hydrolysis of salts of strong acid and strong base, the solution obtained is neutral. Justify your answer with a suitable example.

Derive the hydrolysis constant for the hydrolysis of salt of strong base and weak acid. Deduce its pH.

Derive an expression for the hydrolysis constant for the hydrolysis of salt of weak acid and weak base.

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12th Chemistry Monthly Test - 3 (Ionic Equilibrium)

St. Britto Hr. Sec. School - Madurai

12th Chemistry Monthly Test - 3 (Ionic Equilibrium) -Aug 2020

Part - A

Generic 2 - Answer All Question

Magnesium is not precipitated from a solution of its salt by a mixture of NH4OH and NH4Cl. Explain.

Ksp of Ag2Cr04 is 1.1 X 10-12. what is solubility of Ag2CrO4 in 0.1M K2CrO4.

Define pH.

BF3 is termed as an add though it does not contain H+ ions. Explain.

When temperature is increased, will ionic product of water increase or decrease? Give reason to justify your answer.

The Ka value for HCN is 10-9. What is the pH of 0.4 M HCN solution?

Solubility product of Ag2Cr04 is 1 x 10-12 What is the solubility of Ag2CrO4 in 0.01 M AgNO3 solution?

Ksp of Al(OH)3 is 1 x 10-15 M. At what pH does 1.0 x 10-3 M AI3+ precipitate on the addition of ouffer of NH4Cl and NH4OH solution?

Define solubility product.

Account for the acidic nature of HClO4. In terms of Bronsted- Lowry theory, identify its conjugate base.

Ksp of AgCl is 1.8 x 10-10. Calculate molar solubility in 1 M AgNO3

Define ionic product of water. Give its value at room temperature.

Define neutralisation reaction.

The concentration of hydroxide ion in a water sample is found to be 2.5 x 10-6 M. Identify the nature of the solution.

50 ml of 0.05 M HNO3 is added to 50 ml of 0.025 M KOH. Calculate the pH of the resultant solution.

A saturated solution, prepared by dissolving CaF2(s) in water, has [Ca2+] = 3.3 x 10-4 M. What is the Ksp of CaF2?

Calculate the extent of hydrolysis and the pH of 0.1 M ammonium acetate Given that Ka = Kb = 1.8 x 10-5.

Calculate the pH of 0.04 M HNO3 Solution.

Write the expression for the solubility product of Hg2Cl2.

Write the expression for the solubility product of Ca3 (PO4)2

Give the Limitations of Arrhenius concept theory of acids and bases.

Will a precipitate be formed when 0.150 L of 0.1 M Pb(NO3)2 and 0.100 L of 0.2 M NaCl are mixed? Ksp (PbCl2) = 1.2 X 10-5

Derive an expression for the hydrolysis constant and degree of hydrolysis of salt of strong acid and weak base.

A lab assistant prepared a solution by adding a calculated quantity of HC1 gas 25°C to get a solution with [H3O+] = 4 x 10-5 M. Is the solution neutral (or) acidic (or) basic.

Derive an expression for Ostwald’s dilution law.

Define Buffer solution.

Part - B

Generic 3 - Answer All Question

Based on Arrhenius concept, define acid and bases and give an example for each.

What do you mean by buffer action?

Define buffer Index.

What do you mean by auto ionisation of water?

For an aqueous solution of NH4Cl, prove that \(\left[ H^{ + } \right] =\sqrt { { K }_{ a }.C } \)

What is Henderson equation?

Part - C

Generic 5 - Answer All Question

Explain buffer action in an acidic buffer.

Derive Henderson - Hasselbalch equation.

Derive the relationship between pH and pOH.

On hydrolysis of salts of strong acid and strong base, the solution obtained is neutral. Justify your answer with a suitable example.

Derive the hydrolysis constant for the hydrolysis of salt of strong base and weak acid. Deduce its pH.

Derive an expression for the hydrolysis constant for the hydrolysis of salt of weak acid and weak base.

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Magnesium is not precipitated from a solution of its salt by a mixture of NH₄OH and NH₄Cl. Explain.

Ksp of Ag2Cr04 is 1.1 X 10^-12. what is solubility of Ag₂CrO₄ in 0.1M K₂CrO₄.

BF₃ is termed as an add though it does not contain H⁺ ions. Explain.

The K_a value for HCN is 10^-9. What is the pH of 0.4 M HCN solution?

Solubility product of Ag₂Cr0₄ is 1 x 10^-12What is the solubility of Ag₂CrO₄ in 0.01 M AgNO₃ solution?

K_sp of Al(OH)₃ is 1 x 10^-15 M. At what pH does 1.0 x 10^-3M AI³⁺ precipitate on the addition of ouffer of NH₄Cl and NH₄OH solution?

Account for the acidic nature of HClO₄. In terms of Bronsted- Lowry theory, identify its conjugate base.

K_sp of AgCl is 1.8 x 10^-10. Calculate molar solubility in 1 M AgNO₃

The concentration of hydroxide ion in a water sample is found to be 2.5 x 10^-6 M. Identify the nature of the solution.

50 ml of 0.05 M HNO₃ is added to 50 ml of 0.025 M KOH. Calculate the pH of the resultant solution.

A saturated solution, prepared by dissolving CaF₂(s) in water, has [Ca²⁺] = 3.3 x 10^-4 M. What is the K_sp of CaF₂?

Calculate the extent of hydrolysis and the pH of 0.1 M ammonium acetate Given that K_a = K_b = 1.8 x 10^-5.

Calculate the pH of 0.04 M HNO₃ Solution.

Write the expression for the solubility product of Hg₂Cl₂.

Write the expression for the solubility product of Ca₃ (PO₄)₂

Will a precipitate be formed when 0.150 L of 0.1 M Pb(NO₃)₂ and 0.100 L of 0.2 M NaCl
are mixed? K_sp (PbCl₂) = 1.2 X 10^-5

A lab assistant prepared a solution by adding a calculated quantity of HC1 gas 25°C to get a solution with [H₃O⁺] = 4 x 10^-5 M. Is the solution neutral (or) acidic (or) basic.

For an aqueous solution of NH₄Cl, prove that \(\left[ H^{ + } \right] =\sqrt { { K }_{ a }.C } \)