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11th
Chemistry
Equilibrium
$More About Ionization of Acids and Bases$

More About Ionization of Acids and Bases

Equilibrium

Chemistry

Class 11

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pH of very Dilute Acids or Alkali Solutions

32 mins

Ka for Polyprotic Acids

14 mins

Common ion Effect

14 mins

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Ionisation Constant and pH of Weak Acids And Bases

3 mins read

Ka for Polyprotic Acids

2 mins read

Common Ion Effect

3 mins read

Revise with Concepts

Polyacidic bases and polybasic acids

ExampleDefinitionsFormulaes

Common Ion Effect

ExampleDefinitionsFormulaes

Strength of Acids

ExampleDefinitionsFormulaes

The solubility of $A g I$ in $N a I$ solutions is less than that in pure water because:

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Explain the following:
(i) Hydrolysis of ester (ethyl acetate) begins slowly but becomes fast after sometime.
(ii) The pH value of acetic acid increases on addition of a few drops of sodium acetate.

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The solubility of $A_{2} X_{5}$ is $x m o l d m^{- 3}$ . Its solubility product is:

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The solubility of $H g I_{2}$ in water decreases in presence of $K I$ .

State whether the given statement is true or false.

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The following reaction occurs in a beaker: $A g^{+} (a q) + C l^{-} (a q) \to A g C l (s)$ . If a solution of sodium chloride were added to this beaker,

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The weak acid, $H A$ has a $K_{a}$ of $1.00 \times 10^{- 5}$ . If $0.1$ mol of this acid is dissolved in one litre of water, the percentage of acid dissociated at equilibrium is closet to:

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$p H$ of a solution produced when aqueous solution of $p H = 6$ is mixed with an equal volume of an aqueous solution of $p H = 3$ is about:

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The solubility of $A g C l$ in $N a C l$ solution is less than that in pure water, because of the ________.

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The solubility product of $B a S O_{4}$ is $1.5 \times 10^{- 9}$ . Find out the solubility in (i) pure water and (ii) $0.1 M$ $B a C l_{2}$ solution.

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$0.02 M$ solution of $N H_{4} O H$ is $3$ % dissociated. Calculate the dissociation constant of $N H_{4} O H$ .

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More topics

Equilibrium: Basic Definitions Equilibrium in Physical Processes Equilibrium in Chemical Processes Law of Chemical Equilibrium and Equilibrium Constant Homogeneous and Heterogeneous Equilibria Applications of Equilibrium Constants Relationship between Equilibrium Constant, Reaction Quotient and Gibbs Energy Factors Affecting Equilibria Ionic Equilibrium in Solution Acids, Bases and Salts Ionization of Acids and Bases More About Ionization of Acids and Bases Hydrolysis of Salts and the pH of their Solutions Buffer Solutions Solubility Equilibria

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More About Ionization of Acids and Bases

Overview

Learn

Videos

Quick summary with Stories

Ionisation Constant and pH of Weak Acids And Bases

Ka for Polyprotic Acids

Common Ion Effect

Revise with Concepts

Polyacidic bases and polybasic acids

Common Ion Effect

Strength of Acids

Related questions

The solubility of AgI in NaI solutions is less than that in pure water because:

Explain the following: (i) Hydrolysis of ester (ethyl acetate) begins slowly but becomes fast after sometime. (ii) The pH value of acetic acid increases on addition of a few drops of sodium acetate.

The solubility of A2​X5​ is x mol dm−3. Its solubility product is:

The solubility of HgI2​ in water decreases in presence of KI. State whether the given statement is true or false.

The following reaction occurs in a beaker: Ag+(aq)+Cl−(aq)→AgCl(s). If a solution of sodium chloride were added to this beaker,

The weak acid, HA has a Ka​ of 1.00×10−5. If 0.1 mol of this acid is dissolved in one litre of water, the percentage of acid dissociated at equilibrium is closet to:

pH of a solution produced when aqueous solution of pH=6 is mixed with an equal volume of an aqueous solution of pH=3 is about:

The solubility of AgCl in NaCl solution is less than that in pure water, because of the ________.

The solubility product of BaSO4​ is 1.5×10−9. Find out the solubility in (i) pure water and (ii) 0.1M BaCl2​ solution.

0.02M solution of NH4​OH is 3% dissociated. Calculate the dissociation constant of NH4​OH.

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The solubility of $A g I$ in $N a I$ solutions is less than that in pure water because:

Explain the following:
(i) Hydrolysis of ester (ethyl acetate) begins slowly but becomes fast after sometime.
(ii) The pH value of acetic acid increases on addition of a few drops of sodium acetate.

The solubility of $A_{2} X_{5}$ is $x m o l d m^{- 3}$ . Its solubility product is:

The solubility of $H g I_{2}$ in water decreases in presence of $K I$ .

State whether the given statement is true or false.

The following reaction occurs in a beaker: $A g^{+} (a q) + C l^{-} (a q) \to A g C l (s)$ . If a solution of sodium chloride were added to this beaker,

The weak acid, $H A$ has a $K_{a}$ of $1.00 \times 10^{- 5}$ . If $0.1$ mol of this acid is dissolved in one litre of water, the percentage of acid dissociated at equilibrium is closet to:

$p H$ of a solution produced when aqueous solution of $p H = 6$ is mixed with an equal volume of an aqueous solution of $p H = 3$ is about:

The solubility of $A g C l$ in $N a C l$ solution is less than that in pure water, because of the ________.

The solubility product of $B a S O_{4}$ is $1.5 \times 10^{- 9}$ . Find out the solubility in (i) pure water and (ii) $0.1 M$ $B a C l_{2}$ solution.

$0.02 M$ solution of $N H_{4} O H$ is $3$ % dissociated. Calculate the dissociation constant of $N H_{4} O H$ .