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Chemistry Part-I

Equilibrium

The solubility of { Sr( OH ) }_{ 2 } at 298 K is 19.23 g/L o

Chemistry Part-I

Class 11

NCERT

Chapter 1: Some Basic Concepts of Chemistry

44 questions

Chapter 2: Structure of Atom

85 questions

Chapter 3: Classification of Elements and Periodicity in Properties

50 questions

Chapter 4: Chemical Bonding and Molecular Structure

44 questions

Chapter 5: States of Matter

28 questions

Chapter 6: Thermodynamics and Thermochemistry

36 questions

Chapter 7: Equilibrium

101 questions

If 0.561 g of

K O H

is dissolved in water to give 200 mL of solution at 298 K. Calculate the concentrations of potassium, hydrogen and hydroxyl ions. What is its

p H

The solubility of

S r (O H)_{2}

at 298 K is 19.23 g/L of solution. Calculate the concentrations of strontium and hydroxyl ions and the

p H

of the solution.

The ionization constant of propanoic acid is

1.32 \times 10^{- 5}

. Calculate the degree of ionization of the acid in its 0.05 M solution and also its

p H

. What will be its degree of ionization if the solution is 0.01M in

H Cl

View all question

Question

Medium

Solving time: 4 mins

The solubility of $S r (O H)_{2}$ at 298 K is 19.23 g/L of solution. Calculate the concentrations of strontium and hydroxyl ions and the $p H$ of the solution.

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Chemistry Part-I (NCERT)

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The solubility of

S r (O H)_{2}

at 298 K is 19.23 g/L of solution. Calculate the concentrations of strontium and hydroxyl ions and the

p H

of the solution.

5 mins ago

Discuss this question LIVE

5 mins ago

Text solutionVerified

The molecular weight of

S r (O H)_{2}

87.6 + 2 (17) = 121.6

.
The solubility in mol/L is

\frac{19.23}{121.6} = 0.1581 M

S r (O H)_{2} ⇌ S r^{2 +} + 2 O H^{-}

[S r^{2 +}] = 0.1581 M

[O H^{-}] = 2 \times 0.1581 = 0.3162 M

[H^{+}] = \frac{K _{w}}{[ O H ^{-} ]} = \frac{1 0 ^{- 14}}{0.3162} = 3.163 \times 1 0^{- 14}

p H = - l o g [H^{+}] = - l o g (3.163 \times 1 0^{- 14}) = 13.50

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Practice more questions from Chemistry Part-I (NCERT)

If 0.561 g of

K O H

is dissolved in water to give 200 mL of solution at 298 K. Calculate the concentrations of potassium, hydrogen and hydroxyl ions. What is its

p H

The solubility of

S r (O H)_{2}

at 298 K is 19.23 g/L of solution. Calculate the concentrations of strontium and hydroxyl ions and the

p H

of the solution.

The ionization constant of propanoic acid is

1.32 \times 10^{- 5}

. Calculate the degree of ionization of the acid in its 0.05 M solution and also its

p H

. What will be its degree of ionization if the solution is 0.01M in

H Cl

View all

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Question Text	The solubility of $S r (O H)_{2}$ at 298 K is 19.23 g/L of solution. Calculate the concentrations of strontium and hydroxyl ions and the $p H$ of the solution.
Topic	Equilibrium
Subject	Chemistry
Class	Class 11
Answer Type	Text solution:1
Upvotes	60

The solubility of $S r (O H)_{2}$ at 298 K is 19.23 g/L of solution. Calculate the concentrations of strontium and hydroxyl ions and the $p H$ of the solution.

Text solutionVerified

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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.

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The solubility of $S r (O H)_{2}$ at 298 K is 19.23 g/L of solution. Calculate the concentrations of strontium and hydroxyl ions and the $p H$ of the solution.