[Solved] Calculate the pH of 0.08M solution of hypochlorous acid, HOCl. The ionization constant of the acid is 2.5×10−5. Determine the percent dissociation of HOCl. - Chemistry Part-I

Name: Video solution 1: [Solved] Calculate the pH of 0.08M solution of hypochlorous acid, HOCl. The ionization constant of the acid is 2.5×10−5. Determine the percent dissociation of HOCl. - Chemistry Part-I
Uploaded: 2022-04-18T06:28:38.000Z
Duration: 6 min
Description: Video solution 1: [Solved] Calculate the pH of 0.08M solution of hypochlorous acid, HOCl. The ionization constant of the acid is 2.5×10−5. Determine the percent dissociation of HOCl. - Chemistry Part-I

Solution HOCl(aq)+H2O (l) ⇌H3O+(aq)+ClO−(aq) Initial concentration (M) 0.0800 Change to reach equilibrium concentration (M) −x+x+x equilibrium concentartion (M) (0.08−x)xx Ka={[H3O+][ClO−]/[HOCl]} =x2/(0.08−x) As x<0.08, therefore 0.08−x≃0.08 x2/0.08=2.5×10−5 x2=2.0×10−6, thus, x=1.41×10−3 [H+]=1.41×10−3M. Therefore, Percent dissociation ={[HOCl]disssocinted /[HOCl]inttial }×100 =1.41×10−3×102/0.08=1.76% pH=−log(1.41×10−3)=2.85

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Chemistry Part-I

Equilibrium

Calculate the {pH} of 0.08 {M} solution of hypochlorous acid,

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

The

pH

0.1 M

monobasic acid is

4.50

. Calculate the concentration of species

H^{+}

A^{-}

and

HA

at equilibrium. Also, determine the value of

K_{α}

and

p K_{a}

of the monobasic acid.

Calculate the

pH

0.08 M

solution of hypochlorous acid,

HOCl

. The ionization constant of the acid is

2.5 \times 1 0^{- 5}

. Determine the percent dissociation of

HOCl

The

pH

0.004 M

hydrazine solution is 9.7. Calculate its ionization constant

K_{b}

and

p K_{b}

View all question

Question

Medium

Solving time: 3 mins

Calculate the $pH$ of $0.08 M$ solution of hypochlorous acid, $HOCl$ . The ionization constant of the acid is $2.5 \times 1 0^{- 5}$ . Determine the percent dissociation of $HOCl$ .

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Updated on: Apr 18, 2022

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Chemistry Part-I (NCERT)

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Elijah Discussed

Calculate the

pH

0.08 M

solution of hypochlorous acid,

HOCl

. The ionization constant of the acid is

2.5 \times 1 0^{- 5}

. Determine the percent dissociation of

HOCl

13 mins ago

Discuss this question LIVE

13 mins ago

Text solutionVerified

Solution

HOCl (aq) + H_{2} O

(l)

⇌ H_{3} O^{+} (aq) + ClO^{-} (aq)

Initial concentration

(M)

0.08 00

Change to reach equilibrium concentration (M)

- x + x + x

equilibrium concentartion (M)

(0.08 - x) x x

K_{a} = {[H_{3} O^{+}] [ClO^{-}] / [HOCl]}

= x^{2} / (0.08 - x)

x < 0.08

, therefore

0.08 - x ≃ 0.08

x^{2} /0.08 = 2.5 \times 1 0^{- 5}

x^{2} = 2.0 \times 1 0^{- 6}

, thus,

x = 1.41 \times 1 0^{- 3}

[H^{+}] = 1.41 \times 1 0^{- 3} M

.
Therefore,
Percent dissociation

= {[HOCl]_{disssocinted} / [HOCl]_{inttial}} \times 100

= 1.41 \times 1 0^{- 3} \times 1 0^{2} /0.08 = 1.76%

pH = - lo g (1.41 \times 1 0^{- 3}) = 2.85

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Practice more questions from Chemistry Part-I (NCERT)

The

pH

0.1 M

monobasic acid is

4.50

. Calculate the concentration of species

H^{+}

A^{-}

and

HA

at equilibrium. Also, determine the value of

K_{α}

and

p K_{a}

of the monobasic acid.

Calculate the

pH

0.08 M

solution of hypochlorous acid,

HOCl

. The ionization constant of the acid is

2.5 \times 1 0^{- 5}

. Determine the percent dissociation of

HOCl

The

pH

0.004 M

hydrazine solution is 9.7. Calculate its ionization constant

K_{b}

and

p K_{b}

View all

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Question Text	Calculate the $pH$ of $0.08 M$ solution of hypochlorous acid, $HOCl$ . The ionization constant of the acid is $2.5 \times 1 0^{- 5}$ . Determine the percent dissociation of $HOCl$ .
Updated On	Apr 18, 2022
Topic	Equilibrium
Subject	Chemistry
Class	Class 11
Answer Type	Text solution:1 Video solution: 1
Upvotes	185
Avg. Video Duration	6 min

Calculate the $pH$ of $0.08 M$ solution of hypochlorous acid, $HOCl$ . The ionization constant of the acid is $2.5 \times 1 0^{- 5}$ . Determine the percent dissociation of $HOCl$ .

Text solutionVerified

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Calculate the pH of 0.08M solution of hypochlorous acid, HOCl. The ionization constant of the acid is 2.5×10−5. Determine the percent dissociation of HOCl.

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Calculate the $pH$ of $0.08 M$ solution of hypochlorous acid, $HOCl$ . The ionization constant of the acid is $2.5 \times 1 0^{- 5}$ . Determine the percent dissociation of $HOCl$ .