(a) Interpretation: From the given K a values, p K a of weak acids should be calculated. Concept introduction: The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium. For a general reaction of ionization of weak acid as follows: HA ⇌ H + + A − The expression for dissociation constant of the reaction is as follows: K a = [ H + ] [ A − ] [ HA ] The p K a of a weak acid is defined as negative log of K a or, p K = − log K a

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Answer 1

Question

Chapter 13, Problem 36QAP

Interpretation Introduction

(a)

Interpretation:

From the given Ka values, pKa of weak acids should be calculated.

Concept introduction:

The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.

For a general reaction of ionization of weak acid as follows:

HA⇌H++A−

The expression for dissociation constant of the reaction is as follows:

Ka=[H+][A−][HA]

The pKa of a weak acid is defined as negative log of Ka or,

pK=−logKa

Interpretation Introduction

(b)

Interpretation:

From the given Ka values, pKa of weak acids should be calculated.

Concept introduction:

The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.

For a general reaction of ionization of weak acid as follows:

HA⇌H++A−

The expression for dissociation constant of the reaction is as follows:

Ka=[H+][A−][HA]

The pKa of a weak acid is defined as negative log of Ka or,

pK=−logKa

Interpretation Introduction

(c)

Interpretation:

From the given Ka values, pKa of weak acids should be calculated.

Concept introduction:

The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.

For a general reaction of ionization of weak acid as follows:

HA⇌H++A−

The expression for dissociation constant of the reaction is as follows:

Ka=[H+][A−][HA]

The pKa of a weak acid is defined as negative log of Ka or,

pK=−logKa

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C 5 4 3 CI 2 the Righ B A 5 4 3 The Lich. OH 10 4 5 3 1 LOOP- -147.52 T 77.17 -45.36 200 190 180 170 160 150 140 130 120 110 100 90 80 70 60 50 40 30 20 10 ppm B -126.25 77.03 200 190 180 170 160 150 140 130 120 110 100 90 80 70 60 50 40 30 20 10 ppm 200 190 180 170 160 150 140 130 120 110 100 90 80 TO LL <-50.00 70 60 50 40 30 20 10 ppm 45.06 30.18 -26.45 22.36 --0.00 45.07 7.5 1.93 2.05 -30.24 -22.36 C A 7 8 5 ° 4 3 7.5 7.0 6.5 6.0 5.5 5.0 4.5 4.0 3.5 3.0 2.5 2.0 1.5 1.0 ppm 9 8 5 4 3 ཡི་ OH 10 2 7.5 7.0 6.5 6.0 5.5 5.0 4.5 4.0 3.5 3.0 2.5 2.0 1.5 5 4 3 2 that th 7 I 7.0 6.5 6.0 5.5 5.0 4.5 4.0 3.5 3.0 2.5 2.0 1.5 115 2.21 4.00 1.0 ppm 6.96 2.76 5.01 1.0 ppm 6.30 1.00

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Answer 2

Question

Chapter 13, Problem 36QAP

Interpretation Introduction

(a)

Interpretation:

From the given Ka values, pKa of weak acids should be calculated.

Concept introduction:

The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.

For a general reaction of ionization of weak acid as follows:

HA⇌H++A−

The expression for dissociation constant of the reaction is as follows:

Ka=[H+][A−][HA]

The pKa of a weak acid is defined as negative log of Ka or,

pK=−logKa

Interpretation Introduction

(b)

Interpretation:

From the given Ka values, pKa of weak acids should be calculated.

Concept introduction:

The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.

For a general reaction of ionization of weak acid as follows:

HA⇌H++A−

The expression for dissociation constant of the reaction is as follows:

Ka=[H+][A−][HA]

The pKa of a weak acid is defined as negative log of Ka or,

pK=−logKa

Interpretation Introduction

(c)

Interpretation:

From the given Ka values, pKa of weak acids should be calculated.

Concept introduction:

The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.

For a general reaction of ionization of weak acid as follows:

HA⇌H++A−

The expression for dissociation constant of the reaction is as follows:

Ka=[H+][A−][HA]

The pKa of a weak acid is defined as negative log of Ka or,

pK=−logKa

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Answer 3

Question

Chapter 13, Problem 36QAP

Interpretation Introduction

(a)

Interpretation:

From the given Ka values, pKa of weak acids should be calculated.

Concept introduction:

The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.

For a general reaction of ionization of weak acid as follows:

HA⇌H++A−

The expression for dissociation constant of the reaction is as follows:

Ka=[H+][A−][HA]

The pKa of a weak acid is defined as negative log of Ka or,

pK=−logKa

Interpretation Introduction

(b)

Interpretation:

From the given Ka values, pKa of weak acids should be calculated.

Concept introduction:

The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.

For a general reaction of ionization of weak acid as follows:

HA⇌H++A−

The expression for dissociation constant of the reaction is as follows:

Ka=[H+][A−][HA]

The pKa of a weak acid is defined as negative log of Ka or,

pK=−logKa

Interpretation Introduction

(c)

Interpretation:

From the given Ka values, pKa of weak acids should be calculated.

Concept introduction:

The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.

For a general reaction of ionization of weak acid as follows:

HA⇌H++A−

The expression for dissociation constant of the reaction is as follows:

Ka=[H+][A−][HA]

The pKa of a weak acid is defined as negative log of Ka or,

pK=−logKa

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Answer 4

Question

Chapter 13, Problem 36QAP

Interpretation Introduction

(a)

Interpretation:

From the given Ka values, pKa of weak acids should be calculated.

Concept introduction:

The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.

For a general reaction of ionization of weak acid as follows:

HA⇌H++A−

The expression for dissociation constant of the reaction is as follows:

Ka=[H+][A−][HA]

The pKa of a weak acid is defined as negative log of Ka or,

pK=−logKa

Interpretation Introduction

(b)

Interpretation:

From the given Ka values, pKa of weak acids should be calculated.

Concept introduction:

The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.

For a general reaction of ionization of weak acid as follows:

HA⇌H++A−

The expression for dissociation constant of the reaction is as follows:

Ka=[H+][A−][HA]

The pKa of a weak acid is defined as negative log of Ka or,

pK=−logKa

Interpretation Introduction

(c)

Interpretation:

From the given Ka values, pKa of weak acids should be calculated.

Concept introduction:

The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.

For a general reaction of ionization of weak acid as follows:

HA⇌H++A−

The expression for dissociation constant of the reaction is as follows:

Ka=[H+][A−][HA]

The pKa of a weak acid is defined as negative log of Ka or,

pK=−logKa

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Answer 5

Chapter 13, Problem 36QAP

Interpretation Introduction

(a)

Interpretation:

From the given Ka values, pKa of weak acids should be calculated.

Concept introduction:

The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.

For a general reaction of ionization of weak acid as follows:

HA⇌H++A−

The expression for dissociation constant of the reaction is as follows:

Ka=[H+][A−][HA]

The pKa of a weak acid is defined as negative log of Ka or,

pK=−logKa

Interpretation Introduction

(b)

Interpretation:

From the given Ka values, pKa of weak acids should be calculated.

Concept introduction:

The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.

For a general reaction of ionization of weak acid as follows:

HA⇌H++A−

The expression for dissociation constant of the reaction is as follows:

Ka=[H+][A−][HA]

The pKa of a weak acid is defined as negative log of Ka or,

pK=−logKa

Interpretation Introduction

(c)

Interpretation:

From the given Ka values, pKa of weak acids should be calculated.

Concept introduction:

The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.

For a general reaction of ionization of weak acid as follows:

HA⇌H++A−

The expression for dissociation constant of the reaction is as follows:

Ka=[H+][A−][HA]

The pKa of a weak acid is defined as negative log of Ka or,

pK=−logKa

Answer 6

Chapter 13, Problem 36QAP

Interpretation Introduction

(a)

Interpretation:

From the given Ka values, pKa of weak acids should be calculated.

Concept introduction:

The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.

For a general reaction of ionization of weak acid as follows:

HA⇌H++A−

The expression for dissociation constant of the reaction is as follows:

Ka=[H+][A−][HA]

The pKa of a weak acid is defined as negative log of Ka or,

pK=−logKa

Answer 7

Chapter 13, Problem 36QAP

Interpretation Introduction

(a)

Interpretation:

From the given Ka values, pKa of weak acids should be calculated.

Concept introduction:

The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.

For a general reaction of ionization of weak acid as follows:

HA⇌H++A−

The expression for dissociation constant of the reaction is as follows:

Ka=[H+][A−][HA]

The pKa of a weak acid is defined as negative log of Ka or,

pK=−logKa

Answer 8

Interpretation Introduction

(b)

Interpretation:

From the given Ka values, pKa of weak acids should be calculated.

Concept introduction:

The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.

For a general reaction of ionization of weak acid as follows:

HA⇌H++A−

The expression for dissociation constant of the reaction is as follows:

Ka=[H+][A−][HA]

The pKa of a weak acid is defined as negative log of Ka or,

pK=−logKa

Answer 9

Interpretation Introduction

(b)

Interpretation:

From the given Ka values, pKa of weak acids should be calculated.

Concept introduction:

The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.

For a general reaction of ionization of weak acid as follows:

HA⇌H++A−

The expression for dissociation constant of the reaction is as follows:

Ka=[H+][A−][HA]

The pKa of a weak acid is defined as negative log of Ka or,

pK=−logKa

Answer 10

Interpretation Introduction

(c)

Interpretation:

From the given Ka values, pKa of weak acids should be calculated.

Concept introduction:

The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.

For a general reaction of ionization of weak acid as follows:

HA⇌H++A−

The expression for dissociation constant of the reaction is as follows:

Ka=[H+][A−][HA]

The pKa of a weak acid is defined as negative log of Ka or,

pK=−logKa

Answer 11

Interpretation Introduction

(c)

Interpretation:

From the given Ka values, pKa of weak acids should be calculated.

Concept introduction:

The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.

For a general reaction of ionization of weak acid as follows:

HA⇌H++A−

The expression for dissociation constant of the reaction is as follows:

Ka=[H+][A−][HA]

The pKa of a weak acid is defined as negative log of Ka or,

pK=−logKa

Answer 12

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Answer 13

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Answer 14

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Answer 15

Ch. 13 - For each of the following reactions, indicate the...Ch. 13 - Follow the direction for Question 1 for the...Ch. 13 - According to the BrĂ¸nsted-Lowry theory, which of...Ch. 13 - According to the BrĂ¸nsted-Lowry theory, which of...Ch. 13 - Give the formula of the conjugate acid of (a) OH-...Ch. 13 - Give the formula for the conjugate base of (a)...Ch. 13 - Write a balanced equation showing how the H2PO4-...Ch. 13 - Follow the instructions of Question 7 for the...Ch. 13 - Using the BrĂ¸nsted-Lowry model, write equations...Ch. 13 - Prob. 10QAP

Solution Summary: The author explains that the ionization equation of weak acids is in equilibrium. The pK_a of a weak acid is negative log of acid dissociation constant.

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