The H S O 4 − ion act as a base in water, the balanced equation for this has to be written. Concept Introduction: Acid: According to Bronsted-Lowry theory, a species which donates a proton in a proton transfer-reaction is said to be an acid. Base: According to Bronsted-Lowry theory, a species which accepts a proton in a proton transfer-reaction is said to be base. Conjugated acid: In the conjugate acid-base pair, a species which can donates a proton is said to be conjugated acid. Conjugated base: In the conjugate acid-base pair, a species which can accepts a proton is said to be conjugated base.

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Answer 1

Question

Chapter 14.1, Problem 14.4E

(a)

Interpretation Introduction

Interpretation:

The HSO4− ion act as a base in water, the balanced equation for this has to be written.

Concept Introduction:

Acid: According to Bronsted-Lowry theory, a species which donates a proton in a proton transfer-reaction is said to be an acid.

Base: According to Bronsted-Lowry theory, a species which accepts a proton in a proton transfer-reaction is said to be base.

Conjugated acid: In the conjugate acid-base pair, a species which can donates a proton is said to be conjugated acid.

Conjugated base: In the conjugate acid-base pair, a species which can accepts a proton is said to be conjugated base.

(b)

Interpretation Introduction

Interpretation:

The conjugate acid – base pairs in the equation has to be identified.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

An explanation has to be given about the amphiprotic nature of HSO4−.

Concept Introduction:

Amphiprotic:

A molecule either by donating or accepting a proton, which will act either as an acid or a base and this molecule is said to be amphiprotic.

The examples are water, amino acids, hydrogen carbonate ions and hydrogen sulfate ions.

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Questions 4 and 5

For a titration of 40.00 mL of 0.0500 M oxalic acid H2C2O4 with 0.1000 M KOH, calculate the pH at each of the following volume of KOH used in the titration: 1) before the titration begin;2) 15 mL; 3) 20 mL; 4) 25 mL; 5) 40 mL; 6) 50 mL. Ka1 = 5.90×10^-2, Ka2 = 6.50×10^-5 for oxalic acid.

Predict the major organic product(s), if any, of the following reactions. Assume all reagents are in excess unless otherwise indicated.

Answer 2

Question

Chapter 14.1, Problem 14.4E

(a)

Interpretation Introduction

Interpretation:

The HSO4− ion act as a base in water, the balanced equation for this has to be written.

Concept Introduction:

Acid: According to Bronsted-Lowry theory, a species which donates a proton in a proton transfer-reaction is said to be an acid.

Base: According to Bronsted-Lowry theory, a species which accepts a proton in a proton transfer-reaction is said to be base.

Conjugated acid: In the conjugate acid-base pair, a species which can donates a proton is said to be conjugated acid.

Conjugated base: In the conjugate acid-base pair, a species which can accepts a proton is said to be conjugated base.

(b)

Interpretation Introduction

Interpretation:

The conjugate acid – base pairs in the equation has to be identified.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

An explanation has to be given about the amphiprotic nature of HSO4−.

Concept Introduction:

Amphiprotic:

A molecule either by donating or accepting a proton, which will act either as an acid or a base and this molecule is said to be amphiprotic.

The examples are water, amino acids, hydrogen carbonate ions and hydrogen sulfate ions.

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Answer 3

Question

Chapter 14.1, Problem 14.4E

(a)

Interpretation Introduction

Interpretation:

The HSO4− ion act as a base in water, the balanced equation for this has to be written.

Concept Introduction:

Acid: According to Bronsted-Lowry theory, a species which donates a proton in a proton transfer-reaction is said to be an acid.

Base: According to Bronsted-Lowry theory, a species which accepts a proton in a proton transfer-reaction is said to be base.

Conjugated acid: In the conjugate acid-base pair, a species which can donates a proton is said to be conjugated acid.

Conjugated base: In the conjugate acid-base pair, a species which can accepts a proton is said to be conjugated base.

(b)

Interpretation Introduction

Interpretation:

The conjugate acid – base pairs in the equation has to be identified.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

An explanation has to be given about the amphiprotic nature of HSO4−.

Concept Introduction:

Amphiprotic:

A molecule either by donating or accepting a proton, which will act either as an acid or a base and this molecule is said to be amphiprotic.

The examples are water, amino acids, hydrogen carbonate ions and hydrogen sulfate ions.

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Answer 4

Question

Chapter 14.1, Problem 14.4E

(a)

Interpretation Introduction

Interpretation:

The HSO4− ion act as a base in water, the balanced equation for this has to be written.

Concept Introduction:

Acid: According to Bronsted-Lowry theory, a species which donates a proton in a proton transfer-reaction is said to be an acid.

Base: According to Bronsted-Lowry theory, a species which accepts a proton in a proton transfer-reaction is said to be base.

Conjugated acid: In the conjugate acid-base pair, a species which can donates a proton is said to be conjugated acid.

Conjugated base: In the conjugate acid-base pair, a species which can accepts a proton is said to be conjugated base.

(b)

Interpretation Introduction

Interpretation:

The conjugate acid – base pairs in the equation has to be identified.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

An explanation has to be given about the amphiprotic nature of HSO4−.

Concept Introduction:

Amphiprotic:

A molecule either by donating or accepting a proton, which will act either as an acid or a base and this molecule is said to be amphiprotic.

The examples are water, amino acids, hydrogen carbonate ions and hydrogen sulfate ions.

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Answer 5

Chapter 14.1, Problem 14.4E

(a)

Interpretation Introduction

Interpretation:

The HSO4− ion act as a base in water, the balanced equation for this has to be written.

Concept Introduction:

Acid: According to Bronsted-Lowry theory, a species which donates a proton in a proton transfer-reaction is said to be an acid.

Base: According to Bronsted-Lowry theory, a species which accepts a proton in a proton transfer-reaction is said to be base.

Conjugated acid: In the conjugate acid-base pair, a species which can donates a proton is said to be conjugated acid.

Conjugated base: In the conjugate acid-base pair, a species which can accepts a proton is said to be conjugated base.

(b)

Interpretation Introduction

Interpretation:

The conjugate acid – base pairs in the equation has to be identified.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

An explanation has to be given about the amphiprotic nature of HSO4−.

Concept Introduction:

Amphiprotic:

A molecule either by donating or accepting a proton, which will act either as an acid or a base and this molecule is said to be amphiprotic.

The examples are water, amino acids, hydrogen carbonate ions and hydrogen sulfate ions.

Answer 6

Chapter 14.1, Problem 14.4E

(a)

Interpretation Introduction

Interpretation:

The HSO4− ion act as a base in water, the balanced equation for this has to be written.

Concept Introduction:

Acid: According to Bronsted-Lowry theory, a species which donates a proton in a proton transfer-reaction is said to be an acid.

Base: According to Bronsted-Lowry theory, a species which accepts a proton in a proton transfer-reaction is said to be base.

Conjugated acid: In the conjugate acid-base pair, a species which can donates a proton is said to be conjugated acid.

Conjugated base: In the conjugate acid-base pair, a species which can accepts a proton is said to be conjugated base.

Answer 7

Chapter 14.1, Problem 14.4E

(a)

Interpretation Introduction

Interpretation:

The HSO4− ion act as a base in water, the balanced equation for this has to be written.

Concept Introduction:

Acid: According to Bronsted-Lowry theory, a species which donates a proton in a proton transfer-reaction is said to be an acid.

Base: According to Bronsted-Lowry theory, a species which accepts a proton in a proton transfer-reaction is said to be base.

Conjugated acid: In the conjugate acid-base pair, a species which can donates a proton is said to be conjugated acid.

Conjugated base: In the conjugate acid-base pair, a species which can accepts a proton is said to be conjugated base.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The conjugate acid – base pairs in the equation has to be identified.

Concept Introduction:

Refer to part (a).

Answer 9

(b)

Interpretation Introduction

Interpretation:

The conjugate acid – base pairs in the equation has to be identified.

Concept Introduction:

Refer to part (a).

Answer 10

(c)

Interpretation Introduction

Interpretation:

An explanation has to be given about the amphiprotic nature of HSO4−.

Concept Introduction:

Amphiprotic:

A molecule either by donating or accepting a proton, which will act either as an acid or a base and this molecule is said to be amphiprotic.

The examples are water, amino acids, hydrogen carbonate ions and hydrogen sulfate ions.

Answer 11

(c)

Interpretation Introduction

Interpretation:

An explanation has to be given about the amphiprotic nature of HSO4−.

Concept Introduction:

Amphiprotic:

A molecule either by donating or accepting a proton, which will act either as an acid or a base and this molecule is said to be amphiprotic.

The examples are water, amino acids, hydrogen carbonate ions and hydrogen sulfate ions.

Answer 12

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Answer 13

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Answer 14

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Answer 15

Ch. 14.1 - Identify each molecule or ion as a Brnsted-Lowry...Ch. 14.1 - Using Le Chatelier’s Principle Use Le Chatelier’s...Ch. 14.1 - Prob. 14.3E Ch. 14.1 - Complete the table. Ch. 14.1 - Prob. 14.4E Ch. 14.1 - Prob. 14.5E Ch. 14.2 - Prob. 14.6CE Ch. 14.2 - Prob. 14.7E Ch. 14.3 - Prob. 14.2PSP Ch. 14.3 - Prob. 14.3PSP

Solution Summary: The author explains that the HSO_4- ion act as a base in water, the balanced equation for this has to be written.

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Interpretation:

The conjugate acid – base pairs in the equation has to be identified.

Concept Introduction:

Refer to part (a).

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Chapter 14 Solutions

Solution Summary: The author explains that the HSO_4- ion act as a base in water, the balanced equation for this has to be written.

Concept explainers

Videos

Interpretation: The conjugate acid – base pairs in the equation has to be identified. Concept Introduction: Refer to part (a).

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Chapter 14 Solutions

Interpretation:

The conjugate acid – base pairs in the equation has to be identified.

Concept Introduction:

Refer to part (a).