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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Nido-boranes are structures with the molecular formula BnHn+4 that exhibit B-B, B-H-B and B-H bonds. Correct?

8:07 AM Wed Dec 18 Final Exam 2024 copy Home Insert Draw Page Layout Formulas Data Review AA 田 General A G fx Alexis Cozort ☑ ⚫ 61% A B D E F H K M N P R S T U 3+ 10 125 mM that yielded peak heights of Aa = 9 1-(a)A sample solution was examined under XRF to quantify the analyte Ce³+. Find the response factor F, when standardized concentration of analyte [Ce³+]A = concentration of internal standard S i.e. [In³*]s = 151 mM was spiked with standardized 1600 and As = 3015 respectively? 11 12 (i)Define F, F = Aa As [A] [S] + X 13 (*Define with variables) 4000 14 15 (ii)Calculate F, F = numeral (You will use the F value in part 1-(b) below) As 16 (*Calculate with numerals) 17 18 1-(b)To determine the unknown conc of analyte [Ce³+], a volume of 15 mL of internal standard S having a concentration [In³+]s = 0.264 M 19 20 was added to 45 mL of unknown, and the mixture was diluted to 100 mL in a volumetric flask. XRF analysis yielded a spectrum, Figure-1, where peak heights A and As are…

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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).