The buffer solution of pH value 6.50 cannot be prepared by mixing NH 3 to NH 4 Cl. The reason for this condition is to be explained. Concept introduction: The formulas which will be used- p K a = − log ( K a ) Henderson − Hasselbalch equation is as follows: p H = p K a + log [ B ] [ B H + ]

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Answer 1

Question

Chapter 14, Problem 73QAP

Interpretation Introduction

Interpretation:

The buffer solution of pH value 6.50 cannot be prepared by mixing NH₃ to NH₄ Cl. The reason for this condition is to be explained.

Concept introduction:

The formulas which will be used-

pKa=−log(Ka)

Henderson − Hasselbalch equation is as follows:

pH=pKa+log[B][BH+]

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In the solid state, oxalic acid occurs as a dihydrate with the formula H2C2O4 C+2H2O. Use this formula to calculate the formula weight of oxalic acid. Use the calculated formula weight and the number of moles (0.00504mol) of oxalic acid in each titrated unknown sample recorded in Table 6.4 to calculate the number of grams of pure oxalic acid dihydrate contained in each titrated unknown sample.

1. Consider a pair of elements with 2p and 4p valence orbitals (e.g., N and Se). Draw their (2p and 4p AO's) radial probability plots, and sketch their angular profiles. Then, consider these orbitals from the two atoms forming a homonuclear л-bond. Which element would have a stronger bond, and why? (4 points)

Answer 2

Question

Chapter 14, Problem 73QAP

Interpretation Introduction

Interpretation:

The buffer solution of pH value 6.50 cannot be prepared by mixing NH₃ to NH₄ Cl. The reason for this condition is to be explained.

Concept introduction:

The formulas which will be used-

pKa=−log(Ka)

Henderson − Hasselbalch equation is as follows:

pH=pKa+log[B][BH+]

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 14, Problem 73QAP

Interpretation Introduction

Interpretation:

The buffer solution of pH value 6.50 cannot be prepared by mixing NH₃ to NH₄ Cl. The reason for this condition is to be explained.

Concept introduction:

The formulas which will be used-

pKa=−log(Ka)

Henderson − Hasselbalch equation is as follows:

pH=pKa+log[B][BH+]

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 14, Problem 73QAP

Interpretation Introduction

Interpretation:

The buffer solution of pH value 6.50 cannot be prepared by mixing NH₃ to NH₄ Cl. The reason for this condition is to be explained.

Concept introduction:

The formulas which will be used-

pKa=−log(Ka)

Henderson − Hasselbalch equation is as follows:

pH=pKa+log[B][BH+]

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 5

Chapter 14, Problem 73QAP

Interpretation Introduction

Interpretation:

The buffer solution of pH value 6.50 cannot be prepared by mixing NH₃ to NH₄ Cl. The reason for this condition is to be explained.

Concept introduction:

The formulas which will be used-

pKa=−log(Ka)

Henderson − Hasselbalch equation is as follows:

pH=pKa+log[B][BH+]

Answer 6

Chapter 14, Problem 73QAP

Interpretation Introduction

Interpretation:

The buffer solution of pH value 6.50 cannot be prepared by mixing NH₃ to NH₄ Cl. The reason for this condition is to be explained.

Concept introduction:

The formulas which will be used-

pKa=−log(Ka)

Henderson − Hasselbalch equation is as follows:

pH=pKa+log[B][BH+]

Answer 7

Chapter 14, Problem 73QAP

Interpretation Introduction

Interpretation:

The buffer solution of pH value 6.50 cannot be prepared by mixing NH₃ to NH₄ Cl. The reason for this condition is to be explained.

Concept introduction:

The formulas which will be used-

pKa=−log(Ka)

Henderson − Hasselbalch equation is as follows:

pH=pKa+log[B][BH+]

Answer 8

Expert Solution & Answer

Answer 9

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Answer 10

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Answer 11

Ch. 14 - Write a net ionic equation for the reaction...Ch. 14 - Write a net ionic equation for the reaction...Ch. 14 - Write a balanced net ionic equation for the...Ch. 14 - Write a balanced net ionic equation for the...Ch. 14 - Calculate K for the reactions in Question 1.Ch. 14 - Calculate K for the reactions in Question 2.Ch. 14 - Prob. 7QAP Ch. 14 - Calculate K for the reactions in Question 4.Ch. 14 - Calculate [H+] and pH in a solution in which...Ch. 14 - Calculate [OH-] and pH in a solution in which the...

The buffer solution of pH value 6.50 cannot be prepared by mixing NH 3 to NH 4 Cl. The reason for this condition is to be explained. Concept introduction: The formulas which will be used- p K a = − log ( K a ) Henderson − Hasselbalch equation is as follows: p H = p K a + log [ B ] [ B H + ]

Solution Summary: The author explains that a buffer solution of pH value 6.50 cannot be prepared by mixing NH 3 to 4 Cl. The ratio of ammonia and its conjugate acid is very large.

Concept explainers

Videos

Interpretation:

The buffer solution of pH value 6.50 cannot be prepared by mixing NH₃ to NH₄ Cl. The reason for this condition is to be explained.

Concept introduction:

The formulas which will be used-

pKa=−log(Ka)

Henderson − Hasselbalch equation is as follows:

pH=pKa+log[B][BH+]

Want to see the full answer?

Chapter 14 Solutions

The buffer solution of pH value 6.50 cannot be prepared by mixing NH 3 to NH 4 Cl. The reason for this condition is to be explained. Concept introduction: The formulas which will be used- p K a = − log ( K a ) Henderson − Hasselbalch equation is as follows: p H = p K a + log [ B ] [ B H + ]

Solution Summary: The author explains that a buffer solution of pH value 6.50 cannot be prepared by mixing NH 3 to 4 Cl. The ratio of ammonia and its conjugate acid is very large.

Concept explainers

Videos

Interpretation: The buffer solution of pH value 6.50 cannot be prepared by mixing NH3 to NH4 Cl. The reason for this condition is to be explained. Concept introduction: The formulas which will be used- pKa=−log(Ka) Henderson − Hasselbalch equation is as follows: pH=pKa+log[B][BH+]

Want to see the full answer?

Chapter 14 Solutions

Interpretation:

The buffer solution of pH value 6.50 cannot be prepared by mixing NH₃ to NH₄ Cl. The reason for this condition is to be explained.

Concept introduction:

The formulas which will be used-

pKa=−log(Ka)

Henderson − Hasselbalch equation is as follows:

pH=pKa+log[B][BH+]