This is to be shown that if the concentration of hydronium ion is reduced to half, the pH of solution increases by 0.3 unit. Whether it is true for change in concentration of any species or only hydronium ion needs to be explained. Concept introduction: As per the Bronsted-Lowry theory of bases and acids, proton acceptors are bases and proton donors are acids. Molecule which can either accept or donate the proton are known as amphiprotic. So, an amphiprotic act as either base or acid. Hydrogen sulfate ion, hydrogen carbonate ion, amino acids and water are common illustrations of amphiprotic molecules. Because they might donate the proton, all of the amphiprotic species have hydrogen atom. Molarity of any solution is defined as number of moles of solute in 1 L of the solution. The pH is a degree of hydrogen ion concentration, a degree of the alkalinity or acidity of a solution.

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Answer 1

Question

Chapter 16, Problem 84IAE

Interpretation Introduction

Interpretation:

This is to be shown that if the concentration of hydronium ion is reduced to half, the pH of solution increases by 0.3 unit. Whether it is true for change in concentration of any species or only hydronium ion needs to be explained.

Concept introduction:

As per the Bronsted-Lowry theory of bases and acids, proton acceptors are bases and proton donors are acids. Molecule which can either accept or donate the proton are known as amphiprotic. So, an amphiprotic act as either base or acid. Hydrogen sulfate ion, hydrogen carbonate ion, amino acids and water are common illustrations of amphiprotic molecules. Because they might donate the proton, all of the amphiprotic species have hydrogen atom.

Molarity of any solution is defined as number of moles of solute in 1 L of the solution.

The pH is a degree of hydrogen ion concentration, a degree of the alkalinity or acidity of a solution.

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Answer 2

Question

Chapter 16, Problem 84IAE

Interpretation Introduction

Interpretation:

This is to be shown that if the concentration of hydronium ion is reduced to half, the pH of solution increases by 0.3 unit. Whether it is true for change in concentration of any species or only hydronium ion needs to be explained.

Concept introduction:

As per the Bronsted-Lowry theory of bases and acids, proton acceptors are bases and proton donors are acids. Molecule which can either accept or donate the proton are known as amphiprotic. So, an amphiprotic act as either base or acid. Hydrogen sulfate ion, hydrogen carbonate ion, amino acids and water are common illustrations of amphiprotic molecules. Because they might donate the proton, all of the amphiprotic species have hydrogen atom.

Molarity of any solution is defined as number of moles of solute in 1 L of the solution.

The pH is a degree of hydrogen ion concentration, a degree of the alkalinity or acidity of a solution.

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 16, Problem 84IAE

Interpretation Introduction

Interpretation:

This is to be shown that if the concentration of hydronium ion is reduced to half, the pH of solution increases by 0.3 unit. Whether it is true for change in concentration of any species or only hydronium ion needs to be explained.

Concept introduction:

As per the Bronsted-Lowry theory of bases and acids, proton acceptors are bases and proton donors are acids. Molecule which can either accept or donate the proton are known as amphiprotic. So, an amphiprotic act as either base or acid. Hydrogen sulfate ion, hydrogen carbonate ion, amino acids and water are common illustrations of amphiprotic molecules. Because they might donate the proton, all of the amphiprotic species have hydrogen atom.

Molarity of any solution is defined as number of moles of solute in 1 L of the solution.

The pH is a degree of hydrogen ion concentration, a degree of the alkalinity or acidity of a solution.

Expert Solution & Answer

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Answer 4

Question

Chapter 16, Problem 84IAE

Interpretation Introduction

Interpretation:

This is to be shown that if the concentration of hydronium ion is reduced to half, the pH of solution increases by 0.3 unit. Whether it is true for change in concentration of any species or only hydronium ion needs to be explained.

Concept introduction:

As per the Bronsted-Lowry theory of bases and acids, proton acceptors are bases and proton donors are acids. Molecule which can either accept or donate the proton are known as amphiprotic. So, an amphiprotic act as either base or acid. Hydrogen sulfate ion, hydrogen carbonate ion, amino acids and water are common illustrations of amphiprotic molecules. Because they might donate the proton, all of the amphiprotic species have hydrogen atom.

Molarity of any solution is defined as number of moles of solute in 1 L of the solution.

The pH is a degree of hydrogen ion concentration, a degree of the alkalinity or acidity of a solution.

Expert Solution & Answer

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Answer 5

Chapter 16, Problem 84IAE

Interpretation Introduction

Interpretation:

This is to be shown that if the concentration of hydronium ion is reduced to half, the pH of solution increases by 0.3 unit. Whether it is true for change in concentration of any species or only hydronium ion needs to be explained.

Concept introduction:

As per the Bronsted-Lowry theory of bases and acids, proton acceptors are bases and proton donors are acids. Molecule which can either accept or donate the proton are known as amphiprotic. So, an amphiprotic act as either base or acid. Hydrogen sulfate ion, hydrogen carbonate ion, amino acids and water are common illustrations of amphiprotic molecules. Because they might donate the proton, all of the amphiprotic species have hydrogen atom.

Molarity of any solution is defined as number of moles of solute in 1 L of the solution.

The pH is a degree of hydrogen ion concentration, a degree of the alkalinity or acidity of a solution.

Answer 6

Chapter 16, Problem 84IAE

Interpretation Introduction

Interpretation:

This is to be shown that if the concentration of hydronium ion is reduced to half, the pH of solution increases by 0.3 unit. Whether it is true for change in concentration of any species or only hydronium ion needs to be explained.

Concept introduction:

As per the Bronsted-Lowry theory of bases and acids, proton acceptors are bases and proton donors are acids. Molecule which can either accept or donate the proton are known as amphiprotic. So, an amphiprotic act as either base or acid. Hydrogen sulfate ion, hydrogen carbonate ion, amino acids and water are common illustrations of amphiprotic molecules. Because they might donate the proton, all of the amphiprotic species have hydrogen atom.

Molarity of any solution is defined as number of moles of solute in 1 L of the solution.

The pH is a degree of hydrogen ion concentration, a degree of the alkalinity or acidity of a solution.

Answer 7

Chapter 16, Problem 84IAE

Interpretation Introduction

Interpretation:

This is to be shown that if the concentration of hydronium ion is reduced to half, the pH of solution increases by 0.3 unit. Whether it is true for change in concentration of any species or only hydronium ion needs to be explained.

Concept introduction:

As per the Bronsted-Lowry theory of bases and acids, proton acceptors are bases and proton donors are acids. Molecule which can either accept or donate the proton are known as amphiprotic. So, an amphiprotic act as either base or acid. Hydrogen sulfate ion, hydrogen carbonate ion, amino acids and water are common illustrations of amphiprotic molecules. Because they might donate the proton, all of the amphiprotic species have hydrogen atom.

Molarity of any solution is defined as number of moles of solute in 1 L of the solution.

The pH is a degree of hydrogen ion concentration, a degree of the alkalinity or acidity of a solution.

Answer 8

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Answer 11

Ch. 16 - According to the Brønsted-Lowry theory, lebel each...Ch. 16 - Write the formula of the conjugate based in the...Ch. 16 - For each of the following, identify the acides and...Ch. 16 - Which of the following species are amphiprotic in...Ch. 16 - Why which of the following bases will the...Ch. 16 - In a manner similar to equation (16.3), represent...Ch. 16 - With the aid of Table 16.2, predict the direction...Ch. 16 - With the aid of Table 16.2, predict the direction...Ch. 16 - Calculate [H2O4] and [OH-] or each solution: (a)...Ch. 16 - What is the pH of each of the following solution?...

Solution Summary: The author explains that if the concentration of hydronium ion is reduced to half, the pH of solution increases by 0.3 unit.

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