   Chapter 3, Problem 79GQ

Chapter
Section
Textbook Problem

Identify the primary species (atoms, molecules, or ions) present in an aqueous solution of each of the following compounds. Decide which species are Brønsted acids or bases and whether they are strong or weak.(a) NH3(b) CH3CO2H(c) NaOH(d) HBr

Interpretation Introduction

(a)

Interpretation:

The primary species present in an aqueous solution of given compound has to be identified and the species either Bronsted acid or Bronsted base and strong or weak should be identified.

Concept introduction:

Most of the ionic compounds are soluble in water, very few of the ionic compounds are sparingly soluble, and some of the ionic compounds are insoluble in water.  When it is soluble in water ions gets separated in the solution.

Bronsted acid: An acid donates (loses)H+ ion.

Bronsted Base: A base accepts (gains)H+ ion.

Acids are two types one is strong another one is weak similarly, two types of base one is strong and another one is weak.  Acid strength can be measured by using acid-dissociation equilibrium constant, Ka, for that acid.

Ka=[H3O+][A-][HA]

If Ka is large, the acid is strong acid.

If Ka is small, the acid is weak acid.

Explanation

NH3 in water, behaves as a weak Bronsted base and it is exist as NH4+ and <

Interpretation Introduction

(b)

Interpretation:

The primary species present in an aqueous solution of given compound has to be identified and the species either Bronsted acid or Bronsted base and strong or weak should be identified.

Concept introduction:

Most of the ionic compounds are soluble in water, very few of the ionic compounds are sparingly soluble, and some of the ionic compounds are insoluble in water.  When it is soluble in water ions gets separated in the solution.

Bronsted acid: An acid donates (loses)H+ ion.

Bronsted Base: A base accepts (gains)H+ ion.

Acids are two types one is strong another one is weak similarly, two types of base one is strong and another one is weak.  Acid strength can be measured by using acid-dissociation equilibrium constant, Ka, for that acid.

Ka=[H3O+][A-][HA]

If Ka is large, the acid is strong acid.

If Ka is small, the acid is weak acid.

Interpretation Introduction

(c)

Interpretation:

The primary species present in an aqueous solution of given compound has to be identified and the species either Bronsted acid or Bronsted base and strong or weak should be identified.

Concept introduction:

Most of the ionic compounds are soluble in water, very few of the ionic compounds are sparingly soluble, and some of the ionic compounds are insoluble in water.  When it is soluble in water ions gets separated in the solution.

Bronsted acid: An acid donates (loses)H+ ion.

Bronsted Base: A base accepts (gains)H+ ion.

Acids are two types one is strong another one is weak similarly, two types of base one is strong and another one is weak.  Acid strength can be measured by using acid-dissociation equilibrium constant, Ka, for that acid.

Ka=[H3O+][A-][HA]

If Ka is large, the acid is strong acid.

If Ka is small, the acid is weak acid.

Interpretation Introduction

(d)

Interpretation:

The primary species present in an aqueous solution of given compound has to be identified and the species either Bronsted acid or Bronsted base and strong or weak should be identified.

Concept introduction:

Most of the ionic compounds are soluble in water, very few of the ionic compounds are sparingly soluble, and some of the ionic compounds are insoluble in water.  When it is soluble in water ions gets separated in the solution.

Bronsted acid: An acid donates (loses)H+ ion.

Bronsted Base: A base accepts (gains)H+ ion.

Acids are two types one is strong another one is weak similarly, two types of base one is strong and another one is weak.  Acid strength can be measured by using acid-dissociation equilibrium constant, Ka, for that acid.

Ka=[H3O+][A-][HA]

If Ka is large, the acid is strong acid.

If Ka is small, the acid is weak acid.

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started 