   Chapter 3, Problem 69GQ

Chapter
Section
Textbook Problem

Give a formula for each of the following compounds:(a) a soluble compound containing the brømide ion(b) an insoluble hydroxide(c) an insoluble carbonate(d) a soluble nitrate-containing compound(e) a weak Brønsted acid

(a)

Interpretation Introduction

Interpretation:

The formula for the given compound should be given.

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.

Soluble compounds in water

Almost all the salts of Na+, K+, NH4+(NO3-),(ClO3-),(ClO4-)and(CH3CO2-) are soluble.

Almost all the salts of Cl-, Br-, I-(halides) are soluble.  But some of the halides are (Ag+, Hg22+, Pb2+) insoluble.

Salts of F- are soluble.  But some of the fluoride salt of Mg2+, Ca2+, Sr2+, Ba2+, Pb2+ are insoluble.

Salts of sulfate (SO42-) are soluble.  But sulfates of Ca2+, Sr2+, Ba2+, Pb2+, Ag+, are insoluble.

Insoluble compounds in water:

Most of the salts of (CO32-),(PO43-),(C2O42-),(CrO42-)and (S2-) are insoluble but some of the salts of NH4+, alkali metal cations and BaS are soluble.

Most of the metal hydroxides and oxides are insoluble in water bit some of the alkali metal hydroxides, Ba(OH)2and Sr(OH)2 are soluble in water.

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

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

Explanation

The soluble compound contains bromide ion is shown below

NaBr, KBr or other alkali metal bromides group 2A bromides, other metal bromides other than AgBr, Hg2Br2 and PbBr2 because, almost all the salts of Cl-, Br</

(b)

Interpretation Introduction

Interpretation:

The formula for the given compound should be given.

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.

Soluble compounds in water

Almost all the salts of Na+, K+, NH4+(NO3-),(ClO3-),(ClO4-)and(CH3CO2-) are soluble.

Almost all the salts of Cl-, Br-, I-(halides) are soluble.  But some of the halides are (Ag+, Hg22+, Pb2+) insoluble.

Salts of F- are soluble.  But some of the fluoride salt of Mg2+, Ca2+, Sr2+, Ba2+, Pb2+ are insoluble.

Salts of sulfate (SO42-) are soluble.  But sulfates of Ca2+, Sr2+, Ba2+, Pb2+, Ag+, are insoluble.

Insoluble compounds in water:

Most of the salts of (CO32-),(PO43-),(C2O42-),(CrO42-)and (S2-) are insoluble but some of the salts of NH4+, alkali metal cations and BaS are soluble.

Most of the metal hydroxides and oxides are insoluble in water but some of the alkali metal hydroxides, Ba(OH)2and Sr(OH)2 are soluble in water.

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

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

(c)

Interpretation Introduction

Interpretation:

The formula for the given compound should be given.

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.

Soluble compounds in water

Almost all the salts of Na+, K+, NH4+(NO3-),(ClO3-),(ClO4-)and(CH3CO2-) are soluble.

Almost all the salts of Cl-, Br-, I-(halides) are soluble.  But some of the halides are (Ag+, Hg22+, Pb2+) insoluble.

Salts of F- are soluble.  But some of the fluoride salt of Mg2+, Ca2+, Sr2+, Ba2+, Pb2+ are insoluble.

Salts of sulfate (SO42-) are soluble.  But sulfates of Ca2+, Sr2+, Ba2+, Pb2+, Ag+, are insoluble.

Insoluble compounds in water:

Most of the salts of (CO32-),(PO43-),(C2O42-),(CrO42-)and (S2-) are insoluble but some of the salts of NH4+, alkali metal cations and BaS are soluble.

Most of the metal hydroxides and oxides are insoluble in water but some of the alkali metal hydroxides, Ba(OH)2and Sr(OH)2 are soluble in water.

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

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

(d)

Interpretation Introduction

Interpretation:

The formula for the given compound should be given.

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.

Soluble compounds in water

Almost all the salts of Na+, K+, NH4+(NO3-),(ClO3-),(ClO4-)and(CH3CO2-) are soluble.

Almost all the salts of Cl-, Br-, I-(halides) are soluble.  But some of the halides are (Ag+, Hg22+, Pb2+) are insoluble.

Salts of F- are soluble.  But some of the fluoride salt of Mg2+, Ca2+, Sr2+, Ba2+, Pb2+ are insoluble.

Salts of sulfate (SO42-) are soluble.  But sulfates of Ca2+, Sr2+, Ba2+, Pb2+, Ag+, are insoluble.

Insoluble compounds in water:

Most of the salts of (CO32-),(PO43-),(C2O42-),(CrO42-)and (S2-) are insoluble but some of the salts of NH4+, alkali metal cations and BaS are soluble.

Most of the metal hydroxides and oxides are insoluble in water bit some of the alkali metal hydroxides, Ba(OH)2and Sr(OH)2 are soluble in water.

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

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

(e)

Interpretation Introduction

Interpretation:

The formula for the given compound should be given.

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.

Soluble compounds in water

Almost all the salts of Na+, K+, NH4+(NO3-),(ClO3-),(ClO4-)and(CH3CO2-) are soluble.

Almost all the salts of Cl-, Br-, I-(halides) are soluble.  But some of the halides are (Ag+, Hg22+, Pb2+) insoluble.

Salts of F- are soluble.  But some of the fluoride salt of Mg2+, Ca2+, Sr2+, Ba2+, Pb2+ are insoluble.

Salts of sulfate (SO42-) are soluble.  But sulfates of Ca2+, Sr2+, Ba2+, Pb2+, Ag+, are insoluble.

Insoluble compounds in water:

Most of the salts of (CO32-),(PO43-),(C2O42-),(CrO42-)and (S2-) are insoluble but some of the salts of NH4+, alkali metal cations and BaS are soluble.

Most of the metal hydroxides and oxides are insoluble in water bit some of the alkali metal hydroxides, Ba(OH)2and Sr(OH)2 are soluble in water.

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

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

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