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Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
Not helpful? See similar books
Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
Chemical Reactions. 70GQ

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 + , NH 4 + , ( NO 3 - ) , ( ClO 3 - ) , ( ClO 4 - ) and ( CH 3 CO 2 - ) are soluble. Almost all the salts of Cl - , Br - , I - ( halides ) are soluble. But some of the halides are ( Ag + , Hg 2 2+ , Pb 2+ ) insoluble. Salts of F - are soluble. But some of the fluoride salt of Mg 2+ , Ca 2+ , Sr 2+ , Ba 2+ , Pb 2+ are insoluble. Salts of sulfate ( SO 4 2- ) are soluble. But sulfates of Ca 2+ , Sr 2+ , Ba 2+ , Pb 2+ , Ag + , are insoluble. Insoluble compounds in water: Most of the salts of ( CO 3 2- ) , ( PO 4 3- ) , ( C 2 O 4 2- ) , ( CrO 4 2- ) and ( S 2- ) are insoluble but some of the salts of NH 4 + , 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 ) 2 and Sr ( OH ) 2 are soluble in water. Bronsted acid: An acid donates (loses) H + ion. Bronsted Base: A base accepts (gains) H + ion.

Question
Chapter 3, Problem 70GQ

(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.

(a)

Expert Solution

Answer to Problem 70GQ

CH3COONa, CH3COOK, CH3COONH4 is soluble acetate ion.

Explanation of Solution

The soluble compound contains acetate ion is shown below

CH3COONa, CH3COOK, CH3COONH4 are soluble because, almost all the salts of Na+, K+, NH4+,(NO3-),(ClO3-),(ClO4-)and(CH3CO2-) are soluble.

(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 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.

(b)

Expert Solution

Answer to Problem 70GQ

MnS, CdS and transition metal sulfides.

Explanation of Solution

The insoluble sulfides are MnS, CdS and transition metal sulfides, because 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.

(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 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.

(c)

Expert Solution

Answer to Problem 70GQ

The soluble hydroxides are Ba(OH)2and Sr(OH)2.

Explanation of Solution

The soluble hydroxides are Ba(OH)2and Sr(OH)2, because 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.

(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+) 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.

(d)

Expert Solution

Answer to Problem 70GQ

The insoluble chlorides are AgCl, Hg2Cl2 and PbCl2.

Explanation of Solution

The insoluble chlorides are AgCl, Hg2Cl2 and PbCl2 because, Almost all the salts of Cl-, Br-, I-(halides) are soluble.  But some of the halides are (Ag+, Hg22+, Pb2+) insoluble.

(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.

(e)

Expert Solution

Answer to Problem 70GQ

Strong Bronsted base is NaOH.

Explanation of Solution

Strong Bronsted base is NaOH, other base which accept the H+ ion.

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Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
Not helpful? See similar books
Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
Chemical Reactions. 70GQ
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Chapter 3 Solutions

Chemistry & Chemical Reactivity
Ch. 3.9 - Prob. 1.1ACPCh. 3.9 - Prob. 1.2ACPCh. 3.9 - Prob. 1.3ACPCh. 3.9 - Prob. 1.4ACPCh. 3.9 - Prob. 1.5ACPCh. 3.9 - Prob. 2.1ACPCh. 3.9 - Prob. 2.2ACPCh. 3.9 - Prob. 3.1ACPCh. 3.9 - Prob. 3.2ACPCh. 3 - Prob. 1PSCh. 3 - Prob. 2PSCh. 3 - Prob. 3PSCh. 3 - Prob. 4PSCh. 3 - Prob. 5PSCh. 3 - Prob. 6PSCh. 3 - Prob. 7PSCh. 3 - Prob. 8PSCh. 3 - Prob. 9PSCh. 3 - Prob. 10PSCh. 3 - Prob. 11PSCh. 3 - Prob. 12PSCh. 3 - Prob. 13PSCh. 3 - Prob. 14PSCh. 3 - Prob. 15PSCh. 3 - Prob. 16PSCh. 3 - Prob. 17PSCh. 3 - Prob. 18PSCh. 3 - Prob. 19PSCh. 3 - Prob. 20PSCh. 3 - Prob. 21PSCh. 3 - Prob. 22PSCh. 3 - Prob. 23PSCh. 3 - Prob. 24PSCh. 3 - Prob. 25PSCh. 3 - Prob. 26PSCh. 3 - Prob. 27PSCh. 3 - Prob. 28PSCh. 3 - Prob. 29PSCh. 3 - Prob. 30PSCh. 3 - Prob. 31PSCh. 3 - Prob. 32PSCh. 3 - Prob. 33PSCh. 3 - Prob. 34PSCh. 3 - Prob. 35PSCh. 3 - Prob. 36PSCh. 3 - Prob. 37PSCh. 3 - Prob. 38PSCh. 3 - Prob. 39PSCh. 3 - Prob. 40PSCh. 3 - Prob. 41PSCh. 3 - Prob. 42PSCh. 3 - Prob. 43PSCh. 3 - Prob. 44PSCh. 3 - Prob. 45PSCh. 3 - Prob. 46PSCh. 3 - Prob. 47PSCh. 3 - Prob. 48PSCh. 3 - Prob. 49PSCh. 3 - Prob. 50PSCh. 3 - Prob. 51PSCh. 3 - Prob. 52PSCh. 3 - Prob. 53PSCh. 3 - Prob. 54PSCh. 3 - Prob. 55PSCh. 3 - Prob. 56PSCh. 3 - Prob. 57PSCh. 3 - Prob. 58PSCh. 3 - Prob. 59PSCh. 3 - Prob. 60PSCh. 3 - Prob. 61PSCh. 3 - Prob. 62PSCh. 3 - Prob. 63PSCh. 3 - Prob. 64PSCh. 3 - Prob. 65PSCh. 3 - Prob. 66PSCh. 3 - Prob. 67GQCh. 3 - Prob. 68GQCh. 3 - Prob. 69GQCh. 3 - Prob. 70GQCh. 3 - Prob. 71GQCh. 3 - Prob. 72GQCh. 3 - Prob. 73GQCh. 3 - Prob. 74GQCh. 3 - Prob. 75GQCh. 3 - Prob. 76GQCh. 3 - Prob. 77GQCh. 3 - Prob. 78GQCh. 3 - Prob. 79GQCh. 3 - Prob. 80GQCh. 3 - Prob. 81GQCh. 3 - Prob. 82GQCh. 3 - Prob. 83GQCh. 3 - Prob. 84GQCh. 3 - Prob. 85GQCh. 3 - Prob. 86GQCh. 3 - Prob. 87GQCh. 3 - Prob. 89ILCh. 3 - Prob. 90ILCh. 3 - Prob. 91ILCh. 3 - Prob. 92ILCh. 3 - Prob. 93ILCh. 3 - Prob. 94SCQCh. 3 - Prob. 95SCQCh. 3 - Prob. 96SCQCh. 3 - Prob. 97SCQCh. 3 - Prob. 98SCQCh. 3 - Prob. 99SCQCh. 3 - Prob. 101SCQ
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