   # Predict the products of each precipitation reaction. Balance the equation, and then write the net ionic equation. (a) Pb(NO 3 ) 2 (aq) + KBr(aq) → (b) Ca(NO 3 ) 2 (aq) + KF(aq) → (c) Ca(NO 3 ) 2 (aq) + Na 2 C 2 O 4 (aq) → ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 3, Problem 20PS
Textbook Problem
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## Predict the products of each precipitation reaction. Balance the equation, and then write the net ionic equation.(a) Pb(NO3)2(aq) + KBr(aq) →(b) Ca(NO3)2(aq) + KF(aq) →(c) Ca(NO3)2(aq) + Na2C2O4(aq) →

(a)

Interpretation Introduction

Interpretation:

Product and balanced net ionic equation for the given aqueous solution should be written.

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+, salts of nitrate (NO3-), chlorate (ClO3-), Perchlorate (ClO4-), Acetate (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 carbonate (CO32-), phosphate (PO43-), Oxalate (C2O42-), Chromate (CrO42-), sulfide (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.

### Explanation of Solution

The given compound is lead nitrate and potassium bromidewhich is soluble in water.  In this reaction Pb2+ and K+ cations exchange the anions (NO3- and Br-) to give lead bromide and potassium nitrate.

Balance the equation,

Balance the bromine atom in the given equation, when balancing the equation, we should not alter the subscripts and we can change coefficients.

There are two bromine atoms in the right side and one bromine atom in the left side. Therefore two molecule of sodium bromide is added to left side of reaction.  Therefore the balanced equation is given below.

Balance the sodium atom in the given equation, there are two sodium atoms in the left side and one sodium atom in the right side.  Therefore two molecule of sodium nitrate is added to right side of reaction.  Therefore the balanced equation is given below.

Therefore the balanced equation is given below.

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

(b)

Interpretation Introduction

Interpretation:

Product and balanced net ionic equation for the given aqueous solution should be written.

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+, salts of nitrate (NO3-), chlorate (ClO3-), Perchlorate (ClO4-), Acetate (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 carbonate (CO32-), phosphate (PO43-), Oxalate (C2O42-), Chromate (CrO42-), sulfide (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.

(c)

Interpretation Introduction

Interpretation:

Product and balanced net ionic equation for the given aqueous solution should be written.

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+, salts of nitrate (NO3-), chlorate (ClO3-), Perchlorate (ClO4-), Acetate (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 carbonate (CO32-), phosphate (PO43-), Oxalate (C2O42-), Chromate (CrO42-), sulfide (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.

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