   Chapter 3, Problem 27PS

Chapter
Section
Textbook Problem

Predict the products of each precipitation reaction. Balance the equation, and then write the net ionic equation.(a) NiCl 2 (aq)+(NH 4 ) 2 S(aq) → (b) Mn(NO 3 ) 2 (aq)+Na 3 PO 4 (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 bit some of the alkali metal hydroxides, Ba(OH)2and Sr(OH)2 are soluble in water.

Explanation

The given compound is Nickel (II) chlorideand Ammonium sulfidewhich is soluble in water.  In this reaction Ni2+ and NH4+ cations exchange the anions (Cl- and S2-) to give Nickel sulfide and Ammoniumchloride.

Balance the equation,

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

There are two chlorine atoms in the left side and one chlorine atom in the right side. Therefore two molecule of ammonium chloride is added to left 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 bit some of the alkali metal hydroxides, Ba(OH)2and Sr(OH)2 are soluble in water.

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