Pearson eText Basic Chemistry -- Instant Access (Pearson+)
6th Edition
ISBN: 9780135765982
Author: Karen Timberlake, William Timberlake
Publisher: PEARSON+
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Chapter 12.3, Problem 23PP
(a)
Interpretation Introduction
Interpretation: If the given ionic compound is soluble in water or not should be identified.
Concept Introduction: The solubility of ionic compounds is high in polar solvents such as water. This is because the ions present in it are strongly attracted to the molecules of the polar solvent. If there is any common ion in the ionic compound and the solvent, the solubility of ionic compound in that solvent decreases.
There are following rules of solubility of an ionic compound in the water:
- The salts of group 1 elements (alkali metals) are soluble. Also, salts of ammonium ion are soluble.
- The salts of nitrate ion are commonly soluble.
- The salts of chloride, bromide and iodide ions are commonly soluble. But halide salts of silver ion, lead ion and mercury ions are insoluble.
- Most of the silver salts are insoluble but silver nitrate and silver acetate are generally soluble.
- Most of the sulphate salts are soluble but calcium sulphate, barium sulphate, silver sulphate and strontium sulphate are insoluble.
- Most of the hydroxide salts are slightly soluble but that of group 1 elements are soluble. Hydroxide salts of
transition metals and aluminium ion are insoluble. Therefore, iron hydroxide, aluminium hydroxide and cobalt hydroxide are insoluble. - The sulphides of transition metals are strongly insoluble such as cadmium sulphide, iron sulphide, zinc sulphide and silver sulphide. The salts of arsenic, antimony, bismuth and lead are also insoluble.
- Carbonates are insoluble.
- Chromates are insoluble.
- Phosphates are also insoluble such as calcium phosphate and silver phosphate.
- Fluorides are also insoluble such as barium fluoride, magnesium fluoride and lead fluoride.
(b)
Interpretation Introduction
Interpretation: If the given ionic compound is soluble in water or not should be identified.
Concept Introduction: The solubility of ionic compounds is high in polar solvents such as water. This is because the ions present in it are strongly attracted to the molecules of the polar solvent. If there is any common ion in the ionic compound and the solvent, the solubility of ionic compound in that solvent decreases.
There are following rules of solubility of an ionic compound in the water:
- The salts of group 1 elements (alkali metals) are soluble. Also, salts of ammonium ion are soluble.
- The salts of nitrate ion are commonly soluble.
- The salts of chloride, bromide and iodide ions are commonly soluble. But halide salts of silver ion, lead ion and mercury ions are insoluble.
- Most of the silver salts are insoluble but silver nitrate and silver acetate are generally soluble.
- Most of the sulphate salts are soluble but calcium sulphate, barium sulphate, silver sulphate and strontium sulphate are insoluble.
- Most of the hydroxide salts are slightly soluble but that of group 1 elements are soluble. Hydroxide salts of transition metals and aluminium ion are insoluble. Therefore, iron hydroxide, aluminium hydroxide and cobalt hydroxide are insoluble.
- The sulphides of transition metals are strongly insoluble such as cadmium sulphide, iron sulphide, zinc sulphide and silver sulphide. The salts of arsenic, antimony, bismuth and lead are also insoluble.
- Carbonates are insoluble.
- Chromates are insoluble.
- Phosphates are also insoluble such as calcium phosphate and silver phosphate.
- Fluorides are also insoluble such as barium fluoride, magnesium fluoride and lead fluoride.
(c)
Interpretation Introduction
Interpretation: If the given ionic compound is soluble in water or not should be identified.
Concept Introduction: The solubility of ionic compounds is high in polar solvents such as water. This is because the ions present in it are strongly attracted to the molecules of the polar solvent. If there is any common ion in the ionic compound and the solvent, the solubility of ionic compound in that solvent decreases.
There are following rules of solubility of an ionic compound in the water:
- The salts of group 1 elements (alkali metals) are soluble. Also, salts of ammonium ion are soluble.
- The salts of nitrate ion are commonly soluble.
- The salts of chloride, bromide and iodide ions are commonly soluble. But halide salts of silver ion, lead ion and mercury ions are insoluble.
- Most of the silver salts are insoluble but silver nitrate and silver acetate are generally soluble.
- Most of the sulphate salts are soluble but calcium sulphate, barium sulphate, silver sulphate and strontium sulphate are insoluble.
- Most of the hydroxide salts are slightly soluble but that of group 1 elements are soluble. Hydroxide salts of transition metals and aluminium ion are insoluble. Therefore, iron hydroxide, aluminium hydroxide and cobalt hydroxide are insoluble.
- The sulphides of transition metals are strongly insoluble such as cadmium sulphide, iron sulphide, zinc sulphide and silver sulphide. The salts of arsenic, antimony, bismuth and lead are also insoluble.
- Carbonates are insoluble.
- Chromates are insoluble.
- Phosphates are also insoluble such as calcium phosphate and silver phosphate.
- Fluorides are also insoluble such as barium fluoride, magnesium fluoride and lead fluoride.
(d)
Interpretation Introduction
Interpretation: If the given ionic compound is soluble in water or not should be identified.
Concept Introduction: The solubility of ionic compounds is high in polar solvents such as water. This is because the ions present in it are strongly attracted to the molecules of the polar solvent. If there is any common ion in the ionic compound and the solvent, the solubility of ionic compound in that solvent decreases.
There are following rules of solubility of an ionic compound in the water:
- The salts of group 1 elements (alkali metals) are soluble. Also, salts of ammonium ion are soluble.
- The salts of nitrate ion are commonly soluble.
- The salts of chloride, bromide and iodide ions are commonly soluble. But halide salts of silver ion, lead ion and mercury ions are insoluble.
- Most of the silver salts are insoluble but silver nitrate and silver acetate are generally soluble.
- Most of the sulphate salts are soluble but calcium sulphate, barium sulphate, silver sulphate and strontium sulphate are insoluble.
- Most of the hydroxide salts are slightly soluble but that of group 1 elements are soluble. Hydroxide salts of transition metals and aluminium ion are insoluble. Therefore, iron hydroxide, aluminium hydroxide and cobalt hydroxide are insoluble.
- The sulphides of transition metals are strongly insoluble such as cadmium sulphide, iron sulphide, zinc sulphide and silver sulphide. The salts of arsenic, antimony, bismuth and lead are also insoluble.
- Carbonates are insoluble.
- Chromates are insoluble.
- Phosphates are also insoluble such as calcium phosphate and silver phosphate.
- Fluorides are also insoluble such as barium fluoride, magnesium fluoride and lead fluoride.
(e)
Interpretation Introduction
Interpretation: If the given ionic compound is soluble in water or not should be identified.
Concept Introduction: The solubility of ionic compounds is high in polar solvents such as water. This is because the ions present in it are strongly attracted to the molecules of the polar solvent. If there is any common ion in the ionic compound and the solvent, the solubility of ionic compound in that solvent decreases.
There are following rules of solubility of an ionic compound in the water:
- The salts of group 1 elements (alkali metals) are soluble. Also, salts of ammonium ion are soluble.
- The salts of nitrate ion are commonly soluble.
- The salts of chloride, bromide and iodide ions are commonly soluble. But halide salts of silver ion, lead ion and mercury ions are insoluble.
- Most of the silver salts are insoluble but silver nitrate and silver acetate are generally soluble.
- Most of the sulphate salts are soluble but calcium sulphate, barium sulphate, silver sulphate and strontium sulphate are insoluble.
- Most of the hydroxide salts are slightly soluble but that of group 1 elements are soluble. Hydroxide salts of transition metals and aluminium ion are insoluble. Therefore, iron hydroxide, aluminium hydroxide and cobalt hydroxide are insoluble.
- The sulphides of transition metals are strongly insoluble such as cadmium sulphide, iron sulphide, zinc sulphide and silver sulphide. The salts of arsenic, antimony, bismuth and lead are also insoluble.
- Carbonates are insoluble.
- Chromates are insoluble.
- Phosphates are also insoluble such as calcium phosphate and silver phosphate.
- Fluorides are also insoluble such as barium fluoride, magnesium fluoride and lead fluoride.
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C-RSA CHROMATOPAC CH=1
DATA 1: @CHRM1.C00
ATTEN=10 SPEED= 10.0
0.0 b.092
0.797
1.088
1.813
C-RSA CHROMATOPAC CH=1 Report No. =13
** CALCULATION REPORT **
DATA=1: @CHRM1.000 11/03/05 08:09:52
CH PKNO
TIME
1
2
0.797
3
1.088
4
1.813
AREA
1508566
4625442
2180060
HEIGHT
207739
701206 V
287554 V
MK IDNO
CONC
NAME
18.1447
55.6339
26.2213
TOTAL
8314067 1196500
100
C-R8A CHROMATOPAC CH=1
DATA 1: @CHRM1.C00
ATTEN=10 SPEED= 10.0
0. 0
087
337.
0.841
1.150
C-R8A CHROMATOPAC CH=1 Report No. =14
DATA=1: @CHRM1.000 11/03/05 08:12:40
** CALCULATION REPORT **
CH PKNO
TIME
AREA
1
3 0.841
1099933
41.15
4039778
HEIGHT MK IDNO
170372
649997¯¯¯
CONC
NAME
21.4007
78.5993
TOTAL
5139711 820369
100
3
C-R8A CHROMATOPAC
CH=1
DATA 1: @CHRM1.C00
ATTEN=10 SPEED= 10.0
0.100
0:652
5.856
3
1.165
C-RSA CHROMATOPAC CH-1 Report No. =15
DATA=1: @CHRM1.000 11/03/05 08:15:26
** CALCULATION REPORT **
CH PKNO TIME
AREA
HEIGHT MK IDNO CONC
NAME
1 3 3 0.856
4
1.165
TOTAL
1253386
4838738
175481
708024 V
20.5739
79.4261
6092124…
Draw the product of the reaction shown below. Ignore small byproducts that would evaporate please.
Relative Abundance
20-
Problems
501
(b) The infrared spectrum has a medium-intensity peak at about 1650 cm. There is also a
C-H out-of-plane bending peak near 880 cm.
100-
80-
56
41
69
M(84)
LL
15 20 25
30
35
55 60 65 70
75
80
85 90
m/z
Chapter 12 Solutions
Pearson eText Basic Chemistry -- Instant Access (Pearson+)
Ch. 12.1 - Identify the solute and the solvent in each...Ch. 12.1 - Identify the solute and the solvent in each...Ch. 12.1 - Describe the formation of an aqueous KI solution,...Ch. 12.1 - Prob. 4PPCh. 12.1 - Water is a polar solvent and carbon tetrachloride...Ch. 12.1 - Water is a polar solvent and hexane (C6H14) is a...Ch. 12.2 - KF is a strong electrolyte, and HF is a weak...Ch. 12.2 - Prob. 8PPCh. 12.2 - Prob. 9PPCh. 12.2 - Prob. 10PP
Ch. 12.2 - Indicate whether aqueous solutions of each of the...Ch. 12.2 - Prob. 12PPCh. 12.2 - Classify the solute represented in each of the...Ch. 12.2 - Prob. 14PPCh. 12.3 - Prob. 15PPCh. 12.3 - State whether each of the following refers to a...Ch. 12.3 - Prob. 17PPCh. 12.3 - Prob. 18PPCh. 12.3 - A solution containing 80.g of KCl in 200.g of H2O...Ch. 12.3 - A solution containing 80.g of NaNO3 in 75g of H2O...Ch. 12.3 - Prob. 21PPCh. 12.3 - Prob. 22PPCh. 12.3 - Prob. 23PPCh. 12.3 - Prob. 24PPCh. 12.3 - Prob. 25PPCh. 12.3 - Determine whether a solid forms when solutions...Ch. 12.4 - What is the difference between a 5.00(m/m) glucose...Ch. 12.4 - What is the difference between a 10.0 (v/v)...Ch. 12.4 - Calculate the mass percent (m/m) for the solute in...Ch. 12.4 - Calculate the mass percent (m/m) for the solute in...Ch. 12.4 - Calculate the mass/volume percent (m/v) for the...Ch. 12.4 - Calculate the mass/volume percent (m/v) for the...Ch. 12.4 - Prob. 33PPCh. 12.4 - Calculate the grams or milliliters of solute...Ch. 12.4 - Prob. 35PPCh. 12.4 - Prob. 36PPCh. 12.4 - Prob. 37PPCh. 12.4 - For each of the following solutions, calculate...Ch. 12.4 - Prob. 39PPCh. 12.4 - Prob. 40PPCh. 12.4 - Prob. 41PPCh. 12.4 - Prob. 42PPCh. 12.4 - For each of the following solutions, calculate...Ch. 12.4 - For each of the following solutions, calculate...Ch. 12.4 - Calculate the volume, in milliliters, for each of...Ch. 12.4 - Prob. 46PPCh. 12.4 - Prob. 47PPCh. 12.4 - Prob. 48PPCh. 12.4 - A patient needs 100.g of glucose in the next 12h ....Ch. 12.4 - A patient received 2.0g of NaCl in 8h . How many...Ch. 12.5 - Prob. 51PPCh. 12.5 - A can of frozen lemonade calls for the addition of...Ch. 12.5 - Prob. 53PPCh. 12.5 - Prob. 54PPCh. 12.5 - Determine the final volume, in milliliters, of...Ch. 12.5 - Determine the final volume, in milliliters, of...Ch. 12.5 - Prob. 57PPCh. 12.5 - Prob. 58PPCh. 12.5 - Prob. 59PPCh. 12.5 - Prob. 60PPCh. 12.6 - Prob. 61PPCh. 12.6 - Prob. 62PPCh. 12.6 - Answer the following for the reaction:...Ch. 12.6 - Prob. 64PPCh. 12.6 - Prob. 65PPCh. 12.6 - Answer the following for the reaction:...Ch. 12.7 - Prob. 67PPCh. 12.7 - Prob. 68PPCh. 12.7 - Prob. 69PPCh. 12.7 - Prob. 70PPCh. 12.7 - Prob. 71PPCh. 12.7 - Prob. 72PPCh. 12.7 - Prob. 73PPCh. 12.7 - In each pair, identify the solution that will have...Ch. 12.8 - A 10(m/v) starch solution is separated from a...Ch. 12.8 - A 0.1(m/v) albumin solution is separated from a...Ch. 12.8 - Indicate the compartment (A or B) that will...Ch. 12.8 - Prob. 78PPCh. 12.8 - Prob. 79PPCh. 12.8 - Will a red blood cell undergo crenation,...Ch. 12.8 - Prob. 81PPCh. 12.8 - Each of the following mixtures is placed in a...Ch. 12.8 - Prob. 83PPCh. 12.8 - Prob. 84PPCh. 12.8 - Prob. 85PPCh. 12.8 - Prob. 86PPCh. 12 - The chapter sections to review are shown in...Ch. 12 - Prob. 88UTCCh. 12 - The chapter sections to review are shown in...Ch. 12 - Prob. 90UTCCh. 12 - Prob. 91UTCCh. 12 - Prob. 92UTCCh. 12 - Prob. 93UTCCh. 12 - Prob. 94UTCCh. 12 - Prob. 95UTCCh. 12 - Prob. 96UTCCh. 12 - Why does iodine dissolve in hexane, but not in...Ch. 12 - How do temperature and pressure affect the...Ch. 12 - Prob. 99APPCh. 12 - Prob. 100APPCh. 12 - Prob. 101APPCh. 12 - Prob. 102APPCh. 12 - Prob. 103APPCh. 12 - Write the net ionic equation to show the formation...Ch. 12 - Prob. 105APPCh. 12 - Prob. 106APPCh. 12 - Calculate the mass percent (m/m) of a solution...Ch. 12 - Calculate the mass percent (m/m) of a solution...Ch. 12 - How many milliliters of a 12 (v/v) propyl alcohol...Ch. 12 - Prob. 110APPCh. 12 - Prob. 111APPCh. 12 - Prob. 112APPCh. 12 - Prob. 113APPCh. 12 - Prob. 114APPCh. 12 - Prob. 115APPCh. 12 - Prob. 116APPCh. 12 - Prob. 117APPCh. 12 - How many liters of a 4.00MNaCl solution will...Ch. 12 - How many grams of solute are in each of the...Ch. 12 - Prob. 120APPCh. 12 - Prob. 121APPCh. 12 - Prob. 122APPCh. 12 - Prob. 123APPCh. 12 - Prob. 124APPCh. 12 - Prob. 125APPCh. 12 - Prob. 126APPCh. 12 - Prob. 127APPCh. 12 - Prob. 128APPCh. 12 - Prob. 129APPCh. 12 - Prob. 130APPCh. 12 - Prob. 131APPCh. 12 - Prob. 132APPCh. 12 - Prob. 133CPCh. 12 - Prob. 134CPCh. 12 - Prob. 135CPCh. 12 - Prob. 136CPCh. 12 - Prob. 137CPCh. 12 - Prob. 138CPCh. 12 - Prob. 139CPCh. 12 - Prob. 140CPCh. 12 - Prob. 141CPCh. 12 - Prob. 142CPCh. 12 - Prob. 143CPCh. 12 - Prob. 144CPCh. 12 - Prob. 145CPCh. 12 - Prob. 146CPCh. 12 - The following problems are related to the topics...Ch. 12 - Prob. 148CP
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