Basic Chemistry
6th Edition
ISBN: 9780134878119
Author: Timberlake, Karen C. , William
Publisher: Pearson,
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Chapter 12, Problem 133CP
(a)
Interpretation Introduction
Interpretation: The net ionic equation of the given reaction should be determined.
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: The net ionic equation of the given reaction should be determined.
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: The net ionic equation of the given reaction should be determined.
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: The net ionic equation of the given reaction should be determined.
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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Chapter 12 Solutions
Basic Chemistry
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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