(a)
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: 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: 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: 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: 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.
Want to see the full answer?
Check out a sample textbook solutionChapter 12 Solutions
Basic Chemistry
- Calcium carbonate, CaCO3, can be obtained in a very pure state. Standard solutions of calcium ion are usually prepared by dissolving calcium carbonate in acid. What mass of CaCO3 should be taken to prepare 500. mL of 0.0200 M calcium ion solution?arrow_forwardVitamin C has the formula C6H8O6. Besides being an acid, it is a reducing agent. One method for determining the amount of vitamin C in a sample is to titrate it with a solution of bromine, Br2, an oxidizing agent. C6H8O6(aq) + Br2(aq) 2 HBr(aq) + C6H6O6(aq) A 1.00-g "chewable" vitamin C tablet requires 27.85 ml of 0.102 M Br2 for titration to the equivalence point. What is the mass of vitamin C in the tablet?arrow_forwardAn experiment in a general chemistry laboratory calls for a 2.00-M solution of HCl. How many mL of 11.9 M HCl would be required to make 250 mL of 2.00 M HCl?arrow_forward
- 95. Many metal ions form insoluble sulfide compounds when a solution of the metal ion is treated with hydrogen sulfide gas. For example, nickel(II) precipitates nearly quantitatively as NiS when H2S gas is bubbled through a nickel ion solution. How many milliliters of gaseous H2S at STP are needed to precipitate all (he nickel ion present in 10. mL of 0.050 M NiCl2 solution?arrow_forward. Which of the following will affect the total amount of solute that can dissolve in a given amount of solvent? a. The solution is stirred. b. The solute is ground to line particles before dissolving. c. The temperature changes.arrow_forwardAn experiment calls for 100. mL of 1.25 M HC1. All that is available in the lab is a bottle of concentrated HC1, whose label indicates that it is 12.1 M. How much of the concentrated HC1 would be needed to prepare the desired solution?arrow_forward
- Label each ionic compound as either "soluble" or "insoluble" in water: a. BaSO4 b. Na2CrO4 c. Cu3(PO4)2arrow_forwardSuppose that 15.0 ml of 0.0250M aqueous H,SO4 is required to neutralize 10.0 ml of an aqueous solution of KOH. What is the molarity of the KOH solution? A. 0.0167 M В. 0.0375 M C. 0.0333 M D 0.075 Marrow_forwardWhich of the following aqueous solutions, if any, is expected to be comprised essentially of all ions from the solute rather than a mixture of ions and molecules, or just molecules ? A. a solution of acetic acid B. a solution of sodium chloride C. a solution of nitric acid D. a solution of glucose, C6H12O6arrow_forward
- What is the molarity of a solution that contains 7.07mol of Ba(OH), dissolved in 5.40L of water? ОА. 1.31М В. 16.6M C. 1.76M D. 0.569Marrow_forwardA 2.50 L solution contains 5.00g of NaOH(M.W 40.00g/mol). is the molarity (M) of sodium hydroxide in the solution? a) 0.0500 M b) 3.20 M c)0.500 M d) 2.00 M e)1.00 Marrow_forwardWhat mass of sodium hydroxide (NaOH, molar mass = 40.0 g-mol-1) is needed to make 100.0 mL of a 0.125 M NaOH solution? O A. 5.00 g O B. 0.0500 g O C. 3.13 g O D. 0.500 garrow_forward
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxIntroductory Chemistry: A FoundationChemistryISBN:9781285199030Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning