Concept explainers
Decide whether each of the following is water-soluble. If soluble, tell what ions are produced when the compound dissolves in water.
(a) NiCl2
(b) Cr(NO3)3
(c) Pb(NO3)2
(d) BaSO4
(a)
Interpretation:
Water solubility of the given compounds and ions produced by the compounds should be analyzed.
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
Almost all the salts of
Salts of F- are soluble. But some of the fluoride salt of
Salts of
Insoluble compounds in water:
Most of the salts of
Most of the metal hydroxides and oxides are insoluble in water bit some of the alkali metal hydroxides,
Answer to Problem 24PS
Water soluble compound. Produced ions are
Explanation of Solution
The given compound Nickel (II) chloride which is soluble in water.
(b)
Interpretation:
Water solubility of the given compounds and ions produced by the compounds should be analyzed.
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
Almost all the salts of
Salts of F- are soluble. But some of the fluoride salt of
Salts of
Insoluble compounds in water:
Most of the salts of
Most of the metal hydroxides and oxides are insoluble in water bit some of the alkali metal hydroxides,
Answer to Problem 24PS
Water soluble compound. Produced ions are
Explanation of Solution
The given compound is Chromium (III) nitrate which is soluble in water.
(c)
Interpretation:
Water solubility of the given compounds and ions produced by the compounds should be analyzed.
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
Almost all the salts of
Salts of F- are soluble. But some of the fluoride salt of
Salts of
Insoluble compounds in water:
Most of the salts of
Most of the metal hydroxides and oxides are insoluble in water bit some of the alkali metal hydroxides,
Answer to Problem 24PS
Water soluble compound. Produced ions are.
Explanation of Solution
The given compound is Lead (II) nitrate which is soluble in water.
(d)
Interpretation:
Water solubility of the given compounds and ions produced by the compounds should be analyzed.
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
Almost all the salts of
Salts of F- are soluble. But some of the fluoride salt of
Salts of
Insoluble compounds in water:
Most of the salts of
Most of the metal hydroxides and oxides are insoluble in water bit some of the alkali metal hydroxides,
Answer to Problem 24PS
This compound insoluble in water.
Explanation of Solution
The given compound is Barium sulfate which is insoluble in water.
Want to see more full solutions like this?
Chapter 3 Solutions
Chemistry & Chemical Reactivity
- A soluble iodide was dissolved in water. Then an excess of silver nitrate, AgNO3, was added to precipitate all of the iodide ion as silver iodide, AgI. If 1.545 g of the soluble iodide gave 2.185 g of silver iodide, how many grams of iodine are in the sample of soluble iodide? What is the mass percentage of iodine, I, in the compound?arrow_forward1. Sometimes a reaction can fall in more than one category. Into what category (or categories) does the reaction of Ba(OH)2(aq) + H+PO4(aq) fit? acid-base and oxidation-reduction oxidation-reduction acid-base and precipitation precipitationarrow_forwardA 1.345-g sample of a compound of barium and oxygen was dissolved in hydrochloric acid to give a solution of barium ion, which was then precipitated with an excess of potassium chromate to give 2.012 g of barium chromate, BaCrO4. What is the formula of the compound?arrow_forward
- Describe in words how you would prepare pure crystalline AgCl and NaNO3 from solid AgNO3 and solid NaCl.arrow_forward9. Which of the following solutions has the highest total concentration of ions? Explain how you got your answer. (a) 0.012 M Al2(SO4)3 (b) 0.030 M KCl (c) 0.020 M Al(NO3)3 (d) 0.025 M K2SO4arrow_forwardA solution is prepared by dissolving 2.95 g Co2(SO4)3 in enough water to make 1.00 L of red solution; the red color is due to the presence of the cobalt ions. To this solution was added 1.52 g of magnesium powder. A redox reaction occurred, in which the magnesium atoms lose all of their valence electrons and the red color of the solution fades. (a) Write the total reaction that occurs and the net ionic equation for the redox process. (Assume that one of the products of the redox reaction is a metal.) (b) Calculate the initial concentration of cobalt ions, the final concentration of cobalt ions, and the final concentration of magnesium ions.arrow_forward
- (NH4)2S is a soluble compound True Falsearrow_forward5.00 g of a mixture of sodium carbonate and potassium bromide was dissolved and made up to the mark in a 250. mL volumetric flask. 25.0 mL portions of this solution were neutralized by an average of 24.7 mL of 0.200 mol L-1 HCI. Find the percentage of sodium carbonate in the original 5.00 g sample of the mixture. (4) (Potassium bromide does not react with HCI) Na2CO3(aq) + 2HCI(aq) 2NaCl(aq) + H2O1) + CO2(g)arrow_forward13. Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction. (a) Cr2(SO4)3 (aq) + (NH4)2CO3 (aq) (b) Pb(NO3)2 (aq) + KOH (aq)arrow_forward
- Which of the following solutions will produce a precipitate when added to Na2SO4 solution? (A) Ba(NO3)2(aq) (B) Cu(NO3)2(aq) (C) Zn(NO3)2(aq) (D) All the abovearrow_forwardWhat is the net ionic equation of the reaction of BeCl 2 BeCl2 with NaOH NaOH ?arrow_forwardA stock solution of Cu(C2H302)2 has a concentration of 0.270 M. If 6.00 mL of this solution is transferred to a 50.00 mL flask and then diluted with distilled water, what is the final concentration of Cu2+ ions?arrow_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: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
- Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning