Use the table of solubility rules for ionic compounds in water to predict whether each of the following ionic compounds is soluble in water or not using the dropdown on the right. Table of Solubility Rules for lonic Compounds in Water An ionic compound is soluble in water if it contains one of the following: Positive lons: Lit, Na", K*, Rb*, Cs*, NH,* Negative lons: NO,", C,H;O," Cr, Br", I except when combined with Ag*, Pb*, or Hg,+ So, except when combined with Ba*, Pb*, Ca, Sr, or Hg,? 2+ lonic compounds that do not contain at least one of these ions are usually insoluble. Nal [Choose] [Choose] soluble in water PbS NOT soluble in water AgCI [ Choose ] LICI [ Choose ] FeO [ Choose] КОН [Choose]

Use the table of solubility rules for ionic compounds in water to predict whether each of the following ionic compounds is soluble in water or not using the dropdown on the right. Table of Solubility Rules for lonic Compounds in Water An ionic compound is soluble in water if it contains one of the following: Positive lons: Lit, Na", K, Rb, Cs, NH, Negative lons: NO,", C,H;O," Cr, Br", I except when combined with Ag, Pb, or Hg,+ So, except when combined with Ba, Pb, Ca, Sr, or Hg,? 2+ lonic compounds that do not contain at least one of these ions are usually insoluble. Nal [Choose] [Choose] soluble in water PbS NOT soluble in water AgCI [ Choose ] LICI [ Choose ] FeO [ Choose] КОН [Choose]

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A chemist combines 53.9 mL of 0.372 M potassium bromide with 23.1 mL of 0.451 M silver nitrate. (a) How many grams of silver bromide will precipitate? (b) What is the final molarity of the K* ion? (c) What is the final molarity of the silver or bromide ion, whichever one is in excess? (а) g AgBr (b) M K* (c) Мехсess ion
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You mix aqueous solutions of 100.0 mL 1.70 M NaCl and 75.o mL 1.20 M Pb(NO3)2, calculate the mass of of precipitate formed.
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A chemist combines 53.5 mL of 0.350 M potassium bromide with 23.9 mL of 0.533 M lead nitrate. (a) How many grams of lead bromide will precipitate? (b) What is the final molarity of the K* ion? (c) What is the final molarity of the lead or bromide ion, whichever one is in excess? (а) g PbBr2 (b) M Kt (c) Мехсess ion
Which of the following statements is true with respect to the solubility of ionic compounds? A) Carbonate containing compounds are soluble, except for those containing group I elements, which are insoluble O B) All compounds that contain chloride, bromide, or iodide anions are soluble C) Silver nitrate is an insoluble compound D) Although most sulfate-containing compounds are soluble, barium sulfate is not E) Silver chloride is a soluble compound
Metal ions can be separated from a mixture by a selective precipitation. The technique involves adding a series of aqueous solutions that will selectively precinitate one of the fons A solution X contains the following substances given in the schematic representation: KNO: (al • Pb(NO1)2 (a • Cu(NOa)2 () • Ba(NO3)z (a KNO, Ba(NO,)ı (aq SOLUTION X The following solutions given below added to SOLUTION X senerntely and also in the given order: KCI () K.SO () K:CO ta a) Show that after the addition of all the solutions listed above will leave only one substance in the solution (not precipitated) and name that substance. b) Write the balonced molecular eanation and net-lonie equation for the reactions occuring after the addition off each solutions to the SOLUTION X.
Table 1 - Solubility rules for ionic compounds in water Soluble Compounds 1. All alkali metal components (Group IA) are soluble. 2. All salts containing NH4+1, NO3-1, ClO4-1, ClO3-1 and C2H3O2-1 (acetate) are soluble. 3. All chlorides, bromides and iodides (Cl-1, Br-1 and I-1 respectively) are soluble except when combined with Ag+1, Pb2+ and Hg22+. 4. All sulfates (SO42-) are soluble except when combined with Pb2+, Ca2+, Sr2+, Hg22+ and Ba2+. Insoluble Compounds 5. All metal hydroxides and all metal oxides are insoluble except those in Group IA and those formed by Ca2+, Sr2+ and Ba2+. When metal oxides dissolve, they react with water to form hydrates. The oxide ion (O2-) does not exist in water. For example: Na2O(s) + H2O → 2 NaOH(aq) 6. All salts containing PO43-, CO32-, SO32-, and S2- are insoluble, except those in Group IA and NH4+1. Table 2 - Gases formed in metathesis reactions Gas Equation for formation H2S 2H+1 + S2- → H2S(g) CO2 2H+1 + CO32- → (H2CO3) →…
2. How many ml of 0.280 M barium nitrate are required to precipitate as barium sulfate all the sulfate ions from 25.0 ml of 0.350 M aluminum sulfate? Ba(NO,)l1ag) + Al:(So.)t4) 0 Baso4) + AI(NO,)a{a9)
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Some compounds are soluble in water and some compounds are insoluble in water. For each compound below determine if the compound if soluble or insoluble in water. * Soluble Insoluble Mg(NO:): Agcl LIOH Mg:(PO.):
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