Question

4.30. Using solubility rules, predict the solubility in water of the following ionic compounds. a. AI(OH) b. CaN C. NH4CI d. KOH 4.32. Using solubility rules, decide whether the following ionic solids are soluble or insoluble in water. If they are soluble, write the chemical equation for dissolving in water and indicate what ions you would expect to be present in solution. (NE SO b. BaCO c. Pb(NOs)2 d. Ca(OH) 4.34. Write net ionic equations for the following molecular equations. is a strong electrolyte. a. HBr(on)+NHs(a)-+NE,Br(ae) G Pb(NOs)(a) +2NaBr(aa)PbBr(o)+2NaNOs (aa) 4.36. Lithium carbonate solution reacts with aqueous hydrobromic acid to give a solution of lithium bromide, carbon dioxide gas, and water. Write the molecular equation and the net ionic equation for the reaction. 4.38. Write the molecular equation and the net ionic equation for each of the following aqueous reactions. If no reaction occurs, write NR after the arrow. a. AgNO, + Nal+ that 4.40. For each of the following, write molecular and net ionic equations for any precipitation reaction occurs. If no reaction occurs, indicate this. a. Zinc chloride and sodium sulfide are dissolved in water b. Sodium sulfide and calcium chloride are dissolved in water. c. Magnesium sulfate and potassium bromide are dissolved in water d. Magnesium sulfate and potassium carbonate are dissolved in water 4.42. Classify each of the following as a strong or weak acid or base. a. NH b. HCNO c Mg(OH) 4.44. Complete and balance each of the following molecular equations (in aqueous solution), inel phase labels. Then, for each, write the net ionic equation. include a. Al(OH)s +HCI b. HCO+Sr(OH), → d. H2SO4 +KOH- 4.46. For each of the following, write the molecular equation, including phase labels. Then write the net ionic equation. Note that the salts formed in these reactions are soluble a. the neutralization of lithium hydroxide solution by aqueous chloric acid b. the reaction of barium hydroxide solution and aqueous nitrous acid c. the reaction of sodium hydroxide solution and aqueous nitrous acid d. the neutralization of aqueous hydrogen cyanide by aqueous strontium hydroxide 4.48. Complete the right side of each of the following molecular equations. Then write the net ionic equations. Assume all salts formed are soluble. Acid salts are possible. b. 2H, POs(ag)+Ca(OH)2(4) d. Sr(OH)2 (aq)+ 2H COs(a4)+ 4.50. Write molecular and net ionic equations for the successive neutralizations of each acidic hydrogen of phosphoric acid by calcium hydroxide solution. Calcium phosphate is insoluble; assume that the acid salts are soluble. 4.52. The following reactions occur in aqueous solution. Complete and balance the molecular equations using phase labels. Then write the net ionic equations. a. BaCOs +HNO 4.54. Write the molecular equation and the net ionic equation for the reaction of solid barium carbonate and hydrogen bromide in aqueous solution. Add phase labels. the oxidation number for the element noted in each of the following a. CrinCrOg b. Hg in HgC c. Ga in Ga(OH) d. P in NagPO er 4.58. Obtain the oxidation a. N in N b. Cr in Cros c. Zn in Zn(OH), d. As in Ha AsO, 4.60. Determine the oxidation numbers of all the elements in each of the following compounds. (Hint Look at the ions present.) b. Cr(S04) c. CoSeO d. Pb(OH) 4.62. In the following reactions, label the oxidizing agent and the reducing agent a. Zn0(o)+C(o) Zm(g)+CO(g) 4.64. In the following reactions, label the oxidizing agent and the reducing agent a. Fe20s(o) +3CO(9) 2Fe(o) +3C02(9) b. PbS(o)+4H02(aa)Pbso4()+4H,0() 4.66. Balance the following oxidation-reduction reactions by the half-reaction method. a. Fels (aq) + Mg(s) → Fe(s) + Mg, (ag) b. Ha(a) + Ag (aq)Ag(o)+H (aa) 6s. 4 00 -l, volume of AgNo, solution contains 00345 mol AgNO, Giver mitae),What is the molarity of the solution? 4.70. A samp is then filled to the mark with water. What is the molarity of the solution? ple of oxalic acid, H.C.04, weighing 1.200 g is placed in a 100.0-mL volumetric flask, which 4.72. How many milliliters of 0.126 M HCIO4 (perchloric acid) are required to give 0.150 mol HCIO? 4.74. What is the volume (in milliliters) of H2SO4 (sulfuric acid) containing 0.949 g H:SO4? 4.76. Insulin is a hormone that controls the use of glucose in the body. How many moles of insulin are required to make up 28 mL. of 0.0048 M insulin solution? 4.78. Describe how you would prepare 2.50 x 102 mL of O.50 M NazSO4. What mass (in grams) of sodium sulfate, Na SO4, is needed? 4.80. A chemist wants to prepare 0.75 M HCI. Commercial hydrochloric acid is 12.4 M. How many milliliters of the commercial acid does the chemist require to make up 1.50 L of the dilute acid? ion that results from mixing 50.0 mL of a 0.20 M NaCIo, (aq) solution with 25.0 ml. of a 0.20 M Na:SO. (aq) solution. Assume that the volumes are additive. 4.84. A soluble iodide was dissolved in water. Then an excess of silver nitrate, AgNOs, was precipitate all of the iodide ion as silver iodide, Agl. 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? added to 4.86. Gold has compounds containing goldD) ion or gold(II) ion. A compound of gold and chlorine was treated with a solution of silver nitrate, AgNOs, to convert the chloride ion in the compound precipitate of AgCI. A 162.7-mg sample of the gold compound gave 100.3 mg AgCI. Calculate the percentage of the chlorine in the gold compound. a. Decide whether the formula of the compound is AuCl or AuCls. b. 4.88. A 1.34S-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, BaCrOa. What is the formula of the compound? 4.90. A flask contains 49.8 mL of 0.150 M Ca(OH)2 (calcium hydroxide). How many milliliters of Na COs (sodium carbonate) are required to react completely with the calcium hydroxide in the following reaction? Na:COs (aq)+ Ca(OH)2 (aq) > CaCOs (s)+ 2NaOH (aq) 4.92. How many milliliters of 0.250 M KMnO, are needed to react with 3.55 g of iron(II) sulfate, FeSO4? The reaction is as follows 10 FeSO4(aq)+ 2 KMn04(aq) +3 H SO4(aq)->5 Fe2(SO4)s(aq) +2 MnSO4(aq) + K2S04(aq) + 8 H20() 4.94. A 3.75-g sample of iron ore is transformed to a solution of iron (II) sulfate, FeS04, and this solution is titrated with 0.150 M K2Cr207 (potassium dichromate). If it requires 43.7 mL of potassium dichromate solution to titrate the iron (II) sulfate solution, what is the percentage of iron in the ore? The reaction is 6FeSO4(aq) + K Cr.O(aq)+ 7 H-SO(aq)3Fez(SO)s(aq)+ Cr(SO4)(aq)+ 7 H201)+ K:S0(aq)

Answer 1

4.30)

a)

Hydroxide salts of transition metals and Al³⁺ are insoluble. So Al(OH)₃ are not soluble

b)

Ca₃N₂ is soluble due to presence of Ca²⁺ ions.

c)

All compounds containing NH₄⁺ ions are soluble and Cl^- ions are also soluble. So, NH₄Cl is soluble.

d)

Generally, OH^- are insoluble but K⁺ions are exceptions.So KOH is soluble.