Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Chapter 16, Problem 79E
Interpretation Introduction
Interpretation: A series of chemicals are given to be added to
Concept introduction: Solubility is defined as the maximum amount of solute that can dissolve at a certain amount of solvent at certain temperature.
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Write the balanced chemical equation for each of the reactions. Include phases.
When aqueous sodium hydroxide is added to a solution containing lead(II) nitrate, a solid precipitate forms.
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However, when additional aqueous hydroxide is added, the precipitate redissolves, forming a soluble [Pb(OH)41²¯(aq)
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Write the balanced chemical equation for each of the reactions. Include phases.
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equation:
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When a strong base is added to a solution of CuSO4, which is pale blue, a precipitate forms and the
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menu of the answer module. Include phases in the balanced chemical equation. Click on the
(aq) button in the tools to select the phase to add. Phases should not be subscripted.
Chapter 16 Solutions
Chemistry
Ch. 16 - To what reaction does the solubility product...Ch. 16 - Under what circumstances can you compare the...Ch. 16 - What is a common ion and how does its presence...Ch. 16 - List some salts whose solubility increases as the...Ch. 16 - What is the difference between the ion product, Q,...Ch. 16 - Mixtures of metal ions in aqueous solution can...Ch. 16 - Prob. 7RQCh. 16 - What is a complex ion? The stepwise formation...Ch. 16 - When 5 M ammonia is added to a solution containing...Ch. 16 - Figure 15-3 outlines the classic scheme for...
Ch. 16 - Which of the following will affect the total...Ch. 16 - Prob. 2ALQCh. 16 - You are browsing through the Handbook of...Ch. 16 - A friend tells you: The constant Ksp of a salt is...Ch. 16 - Explain the following phenomenon: You have a test...Ch. 16 - What happens to the Ksp value of a solid as the...Ch. 16 - Which is more likely to dissolve in an acidic...Ch. 16 - Two different compounds have about the same molar...Ch. 16 - Sodium chloride is listed in the solubility rules...Ch. 16 - For which of the following is the Ksp value of the...Ch. 16 - Ag2S(s) has a larger molar solubility than CuS...Ch. 16 - Solubility is an equilibrium position, whereas Ksp...Ch. 16 - Prob. 13QCh. 16 - Prob. 14QCh. 16 - The common ion effect for ionic solids (salts) is...Ch. 16 - Sulfide precipitates are generally grouped as...Ch. 16 - List some ways one can increase the solubility of...Ch. 16 - The solubility of PbCl2 increases with an increase...Ch. 16 - You have two salts, AgX and AgY, both with very...Ch. 16 - The stepwise formation constants for a complex ion...Ch. 16 - Silver chloride dissolves readily in 2 M NH3 but...Ch. 16 - If a solution contains either Pb2+(aq) or Ag+(aq),...Ch. 16 - Write balanced equations for the dissolution...Ch. 16 - Write balanced equations for the dissolution...Ch. 16 - Prob. 25ECh. 16 - Use the following data to calculate the Ksp value...Ch. 16 - Approximately 0.14 g nickel(II) hydroxide,...Ch. 16 - The solubility of the ionic compound M2X3, having...Ch. 16 - The concentration of Pb2+ in a solution saturated...Ch. 16 - The concentration of Ag+ in a solution saturated...Ch. 16 - Calculate the solubility of each of the following...Ch. 16 - Calculate the solubility of each of the following...Ch. 16 - Cream of tartar, a common ingredient in cooking,...Ch. 16 - Barium sulfate is a contrast agent for X-ray scans...Ch. 16 - Calculate the molar solubility of Cd(OH)2, Ksp =...Ch. 16 - The solubility rules outlined in Chapter 4 say...Ch. 16 - Calculate the molar solubility of Al(OH)3, Ksp = 2...Ch. 16 - Calculate the molar solubility of Co(OH)3, Ksp =...Ch. 16 - For each of the following pairs of solids,...Ch. 16 - For each of the following pairs of solids,...Ch. 16 - Calculate the solubility (in moles per liter) of...Ch. 16 - Calculate the solubility of Co(OH)2(s) (Ksp = 2.5 ...Ch. 16 - The Ksp for silver sulfate (Ag2SO4) is 1.2 105....Ch. 16 - The Ksp for lead iodide (PbI2) is 1.4 108....Ch. 16 - Calculate the solubility of solid Ca3(PO4)2 (Ksp =...Ch. 16 - Calculate the solubility of solid Pb3(P04)2 (Ksp =...Ch. 16 - Prob. 47ECh. 16 - The solubility of Pb(IO3)(s) in a 0.10-M KIO3...Ch. 16 - Which of the substances in Exercises 27 and 28...Ch. 16 - For which salt in each of the following groups...Ch. 16 - What mass of ZnS (Ksp = 2.5 1022) will dissolve...Ch. 16 - The concentration of Mg2+ in seawater is 0.052 M....Ch. 16 - Will a precipitate form when 100.0 mL of 4.0 104...Ch. 16 - A solution contains 1.0 105 M Ag+ and 2.0 106 M...Ch. 16 - A solution is prepared by mixing 100.0 mL of 1.0 ...Ch. 16 - If 10.0 mL of 2.0 103 M Cr(NO3)3 is added to 10.0...Ch. 16 - Calculate the final concentrations of K+(aq),...Ch. 16 - A solution is prepared by mixing 75.0 mL of 0.020...Ch. 16 - A 50.0-mL sample of 0.00200 M AgNO3 is added to...Ch. 16 - Prob. 60ECh. 16 - A solution contains 1.0 105 M Na3PO4. What is the...Ch. 16 - A solution is 1 104 M in NaF, Na2S, and Na3PO4....Ch. 16 - A solution contains 0.25 M Ni(NO3)2 and 0.25 M...Ch. 16 - Write equations for the stepwise formation of each...Ch. 16 - Write equations for the stepwise formation of each...Ch. 16 - In the presence of CN, Fe3+ forms the complex ion...Ch. 16 - In the presence of NH3, Cu2+ forms the complex ion...Ch. 16 - Prob. 69ECh. 16 - Prob. 70ECh. 16 - The overall formation constant for HgI42 is 1.0 ...Ch. 16 - A solution is prepared by adding 0.10 mole of...Ch. 16 - A solution is formed by mixing 50.0 mL of 10.0 M...Ch. 16 - A solution is prepared by mixing 100.0 mL of 1.0 ...Ch. 16 - a. Calculate the molar solubility of AgI in pure...Ch. 16 - Solutions of sodium thiosulfate are used to...Ch. 16 - Kf for the complex ion Ag(NH3)2+ is 1.7 107. Ksp...Ch. 16 - Prob. 78ECh. 16 - Prob. 79ECh. 16 - The solubility of copper(II) hydroxide in water...Ch. 16 - A solution contains 0.018 mole each of I, Br, and...Ch. 16 - Magnesium hydroxide, Mg(OH)2, is the active...Ch. 16 - Tooth enamel is composed of the mineral...Ch. 16 - The U.S. Public Health Service recommends the...Ch. 16 - What mass of Ca(NO3)2 must be added to 1.0 L of a...Ch. 16 - Calculate the mass of manganese hydroxide present...Ch. 16 - Prob. 87AECh. 16 - The active ingredient of Pepto-Bismol is the...Ch. 16 - Consider saturated solutions of die following...Ch. 16 - Silver cyanide (AgCN) is an insoluble sail with...Ch. 16 - Nanotechnology has become an important field, with...Ch. 16 - The equilibrium constant for the following...Ch. 16 - Calculate the concentration of Pb2+ in each of the...Ch. 16 - Will a precipitate of Cd(OH)2 form if 1.0 mL of...Ch. 16 - a. Using the Ksp value for Cu(OH)2 (1.6 1019) and...Ch. 16 - Describe how you could separate the ions in each...Ch. 16 - Nitrate salts are generally considered to be...Ch. 16 - In the chapter discussion of precipitate...Ch. 16 - Assuming that the solubility of Ca3(PO4)2(s) is...Ch. 16 - Order the following solids (ad) from least soluble...Ch. 16 - The Ksp for PbI2(s) 1.4 108. Calculate the...Ch. 16 - The solubility of Pb(IO3)2(s) in a 7.2 102-M KIO3...Ch. 16 - A 50.0-mL sample of 0.0413 M AgNO3(aq) is added to...Ch. 16 - Prob. 105CPCh. 16 - Prob. 106CPCh. 16 - a. Calculate the molar solubility of AgBr in pure...Ch. 16 - Calculate the equilibrium concentrations of NH3,...Ch. 16 - Calculate the solubility of AgCN(s) (Ksp = 2.2 ...Ch. 16 - Calcium oxalate (CaC2O4) is relatively insoluble...Ch. 16 - The salt MX has a solubility of 3.17 108 mol/L in...Ch. 16 - Consider 1.0 L of an aqueous solution that...Ch. 16 - A solution saturated with a salt of the type M3X2...Ch. 16 - What mass of Ca(NO3O)2 must be added to 1.0 L of a...Ch. 16 - The Ksp for Q, a slightly soluble ionic compound...Ch. 16 - Aluminium ions react with the hydroxide ion to...
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- Solve correctly please. (Gpt/ai wrong answer not allowed)arrow_forwardWrite the balanced chemical equation for each of the reactions. Include phases. When aqueous sodium hydroxide is added to a solution containing lead(II) nitrate, a solid precipitate forms. equation:However, when additional aqueous hydroxide is added, the precipitate redissolves, forming a soluble [Pb(OH)4]2−(aq) complex ion.equation:arrow_forwarda three step process is required in order to determine the concentration of NO3- in a basic solution: 1) Zinc metal reduces Nitrate ions into ammonia in basic environments2) the ammonia is transferred to a solution with a known excess of HCl3) the unreacted HCL is titrated with NaOH A) write a balanced equation for each process B) a 25.00ml basic Solution containing an unknown concentration of NO3- was treated with zinc metal, the ammonia gas from the reaction was reacted with a 50ml solution of 2.5*10^-3M of HCl, the remaining unreacted HCL was then titrated to the stochiometric point with 28.22ml of 1.5*10^-3 NaOHWhat is the molar concentration of NO3- in the original solution?arrow_forward
- Analyze the table of some common inorganic precipitating agents and answer the following questions: Zn and Sn ions coprecipitate when they exist in solution to form mixed oxides. Suggest a precipitating agent that precipitate one of the oxides a. only A silver chloride precipitate is precipitated in gravimetric analysis. Which solution would you recommend to wash the precipitate: AGNO3 or HNO3. Justify your answer. b. Precipitating Element precipitated agent NH3(aq) Be (BeO), Al (A12O3), Sc(Sc203), Cr (Cr203), Fe (Fe203) Ga (Ga2O3), Zr (Zr02), In (In2O3), Sn (SnO2), U (U3O8) H2S Cu (CuO), Zn (ZnO or Zn2O4), Ge (GeO), As (As203 or As205), Mo (Mo03), Sn (SnO2), Sb (Sb2O3 or Sb2O5) (NH4)2S Hg (HgS), Co (Co304) (NH4);HPO4 Mg (Mg2P2O7), Al (AIPO4), Mn (Mn2P2O7), Zn (Zn2P2O7), Zr (Z12P207), Cd (Cd2P207), Bi (BİP04) H2SO4 Li, Mn, Sr, Cd, Pb, Ba (all as sulfates) H;C¿O4 Ca (СаО), Sr (SrO), Th (ThО2) HCI Ag (AgCl), Hg (Hg2C12), Na (NaCl), Si (SiO2) AGNO3 CI (A£CI), Br (AgBr), I (Agl) (NH4);CO3…arrow_forwardConsider the insoluble compound silver iodide , AgI . The silver ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of AgI (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction.For Ag(NH3)2+ , Kf = 1.6×107 . Be sure to specify states such as (aq) or (s). + + K =arrow_forwardCalculate the equilibrium concentration of Zn2+(aq) in a solution that is initially 0.150 M Zn(NO3)2 and 0.800 M NH3. The formation constant for [Zn(NH3)4]2+(aq) is Kf = 2.8 × 109.arrow_forward
- provide explanation of formula.arrow_forwardConsider the insoluble compound zinc carbonate, ZnCO3. The zinc ion also forms a complex with hydroxide ions. Write a balanced net ionic equation to show why the solubility of ZnCO3 (s) in presence of hydroxide ions and calculate the equilibrium constant for this reaction. For Zn(OH)42, K₁= 2.9x1015. Be sure to specify states such as (aq) or (s). K=arrow_forwardConsider the insoluble compound silver chloride , AgCl . The silver ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of AgCl (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction.For Ag(NH3)2+ , Kf = 1.6×107 . Be sure to specify states such as (aq) or (s). + + K =arrow_forward
- An aqueous solution is prepared in which 0.00113 mol Ni(NO3)2 and 0.484 mol NH3 are dissolved in a total volume of 1.00 L. Kf for Ni(NH3)62+ is equal to 5.5 × 108. Calculate the concentration of Ni(H2O)62+ ions at equilibrium in the solution formedarrow_forward1) Explain why you can dissolve Ni(OH)2 in aqueous ammonia. 2) Explain how the reaction of Ni(OH)2 with NH3 would enable you to separate a mixture of iron(III) 3) Could you use excess NaOH to separate a mixture of the precipitates of Fe(OH)3 and Ni(OH)2? Explain why or why not.arrow_forward13arrow_forward
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