Chemistry
9th Edition
ISBN: 9781133611097
Author: Steven S. Zumdahl
Publisher: Cengage Learning
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Chapter 16, Problem 81AE
Interpretation Introduction
Interpretation:
The mass of
Concept introduction:
Solubility is defined as the maximum amount of solute that can dissolve at a certain amount of solvent at certain temperature. The solubility product,
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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 - 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. 11QCh. 16 - Prob. 12QCh. 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 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. 21ECh. 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 Mg (OH)2, Ksp =...Ch. 16 - Prob. 32ECh. 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. 43ECh. 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 - Prob. 52ECh. 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. 56ECh. 16 - A solution contains 1.0 105 M Na3PO4. What is the...Ch. 16 - The Ksp of Al(OH)3 is 2 1032. At what pH will a...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. 65ECh. 16 - Prob. 66ECh. 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. 74ECh. 16 - Prob. 75ECh. 16 - The solubility of copper(II) hydroxide in water...Ch. 16 - A solution contains 0.018 mole each of I, Br, and...Ch. 16 - You have two salts, AgX and AgY, with very similar...Ch. 16 - Tooth enamel is composed of the mineral...Ch. 16 - The U.S. Public Health Service recommends the...Ch. 16 - Prob. 81AECh. 16 - Calculate the mass of manganese hydroxide present...Ch. 16 - Prob. 83AECh. 16 - The active ingredient of Pepto-Bismol is the...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 - The solubility rules outlined in Chapter 4 say...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. 99CPCh. 16 - Prob. 100CPCh. 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 - A solution saturated with a salt of the type M3X2...Ch. 16 - Consider 1.0 L of an aqueous solution that...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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Similar questions
- What mass of Ca(NO3)2 must be added to 1.0 L of a 1.0-M HF solution to begin precipitation of CaF2(s)? For CaF2, Ksp = 4.0 1011 and Ka for HF = 7.2 104. Assume no volume change on addition of Ca(NO3)2(s).arrow_forwardCalculate the molar solubility of X(OH)3 within water. Ksp X(OH)3 = 8.3 x 10–34 2.6 x 10–9 M 1.7 x 10–17 M 2.4 x 10–9 M 6.0 x 10–19 M 2.9 x 10–17 Marrow_forwardCalculate the solubility of AgCl in: Ksp = 1.6 × 10–10 a) 100.0 mL of 4.00 x 10-3 M calcium chloride. b) 100.0 mL of 4.00 x 10-3 M calcium nitrate.arrow_forward
- Which of the following is true in the determination of calcium hydroxide’s solubility and Ksp? a. The Ksp of Ca(OH)2 is unaffected by the presence of CaCl2. b. The solubility of Ca(OH)2 remains the same even in the presence of CaCl2. c. Saturated solution of Ca(OH)2 still forms a solution with the addition of CaCl2 at constant temperature. d. Saturated solution of Ca(OH)2 requires less hydrochloric acid to reach equivalence point compared to its solution that contains CaCl2.arrow_forwardThe Ksp values for AgCl and Mg(OH)2 respectively are 1.0 x 10-10 and 1.2 x 10-11. Which of these sparingly soluble salts is actually more soluble?arrow_forward1. Calculate the molar solubility of CaF2 at 25 degrees Celsius in 0.010 M Ca(NO3)2 solution. (Ksp = 3.1 x 10-5 M) 2. Determine the Ksp of mercury (I) bromide (Hg2Br2), given that its molar solubility is 2.52 x 10-8 mole per liter. 3. The value of Ksp of AgCl is 1.8 x 10-10. What would be the molar concentration of Ag+ and Cl- in AgCl in pure water placed in contact with solid AgCl(s)?arrow_forward
- 1 ) The density of a 5.26MNaHCO 3 (84.0 g/mol) is 1.19g / m * l . Its molality is 2) Calculate the pAg^ + at the equivalence point in the titration of 25.0ml of 0.0823 M Kl with 0.051M AgNO 3 . Ksp Agl=8.3*10^ -16 3) Commercial concentrated aqueous nitric acid is 70.4% HNO3(63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is 4) Consider the titration of 25ml of 0.0823M KI with 0.051M AGNO3, Kspagi =8.3x10-16 Calculate pAg* after adding 39.0 ml I03 Ag* + 103 ====AglO3 5) Commercial concentrated aqueous nitric acid is 70.4 1\%HNO 3 (63.0 g/mol) by mass and has a density of 1.41g / m * l . The molarity of this solution is: 6) What mass in g of Na 2 CO 3 [106 g/mol] is required to prepare 250 ml of 0.3M aqueous solution in Na^ + [23.g/mol] ? 7) Calculate pAg^ + after adding 42.30ml AgNO 3 In the titration of of 0.0823M Kl with 0.051M AgNO 3 . KspAgl = 8.3 * 10 ^ - 16 8) The milliliters of concentrated HClO 4 (100.5 g/mol),6 60% by mass,…arrow_forwardIn a hardness of water determination like the one performed in this experiment, it was found that a 25.00-mL sample of water required 12.25mL of 0.0128 M EDTA solution for complete titration. What is the concentration (molarity) of Ca2+ ions in the water sample? What is concentration of CaCO3 (in mg/L) in the water sample? Describe the hardness level of the water using the U.S. government standards.arrow_forward1. Compare the pH values of boiled and unboiled distilled H2O. 2. The Henderson-Hasselbalch equation relates the pH of a buffer to the relative concentrations of the buffercomponents. According to this equation, under which conditions is pH = pKa? 3. How does the concentration of the buffer affect the buffer capacity?arrow_forward
- Consider the dissolution of A(OH)2 in a medium with [OH-] = 0.15 M. Calculate the molar solubility of A(OH)2 in this medium.arrow_forwarda) The concentra=on of Mg2+ in seawater is 0.052 M. If the Ksp for Mg(OH)2 is 8.9 × 10–12, at what pH will >99.9% of the Mg2+ be precipitated from seawater as its hydroxide salt? b) The solubility of the ionic compound M2X3, having a molecular mass of 288 g/mol, is 3.60 × 10–7g/L. Calculate the Ksp of the compound.arrow_forwardA 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach the endpoint, a total of 20.2 mL of HNO₃ was required. How many moles of Ca(OH)2 had to be present in the initial reaction?arrow_forward
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