General Chemistry: Principles and Modern Applications (11th Edition)
11th Edition
ISBN: 9780132931281
Author: Ralph H. Petrucci, F. Geoffrey Herring, Jeffry D. Madura, Carey Bissonnette
Publisher: PEARSON
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Chapter 18, Problem 16E
How would you expect the presence of the following solutes to affect the molar solubility of
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Because barium sulfate is opaque to X-rays, it is suspended in water and taken internally to make the gastrointestinal tract visible in an X-ray photograph. Although barium ion is quite toxic, barium sulfate’s Ksp of 1.1 x 10–10 gives it such low solubility that it can be safely consumed.
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Chapter 18 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
Ch. 18 - Write K10 expressions for the following...Ch. 18 - Write solubility equilibrium equations that are...Ch. 18 - The following K10 values ate found in a handbook....Ch. 18 - Calculate the aqueous solubility, in moles per...Ch. 18 - Prob. 5ECh. 18 - Which of the following saturated aqueous solutions...Ch. 18 - Fluoridated drinking water contains about 1 part...Ch. 18 - In the qualitative cation analysis procedure, Bi2+...Ch. 18 - Prob. 9ECh. 18 - A 725mL sample of a saturated solution of calcium...
Ch. 18 - A 25.00mL sample of a clear saturated solution of...Ch. 18 - A 250 mL sample of saturated CaC2O4 (aq) requires...Ch. 18 - Prob. 13ECh. 18 - Prob. 14ECh. 18 - Calculate the molar solubility of...Ch. 18 - How would you expect the presence of the following...Ch. 18 - Prob. 17ECh. 18 - Describe the effect of the salt NNO2 on the...Ch. 18 - A 0.150 M Na2SO4 , solution that is saturated with...Ch. 18 - It 100.0 mL of 0. 0025 U Na2SO4(aq) is saturated...Ch. 18 - What [Pb2+] should be maintained in Pb( NO2)2(aq)...Ch. 18 - What [l-] should be maintained in Kl(aq) to...Ch. 18 - Can the solubility of Ag2CrO4 be lowered to 5.0104...Ch. 18 - Prob. 24ECh. 18 - Prob. 25ECh. 18 - Prob. 26ECh. 18 - Will prectiation of MgF2(s) occur if a 22.5 mg...Ch. 18 - Will pbCl2 precitate when 155mL of 0.016M KCl(aq)...Ch. 18 - What is the minimum pH at which Cd(OH)2(s) will...Ch. 18 - What is the minimum pH at which Cr(OH)2(s) will...Ch. 18 - Will precipitation occur in the following cases?...Ch. 18 - Prob. 32ECh. 18 - Prob. 33ECh. 18 - Prob. 34ECh. 18 - When 200.0 ml. of 0 350 N K2CrO4(aq) are added to...Ch. 18 - What percentage of the original Ag4 remains in...Ch. 18 - Prob. 37ECh. 18 - The ancient Romans added calcium sulfate to wine...Ch. 18 - Prob. 39ECh. 18 - Prob. 40ECh. 18 - Kl(aq) is slowly added to a solution with...Ch. 18 - A solution is 0010 M en both CrO42- and SO42 . To...Ch. 18 - An aqueous solution that 200 U m AgNO2 slowly...Ch. 18 - AgNO2(aq) is slowly added to a solution that is...Ch. 18 - Which of the following solids is (are) more...Ch. 18 - Which of the blowing solids is (are) more soluble...Ch. 18 - The solubility of Mg(OH)2 m a particualr buffer...Ch. 18 - To 0.350L of 0.150MNH2 is added 0.150 L of 0.100 M...Ch. 18 - For the equilibrium...Ch. 18 - Will the following precipitates form under the...Ch. 18 - Prob. 51ECh. 18 - Prob. 52ECh. 18 - In a solution that is 0.0500M in [Cu( CN)4]2 and...Ch. 18 - Calculate [Cu2+] in a 0.10M CuSO4(aq) solution...Ch. 18 - Prob. 55ECh. 18 - A solution is 0.10 M in free NH2 ,0.10M in NH4Cl ,...Ch. 18 - A 0.10 mol sample of AgNO2(s) is dissolved in...Ch. 18 - A solution is prepared at has [NH2]=1.00M and...Ch. 18 - Prob. 59ECh. 18 - A solution is 0.05 U m Cu2+ in Hg2+ , and in Mn2+...Ch. 18 - Prob. 61ECh. 18 - Prob. 62ECh. 18 - Suppose you did a group 1 qualitative cation...Ch. 18 - Prob. 64ECh. 18 - Prob. 65ECh. 18 - Prob. 66ECh. 18 - Prob. 67IAECh. 18 - A handbook lists the solubility of CaHPO4 as 0.32g...Ch. 18 - Prob. 69IAECh. 18 - What percentage of the Ba2+ in solution is...Ch. 18 - Prob. 71IAECh. 18 - Prob. 72IAECh. 18 - Prob. 73IAECh. 18 - What is the solubility of MnS, in grams per liter,...Ch. 18 - Prob. 75IAECh. 18 - Prob. 76IAECh. 18 - Prob. 77IAECh. 18 - Prob. 78IAECh. 18 - Prob. 79IAECh. 18 - Prob. 80IAECh. 18 - Prob. 81IAECh. 18 - Prob. 82IAECh. 18 - Prob. 83IAECh. 18 - Prob. 84IAECh. 18 - A 2509 sample of Ag2SO4(s) added to a beaker...Ch. 18 - Prob. 86IAECh. 18 - Prob. 87FPCh. 18 - In the Mohr titration, Cl(aq) is titrated with...Ch. 18 - The accompanying drawing suggests a series of...Ch. 18 - Prob. 90SAECh. 18 - Briefly describe each of the following ideas,...Ch. 18 - Prob. 92SAECh. 18 - Prob. 93SAECh. 18 - Prob. 94SAECh. 18 - Prob. 95SAECh. 18 - Prob. 96SAECh. 18 - Prob. 97SAECh. 18 - Prob. 98SAECh. 18 - Prob. 99SAECh. 18 - Prob. 100SAECh. 18 - Prob. 101SAECh. 18 - Prob. 102SAECh. 18 - Prob. 103SAECh. 18 - Prob. 104SAECh. 18 - Prob. 105SAECh. 18 - Prob. 106SAECh. 18 - Will Agl(s) precipitate from a solution with [[Ag...Ch. 18 - Prob. 108SAECh. 18 - Appendix describes a useful study aid known as...
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- Consider the reaction BaF2(s)+SO42(aq)BaSO4(s)+2 F(aq) (a) Calculate K for the reaction. (b) Will BaSO4 precipitate if Na2SO4 is added to a saturated solution of BaF2?arrow_forwardHow do the concentrations of Ag+ and CrO42- in a saturated solution above 1.0 g of solid Ag2CrO4 Change when 100 g of solid Ag2CrO4 is added to the system? Explain.arrow_forwardAcrylic acid is used in the polymer industry in the production of acrylates. Its K, is 5.6 X 10“’. What is the pH of a 0.11 M solution of acrylic acid, CH2CHCOOH?arrow_forward
- To a beaker with 500 mL of water are added 95 mg of Ba(NO3)2, 95 mg of Ca(NO3)2, and 100.0 mg of Na2CO3. After equilibrium is established, will there be • no precipitate? • a precipitate of BaCO3 only? • a precipitate of CaCO3 only? • a precipitate of both CaCO3 and BaCO3? Assume that the volume of the solution is still 500.0 mL after the addition of the salts.arrow_forwardThe solubility of iron(II) hydroxide, Fe(OH)2, is 1.43×10–3 gram per liter at 25 °C. (a) Write a balanced equation for the solubility equilibrium. (b) Write the expression for the solubility product constant, Ksp, and calculate its value. (c) Calculate the pH of a saturated solution of Fe(OH)2 at 25 °C.arrow_forwardThe molar solubility of silver chromate, Ag₂CrO4, is 1.31×10-4 mol/L. (1) Express the solubility in units of grams per liter. g/L (2) Calculate the concentration of silver ion in a saturated solution of silver chromate. mol/Larrow_forward
- Lead (II) chloride, PbCl2, has Ksp = 1.6 x 10–5. (a) Determine the solubility of PbCl2 expressed in mol/L; (b) How many grams of PbCl2 will dissolve in 250 mL of water? (c) Predict whether PbCl2 precipitate will be formed when 2.0 mL of 0.10 M Pb(NO3)2 is added to 3.0 mL of 0.10 M NaCl.arrow_forwardLead (II) bromide, PbBr2, has Ksp = 4.6 x 10–6. (a) Will precipitate of PbBr2 form when 20.0 mL of 0.10 M Pb(NO3)2 is reacted with 30.0 mL of 0.10 M NaBr? (b) Determine the concentration of Pb2+, NO3–, Na+, and Br–, respectively, in the saturated solution at equilibrium. (c) How many grams of PbBr2 precipitate are formed at equilibrium? (Hint: use successive approximation method to determine concentrations of Pb2+ and Br– at equilibrium.)arrow_forwardLead (II) bromide, PbBr2, has Ksp= 4.6 x 10–6. (a) Will precipitate of PbBr2 form when 20.0 mL of 0.10 M Pb(NO3)2 is reacted with 30.0 mL of 0.10 M NaBr? (b) Determine the concentration of Pb2+, NO3–, Na+, and Br–, respectively, in the saturated solution at equilibrium. (c) How many grams of PbBr2 precipitate are formed at equilibrium? (Hint: use successive approximation method to determine concentrations of Pb2+and Br–at equilibrium.)arrow_forward
- Lead(II) carbonate, PbCO3, is one of the components of the passivating layer that forms inside lead pipes. Will the solubility of PbCO3 increase or decrease as the pH is lowered?arrow_forwardThe precipitation of Al(OH)3 (Ksp = 1.3 x 10-33) is sometimesused to purify water. (a) Estimate the pH at whichprecipitation of Al(OH)3 will begin if 5.0 lb of Al2(SO4)3is added to 2000 gal of water. (b) Approximately howmany pounds of CaO must be added to the water toachieve this pH?arrow_forwardCalculate the value of Kp of barium bromate, Ba(BrO3)2 given that the concentration of the barium ion, Ba*, in a saturated solution of barium bromate is 0.0393 mol/L.arrow_forward
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