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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Textbook Question
Chapter 18, Problem 31E
Will precipitation occur in the following cases?
- 010mg NeCI s added to 1.0 Lot 010 M AgNO2(aq).
- One drop (0.05 mL) of 0.10 M KBr is added to 250 mL of a saturated solution of AgCI.
- One drop (005 mL) of 0.0150 U NaOH(eq) is added to 3.0 Lola solution with 20mg Mg2+ per litter.
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A saturated solution of magnesium hydroxide is prepared and the excess solid magneisum hydorixed is allowed to settle. A 25.0 mL aliquot of the saturated solution is withdrawn and transfered to a flask, two drops of inficator are added. A 0.00053 M HCL is dispensed from a buret into a solution. The solution changes color after the addition of 13.2 mL. What is the molar solubility of magnesium hydroxide?
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A student was given 2 beakers labeled with
numbers 1 and 2, each beaker contains a
clear solution. Additionally, he was given two
reagent bottles labeled with A and B. Now,
he added reagent A to both beakers and he
noticed the formation of a precipitate in
beaker 2 but not in beaker 1. However, the
addition of reagent B to both beakers
resulted in the formation of a precipitate in
beaker 1 but not in beaker 2. Based on the
information, which of the following is
correct?
a. compound A is the limiting reactant
in beaker 1.
b. compound B is the limiting reactant
in beaker 2.
c. compound A is the limiting reactant
in beaker 2.
d. compound B will be the excess
reactant in beaker 1.
Question 2
Calculate the molar solubility of lead(II) iodide in water at 25°C. given that Ksp = 7.1 x 10-9Calculate the molar solubility of Mg(OH)2 (Ksp = 1.8 * 10-11 ) in(a) pure water;(b) 0.0862 M MgCl2.(c) 0.0355 M KOH(aq).
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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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that changes in the initial concentrations of the common ions can be neglected. (a) TlCl(s) in 1.250 M HCl. (b) PbI2(s) in 0.0355 M Cal2. (c) Ag2CrO4(s) in 0.225 L of a solution containing 0.856 g of K2CrO4. (d) Cd(OH)2(s) in a solution buffered at a pH of 10.995arrow_forwardThe Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSeO4, 0.0118 g/100 mL. (b) Ba(BrO3)2H2O, 0.30 g/100 mL. (c) NH4MgAsO46H2O, 0.033 g/100 mL. (d) La2(MoO4)3, 0.00179 g/100 mLarrow_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_forward
- The following solutions are mixed: 1.0 L of 0.00010 M NaOH and 1.0 L of 0.0014 M MgSO4. Is a precipitate expected? Explain.arrow_forwardA saturated solution of a slightly soluble electrolyte in contact with some of the solid electrolyte is said to be a system in equilibrium. Explain. Why is such a system called a heterogeneous equilibrium?arrow_forwardThe solubility product, Ksp, of PbCl2Â is 1.6 Ă— 10-5. What mass of KCl(s) must be dissolved in 150.00 mL of 1.15M Pb(NO3)2Â to produce a solution that is just saturated in PbCl2?arrow_forward
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