AgCl(s) 2 Ag+ (aq) + CI- (aq) Ken = 4.0 x 10-10ds.Ag* (aq) + 2 CIF (aq) 2 [AgCl,] (aq)K2 = 1.8 x 105AgCl(s) + CIF (aq) [AgCl,]¯ (aq)K3 = ?(i) The student finds that AgCl is more soluble in NaCI(aq) than in water because of the series of reactions above. Determine the value of K3 for the overall reaction.В I Ux2X2 5ΩII 2 of 2The student then conducts an experiment to determine the solubility of AgCl in a 2.5 M NaCl solution at various temperatures. Some AgCl(s) remains in the container at all temperatures studied. Thedata are plotted on the graph below.0.90.80.70.60.5-0.4+707580859095 100Temperature (°C)(h) A 1000. g sample of a saturated solution at 95° C is cooled to 85°C. Determine the mass of AgCl(s) that would precipitate out of the solution.BUx2X.Mass of AgCl Dissolvedsolution)

Given step reactions are : AgCl (s) <------------> Ag+ (aq) + Cl- (aq) , Ksp = 4.0 x 10-10…

Answered: AgCI(s) 2 Ag* (aq) + CIF (aq) Ksp = 4.0…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 14.67QE

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. K for copper(II)hydroxide, Cu(OH)2, has a value 2.21020at 25 °C. Calculate the solubility of copper(II) hydroxide in mol/L and g/L at 25 °C.
Some lithium chloride, LiCl, is dissolved in 100 mL of water in one beaker, and some Li2SO4 is dissolved in 100 mL of water in another beaker. Both are at 10 C, and both are saturated solutions; some solid remains undissolved in each beaker. Describe what you would observe as the temperature is raised. The following data are available to you from a handbook of chemistry:
For each of the following pairs of solutions, select the solution for which solute solubility is greatest. a. Ammonia gas in water with P = 1 atm and T = 50C Ammonia gas in water with P = 1 atm and T = 90C b. Carbon dioxide gas in water with P = 2 atm and T = 50C Carbon dioxide gas in water with P = 1 atm and T = 50C c. Table salt in water with P = 1 atm and T = 60C Table salt in water with P = 1 atm and T = 50C d. Table sugar in water with P = 2 atm and T = 40C Table sugar in water with P = 1 atm and T = 70C
Assume that the solubility of carbon dioxide gas in pop at 5oC is 0.586 g/100 mL and at 20oC its solubility is 0.169 g/100 mL. What mass of carbon dioxide gas will escape from a 355-mL can of Coke that has been taken out of the fridge and has been sitting open at 20oC?
7.A solution is prepared by dissolving 0.030 mol of potassium perchlorate in 75 mL of hot water. KClO4 dissolves according to the equation KClO4 (s) ? K+ (aq) + ClO4- (aq). Will a precipitate form if the solution is cooled to 25oC? Assume that a negligible change in volume occurs during the operations. (Ksp = 8.9 x 10-3).
The solubility of manganese (II) hydroxide (Mn(OH)2) is 2.2 x 10-5 M. What is the Ksp of Mn(OH)2?
Pseudogoutis caused by the formation of calcium diphosphate (Ca2P2O7) crystals in tendons, cartilage and ligaments, usually occurring if diphosphate levels in blood plasma 7 become very If the [Ca2+] in blood plasma is 9.2 mg/dL and Ksp for Ca2P2O7 is 8.64 x 10-13, what is the minimum concentration of diphosphate P2O 4- necessary for precipitation?
The solubility of barium chlorite at 20.0 ℃ is 45.4 g/100 mL. From this information, calculate the molar concentration of a saturated solution of barium chlorite. (Do not show your work in the space provided; record only your final answer with the correct number of significant digits and the proper units.) The following evidence was obtained from an experiment to determine the molar concentration of a sodium nitrate solution. A sample of sodium nitrate solution was evaporated to dryness and the mass of solid residue was measured.Evidence:Volume of solution = 10.00 mLMass of beaker = 79.54 gMass of beaker and residue = 83.25 gFrom this data, calculate the molar concentration of the original sodium nitrate solution.(Do not show your work in the space provided; record only your final answer with the correct number of significant digits and the proper units.)
2.3 - At temperature of 18°C was 4,7 g of silver molybdate (M = 376 g mol–1) mixed with 500 cm3 of a) distilled water b) solution of AgNO3 with concentration of 0,02 mol dm–3 c) solution of Na2MoO4 with concentration of 0,02 mol dm–3 Determine, how many percent of Ag2MoO4 will dissolve in each case. Solubility equilibrium of Ag2MoO4 is 3,1.10-11.
Tooth enamel is composed of hydroxyapatite, whose simplest formula is Ca5(PO4)3OH, and whose corresponding Ksp = 6.8 * 10-27. As, fluoride in fluorinated water or in toothpaste reacts with hydroxyapatite to form fluoroapatite, Ca5(PO4)3F, whose Ksp = 1.0 * 10-60. Write the expression for the solubility-constant for hydroxyapatite and for fluoroapatite.
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The solubility of Fe(OH)2 is 2.1 x 10-4 g L-1. What is the Ksp for Fe(OH)2 at 25 °C?

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