Use the atomic weights: Ag = 108, CI = 35If the Ksp of silver chloride is 1.56 x 10-10 at 25°C, how much will dissolve in400ml of a solution?Guide questions:a. Write the equilibrium reaotionb. Write the Ksp equationc. Determine the MW of silver ohlorided. Let x be the molar solubility, solve for M = xe. Solve for the weight of silver chloride that will dissolve in 400mL ofsolution

Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Use the atomic weights: Ag = 108, Cl = 35 If the Ksp of silver chloride is 1.56 x 10-10 at 25°C, how much will dissolve in 400ml of a solution? Guide questions: a. Write the equilibrium reaotion b. Write the Ksp equation . Determine the MW of silver ohloride d. Let x be the molar solubility, solve for M = x e. Solve for the weight of silver ohloride that will dissolve in 400mL of solution

Use the atomic weights: Ag = 108, Cl = 35 If the Ksp of silver chloride is 1.56 x 10-10 at 25°C, how much will dissolve in 400ml of a solution? Guide questions: a. Write the equilibrium reaotion b. Write the Ksp equation . Determine the MW of silver ohloride d. Let x be the molar solubility, solve for M = x e. Solve for the weight of silver ohloride that will dissolve in 400mL of solution

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter16: Solubility And Complex Ion Equilibria

Section: Chapter Questions

Problem 7RQ

See similar textbooks

Similar questions

Sodium chloride is added slowly to a solution that is 0.010 M in Cu+, Ag+, and Au+. Because solubility "rules" are generalizations, we don't use solubility rules when we have the specific Ksp data available. Instead, here, we can just use the Ksp value for CuCl which is 1.9 × 10–7, for AgCl is 1.6 × 10–10, and for AuCl is 2.0 × 10–13. Based on these specific Ksp values, which compound will precipitate first? All will precipitate at the same time. It cannot be determined. CuCl(s) AgCl(s) AuCl(s)
Calculate The solubility of Ba(IO3)2 in a solution prepared by mixing 200 mL of 0.00100 M Ba(NO3)2 with 100 mL of 0.0100 M NaIO3. The Ksp for barium iodate is 1.57 x 10-9(a) Write the solubility equilibria expression for Ba(IO3)2(b) Write the Ksp expression for the reaction in (a)(c) Determine the new concentration of Barium and Iodate ions(d) Determine the limiting and excess reactant(e) Calculate the molar solubility of Barium Iodate(f) What does a small value of Ksp tell us?
An aqueous solution contains Cu+, Tl+, Hg+, and Ti+ with each ion at a concentration of 0.15M. Chloride ion is slowly added to the solution. Using the Ksp information below, determine the order in which the ions would precipitate. AgCl = 1.8 x 10−10TiCl = 1.8 x 10−4PbCl2 = 1.7 x 10−5CuCl = 6.73 x 10−7TlCl = 3.7 x 10−4HgCl2 = 17.91 x 10−18
calculate the number of grams of magnesium ammonium phosphate MgNH4PO4, which will dissolve per liter if its Ksp is 2.5x10^-13 MW Of MgNH4PO4 = 137.34g/mol equilibrium reaction : MgNH4PO4 = Mg+NH4+PO4 A. write the ksp reaction B. let x be the molar solubility, solve for M=x c. solve for the weight of magnesium ammonium phosphate that will dissolve in 1L
PART 2: A solution is prepared by mixing 150.0 mL of 0.0010 M magnesium nitrate and 250.0 mL of 0.100 M sodium fluoride (Ksp = 7.4x10-11). Is Ksp greater than , equal to, or lower than Qsp? Will a precipitate form, Y/N? What is the fluoride ion concentration (in solution) after mixing is complete? Give your answer in exponential form and to three sig. figs. (e. g. 1.23E-3). What is the magnesium ion concentration (in solution) after mixing is complete? Give your answer in exponential form and to three sig. figs. (e. g. 1.23E-3).
The solubility of Fe(OH)2 is measured and found to be 1.15×10-3 g/L. Use this information to calculate a Ksp value for iron(II) hydroxide.
Magnesium fluoride (MgF2, MW = 62.30 g/mol) is slightly soluble in water, with Ksp = 7.4 x 10^-11 at T= 25. C.a) Give the correctly balanced solubility reaction and expression for Ksp for MgF2.b) What mass of magnesium fluoride will dissolve in 1.000 L of pure water?
Calculate the solubility of lead(II) sulfate (Ksp = 2.53x10-8) in a 0.0034 M solution of sodium sulfate. Give your answer to three sig. figs. and in exponential form (e. g. 1.23E-3).
Solid potassium hydroxide is slowly added to 175 mL of a 0.318 M nickel(II) acetate solution until the concentration of hydroxide ion is 0.0568 M. The percent of nickel ion remaining in solution is __ % Solubility Product Constants (Ksp at 25 oC) Type Formula Ksp Bromides PbBr2 6.3 × 10-6 AgBr 3.3 × 10-13 Carbonates BaCO3 8.1 × 10-9 CaCO3 3.8 × 10-9 CoCO3 8.0 × 10-13 CuCO3 2.5 × 10-10 FeCO3 3.5 × 10-11 PbCO3 1.5 × 10-13 MgCO3 4.0 × 10-5 MnCO3 1.8 × 10-11 NiCO3 6.6 × 10-9 Ag2CO3 8.1 × 10-12 ZnCO3 1.5 × 10-11 Chlorides PbCl2 1.7 × 10-5 AgCl 1.8 × 10-10 Chromates BaCrO4 2.0 × 10-10 CaCrO4 7.1 × 10-4 PbCrO4 1.8 × 10-14 Ag2CrO4 9.0 × 10-12 Cyanides Ni(CN)2 3.0 × 10-23 AgCN 1.2 × 10-16 Zn(CN)2 8.0 × 10-12 Fluorides BaF2 1.7 × 10-6 CaF2 3.9 × 10-11 PbF2 3.7 × 10-8 MgF2 6.4 × 10-9 Hydroxides AgOH 2.0 × 10-8 Al(OH)3 1.9 × 10-33 Ca(OH)2 7.9 × 10-6 Cr(OH)3 6.7 × 10-31 Co(OH)2 2.5 ×…
The Ksp of Al(OH)3 (MM: 78) is 1.90 xx 10^(-33). a) What is the molar solubility of Al(OH)3?
The compound lead(II) sulfate has a solubility of 4.824E-3 g/100mL at 25 degC.What is the molar solubility of this solution at saturation? 0.0002 mol/L What is the Ksp at 25 degC for lead(II) sulfate? What is the molar solubility of lead(II) sulfate in 0.28 M lead(II) nitrate ?
Calculate the solubility (in g/L) of silver chromate in water at 25°C if the Ksp for Ag3PO4 is 1.75 × 10-18. Ag3PO4(s) <==> 3Ag+ (aq) + PO43- (aq); Ksp = 27s4, s = _________ mol/L x MM of Ag3PO4 = _________ g/L.