Sodium sulfate is slowly added to a solution containing 0.0500 M Ca² + (aq) and 0.0330 M Ag*(aq). What will be the concentration of Ca? + (aq) when Ag,SO,(s) begins to precipitate? Solubility-product constants, Ksp, can be found in the chempendix. [Ca**] = M What percentage of the Ca² + (aq) can be precipitated from the Ag*(aq) by selective precipitation? percentage: %

Sodium sulfate is slowly added to a solution containing 0.0500 M Ca² + (aq) and 0.0330 M Ag*(aq). What will be the concentration of Ca? + (aq) when Ag,SO,(s) begins to precipitate? Solubility-product constants, Ksp, can be found in the chempendix. [Ca**] = M What percentage of the Ca² + (aq) can be precipitated from the Ag*(aq) by selective precipitation? percentage: %

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 70QAP: . The solubility product of iron(III) hydroxide is very small: Ksp=41038at 25 °C. A classical method...

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. The solubility product of iron(III) hydroxide is very small: Ksp=41038at 25 °C. A classical method of analysis for unknown samples containing iron is to add NaOH or NH3. This precipitates Fe(OH)3, which can then be filtered and weighed. To demonstrate that the concentration of iron remaining in solution in such a sample is very small, calculate the solubility of Fe(OH)3in moles per liter and in grams per liter.
The solubility of Ag(I) in aqueous solutions containing dif-ferent concentrations of Cl is based on the following equilibria:Ag⁺(aq)+Cl⁻(aq)⇌AgCl(s) Kₛₚ=1.8X10⁻¹⁰ Ag⁺(aq)+2Cl⁻(aq)⇌AgCl₂⁻(s) K(f)=1.8X10⁻⁵ When solid AgCl is shaken with a solution containing Cl⁻, Ag(I)is present as both Ag⁺ and AgCl₂⁻. The solubility of AgCl is thesum of the concentrations of Ag and AgCl₂.(a) Show that [Ag⁺] in solution is given by[Ag⁺]=1.8X10⁻¹⁰/[Cl⁻]and that [AgCl₂⁻] in solution is given by [AgCl₂⁻](3.2X10⁻⁵)([Cl⁻] (b) Find the [Cl⁻] at which [Ag⁺][AgCl₂⁻].(c) Explain the shape of a plot of AgCl solubility vs. [Cl⁻].(d) Find the solubility of AgCl at the [Cl⁻] of part (b), which is the minimum solubility of AgCl in the presence of Cl
The mineral pyrite, FeS2(s), can incorporate large amounts of arsenic. The dissolution of arsenic-rich pyrite can therefore release arsenic into groundwater (i.e., pyrite dissolution can be written as FeS2(s) = Fe2+ + S22-). What equation would you use to calculate whether pyrite in an aquifer will dissolve or precipitate?
The concentration of calcium carbonate in a sample of water saturated with the solid was found to be 7.00 x 10-5 moldm-3 at 200C. What is the solubility product of calcium carbonate at this temperature?
2. Copper(II) hydroxide is only very slightly soluble in water. The reaction by which it goes into solution is: Cu(OH)2(s) (reaversable) Cu+2 (aq) +2OH-(aq) A) It is possible to dissolve siginificant amounts of Cu(OH)2 in solutions i which the concentrations of either Cu+2 or OH- is very small. Explain why this is true using Ksp. B) Explain why Cu(OH)2 might have very appreciable solubility in 1 M HCl. (Consider the effect of Reaction 3 on the Cu(OH)2 solution reactioin) -reaction 3 =H2O (reverse) H+(aq)+OH-(aq), Kc= [H+][OH-]=1*10-14 AT 25 C
Among the solubility rules previously discussed is the statement: Carbonates, phosphates, borates, andarsenates—except those of the ammonium ion and the alkali metals—are insoluble. (a) Write the expression for the equilibrium constant for the reaction represented by the equationCaCO_3(s) ⇌ Ca^2+(aq) + CO3^1−(aq). Is Kc > 1, < 1, or ≈ 1? Explain your answer. (b) Write the expression for the equilibrium constant for the reaction represented by the equation3Ba^2+(aq) + 2PO_4^3−(aq) ⇌ Ba_3(PO_4)_2(s). Is Kc > 1, < 1, or ≈ 1? Explain your answer.
The solubility of lead(II) fluoride, PbF2, in pure water is 2.1 × 10–3 moles per liter. Calculate the value of Ksp for lead(II) fluoride from this data.
The hardness of water (hardness count) is usually expressed in parts per million (by mass) of CaCO3. What is the molar concentration of Ca2+ ions in a water sample with a hardness count of 175mg CaCO3il? How many milliliters of concentrated sulfuric acid, 94.0% (w/w), specific gravity of 1.831 are required to prepare 1 liter of a 0.100 M solution? The solubility-product constant for Ce(IO3)3 is 3.2x1010. What is the Ce3+ concentration in a solution prepared by mixing 50.0 ml of 0.0250 M Ce3.. with 50.00 ml of water?
As part of a soil analysis on a plot of land, a scientist wants to determine the ammonium content using gravimetric analysis with sodium tetraphenylborate, Na+B(C6H5)4−. Unfortunately, the amount of potassium, which also precipitates with sodium tetraphenylborate, is non‑negligible and must be accounted for in the analysis. Assume that all potassium in the soil is present as K2CO3 and all ammonium is present as NH4Cl. A 5.095 g soil sample was dissolved to give 0.500 L of solution. A 150.0 mL aliquot was acidified and excess sodium tetraphenylborate was added to precipitate both K+ and NH4+ ions completely. B(C6H5)4-+K+⟶KB(C6H5)4(s) B(C6H5)4-+NH4+⟶NH4B(C6H5)4(s) The resulting precipitate amounted to 0.269 g. A new 300.0 mL aliquot of the original solution was made alkaline and heated to remove all of the NH4+ as NH3. The resulting solution was then acidified, and excess sodium tetraphenylborate was added to give 0.129 g of precipitate. Find the mass percentages of NH4Cl and…
Sodium sulfate is slowly added to a solution containing 0.0500 M Ca2+(aq) and 0.0260 M Ag+(aq). What will be the concentration of Ca2+(aq) when Ag2SO4(s) begins to precipitate? Solubility-product constants, ?sp, can be found in the chempendix. [Ca2+]= M What percentage of the Ca2+(aq) can be precipitated from the Ag+(aq) by selective precipitation? percentage:
1.1The Ksp of Ca3 (PO4 ) 2 is 1.3 × 10−26 . Estimate the solubility of this salt in units of g. L −1 . You must show any reaction equation(s) that you may think are necessary. 1.2 If a sample of solid Ca3(PO4)2 is stirred into exactly one litre of a 0.550M solution of Na3PO4, how will the solubility of the salt compare with the answer that you have obtained in question 1.1? Explain you answer in a short sentence.
(a) If the molar solubility of Mg3(PO4)2 at 25 oC is 6.26e-06 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 0.00336 g of Ag2C2O4 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Ag2C2O4.Ksp = (c) The Ksp of Sc(OH)3 at 25 oC is 2.22e-31. What is the molar solubility of Sc(OH)3?solubility = mol/L