Write balanced equations for the dissolution reactions and the corresponding solubility product expressions for each of the following solids. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) Ag, CO3 а. + Ksp = b. Ce(IO3)3 + Ksp = c. BaF2 + Ksp
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- Write an appropriate expression for the solubility product of the sparingly soluble compound Ca(OH)2 Given the solubility product, Ksp, of Ca(OH)2 is 5.3x10-5M3 at 25oC, calculate its solubility at this temperature in Water 25 M CaCl2 solutionA sparingly soluble compound with the general formula M3X2 has a solubility of 1.2 x 10-2 mg per 200 ml of water at 250C . Calculate the solubility product of this compound Provide the expression for the solubility product per 100ml of water. Given RAM: M=108, X=96Given that the ΔG°f for Pb2+(aq) and Cl−(aq) is −24.3 kJ/mole and −131.2 kJ/mole respectively, determine the solubility product, Ksp, for PbCl2(s).
- The solubility product constant for CaCO3 (s) in water is Ksp = [Ca+2] [CO3 -2] = 4.8 x 10^-9 Consider a 1.00 M solution of calcium chloride, in which you drop a piece of Dry Ice. Show that the minimum concentration (threshold amount) of carbonate ions necessary for a precipitate to appear is 4.8 x 10-9 M. Another way to think about this situation is to calculate the Q for the calcium chloride/Dry Ice solution and ask “will precipitation occur?”..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 Cl1.1The 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.
- In order to prepare for a qualitative analysis experiment, Felix is predicting whether small samples of several pairs of 0.10 M control solutions will form a precipitate when mixed. He uses the table of solubility values provided as well as the general solubility guidelines in the chempendix. Solubilities of Alkaline Earth Salts (g/100 g H2O, at 20−25∘C) OH− CO2−3 SO2−4 CrO2−4 C2O2−4 Mg2+ 0.00069 0.18 35.7 54.8 0.038Ca2+ 0.16 0.00066 0.205 13.2 0.00061Sr2+ 2.25 0.00034 0.135 0.106 0.005Ba2+ 4.91 0.0014 0.00031 0.00026 0.0075For each pair of compounds, predict the formula for the precipitate that Felix will see when he mixes the solutions in lab. If no precipitate forms, enter NP for no precipitate.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?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).
- Calculate the solubility (in g/L) of CaSO4(s) in 0.400 M Na2SO4(aq) at 25°C 0.400 M Na2SO4(aq) at 25°C. The Ksp of CaSO4 is 4.93×10−5.Chemistry The first container contains 20 ml 0.02 M AgNO3 solution at 25 ° C and the second container contains 40mL 0.04 M CaCl2 solution. (A) Determine the solubility product of AgNO3 in solution of 1st pot. (B) Analyze whether AgCI precipitation will occur when the solution of the 2nd container is completely mixed with the solution of the 1st container. The solubility of AgNO3 at 25 ° C = 2.2 × 10-3gL-1 and the solubility of AgCI is 1.8 × 10-10, the mass of Ag = 107.87A solution is prepared by combining 20.00ml of 0.150 molar Ba2+ and 25.00ml of 0.125 molar Cl- Using concentrations and volumes above, determine if a precipitate will form when these solutions are mixed at 25C. Provide a calculation to support your answer, keep in mind the system is not at standard state. Ba2+ (aq) -560.77 kJ/mol Delta Gfo Cl- (aq) -131.228 kJ/mol Delta Gfo BaCl2 -1296.32 kJ/mol Delta Gfo