Select the chromate compound that is most soluble in water at 25°C on a molar basis using the following solubility data. Ksp BaCrO4 2.0 x 10-9 PbCrO4 1.8 x 10-14 Ag2CrO4 7.0 x 10-12

What percent of Ba2+ ions remain  when CaSO4 begins to precipitate from asolution that is 0.05M in both Ba2+ and Ca2+?  Ksp CaSO4=4.9x10-5 and Ksp of BaSO4=1.1x10-10  ?

1. Why must the solution be saturated when its solubility is determined? 2. Compare your experimental value for Ksp of Ca(OH)2 with the literature value (Ksp = 8.0 × 10-6 at 25°C). Account fora anydifference. 3. Is Ca(OH)2 more soluble in aqueous solution containing calcium ions or in pure water? Explain your observation in terms of shift in equilibrium and in terms of the ion product in relation to Ksp. 4. Cite possible sources of error in the experiment. 5. The solubility of CdS in water is 1.29 x10-12 M. Determine the solubility product constant for CdS. 6. The solubility product constant of Cd(OH)2 and Co(OH)2 are 7.21 × 10–15 and 5.92 × 10–15, respectively. In terms of calculating molar solubility, which of these hydroxides is less soluble?

A student titrates a weak acid and draws the titration curve. Suppose s/he forgets to subtract off Vinitial from the volume data, causing the curve to be shifted to the right. (a) Will the calculated pKa be affected? Explain your answer. ---Select--- v| because the y-values are ---Select--- V (b) Will the molar mass be affected? Explain your answer. ---Select--- v because the x-values are ---Select---

ksp When 15.0 mL of a 3.39×104 M copper(II) sulfate solution is combined with 25.0 mL of a 7.45×10-4 M potassium sulfide solution does a precipitate form? (yes or no) For these conditions the Reaction Quotient, Q, is equal to

P Chemical eg X P Chemical eq X P Chemical ec X P Chemical ec X P Chemical ec x P Chemi View?assignmentProblemlD=144082837&offset%3Dnext CHE154-H Gen Chem II Bronikowski S20 Part A sp Use the molar solubility, 1.08 × 10-5 M, in pure water to calculate K, for BaCrO4. Express your answer using three significant figures. . ΑΣφ Ksp

What is the molar solubility (in mol L-1) of a salt with general molecular formula MX (where M is a cation and X is an anion) in a solution already containing 0.534 mol L-1 M+ ? The Ksp of MX = 2.1 x 10-8

Sodium carbonate, Na2CO3, is added dropwise to a solution that contains 1.0 X 10-2 M Ag+ and 5.0 X 10-2 M Cd2+.  Specify the minimum molar concentrations of carbonate ion needed to precipitate each cation.  (Ksp = 8.1 X 10-12 for Ag2CO3; Ksp = 1.8 X 10-14 for CaCO3)

The Ksp for silver chromate (Ag2CrO4) is 1.1x10-12. Using the same initial set up of 10mL of 1M silver nitrate is combined with 25mL of 0.1M sodium chromate, what is the mass of the silver chromate precipitate in grams?

SPECTROPHOTOMETRIC DETERMINATION OF A SOLUBILITY PRODUCT CONSTANT A) Write the Equation for the dissolving of solid AgCrO4 in water and the Ksp expression for equilibrium.  B) Calculate the molar solubility of BaCrO4. Ksp = 2.1 X 10^-10. Show the equilibrium setup and the calculation.  C) Calculate the molar solubility of BaCrO4 in the presence of 0.020 M Na2CrO4. Show the equilibrium setup and calculation.