3. For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. Use Ksp data from the ALEKS Data tab if needed. Does solubility change Highest Solubility? pH = Compound with pH? (yes or no) 3, 4, or 5? PbF2 Cal2 BaCl2 NaNO3

3. For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. Use Ksp data from the ALEKS Data tab if needed. Does solubility change Highest Solubility? pH = Compound with pH? (yes or no) 3, 4, or 5? PbF2 Cal2 BaCl2 NaNO3

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter15: Equilibria Of Other Reaction Classes

Section: Chapter Questions

Problem 11E: The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities...

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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)
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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?
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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.
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 ?
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Consider the reaction CaCl2 (s) = Ca2+ (g) + 2Cl- (aq) (Ksp = 5.5 x 10-6) 1. What is the solubility (in mg/L) of calcium chloride at 298K? 2. What is the equilibrium concentration of chloride ions in a saturated solution of calcium chloride? 3. What is the pH of this solution?
To compute the solubility product (Ksp) of barium nitrate (Ba(NO3)2), an excess amount of Ba(NO3)2 was added to 2 liters of water at 25 degrees celcius until the solution is saturated. Ba(NO3)2 is only slightly soluble in water. It was observed in their experiments that the solution boils at 100.15 K. Barium nitrate dissociates via the process: ?a(NO3)2(s) ⇄ Ba2+(aq) + 2NO3- (aq) Ksp = [Ba2+][NO3-]2 What is the solubility product Ksp and vapor pressure of the solution?
Calculate the Molar Solubility of Calcium Hyroxide in the Presence of a Common Ion (CaCl2) I have included the data and some calculation that can help with solving, but I am unsure if the calculation I have provided are accurate Data: 1. Concentration of standardized HCl Solution (mol/L) = 0.0646 2. volume of saturated Ca(OH)2 with added CaCl2 solution (mL) = 25 mL 3. Buret reading, initial (mL) = 0.03 mL 4. Buret reading, final (mL) = 19.85 mL 5. Volume of HCl added (mL) = 19.82mL Calculations: 6. Amount of HCl added (mol) = 1.28x10^-3 7. Amount of OH- in saturated solution (mol) =1.28x10^-3 8. [OH-] equillirium (mol/L) =5.12x10^-2 Molar solubility of Ca(OH)2=?
CrO42- can be used as an indicator when Br- is titrated with Ag+. What concentration of CrO42- should be used so that Ag2CrO4(s) just starts to form at the equivalence point? If a concentration of 0.0010 M CrO42- is used instead, at what concentration of Br- will Ag2CrO(s) just start to precipitate? Do you think this is likely to introduce significant error? The Ksp for Ag2CrO4(s) is 1.2x10-12.