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 pHat which you'd expect the highest solubility. You'lIl find K, data in the ALEKS Data tab.spDoes solubilitychange withpH?highest solubilitycompoundpH = 5pH = 4pH = 2O yesCaCO,O noO yesCuBrO noO yesNi(OH),O no

In a given compound if either cation or anion undergoes hydrolysis then solubility changes with pH.

Answered: For each of the following compounds,…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter16: Solubility And Precipitation Equilibria

Section: Chapter Questions

Problem 82CP

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The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSeO4, 0.0118 g/100 mL. (b) Ba(BrO3)2H2O, 0.30 g/100 mL. (c) NH4MgAsO46H2O, 0.033 g/100 mL. (d) La2(MoO4)3, 0.00179 g/100 mL
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. You'll find Ksp data in the ALEKS Data tab. compound Does solubility change with pH? highest solubility pH = 7 pH = 9 pH = 10 MgCl2 yes no BaOH2 yes no ZnS yes no huigp9ihb u
Compare the solubility of silver chloride in each of the following aqueous solutions: Match to soubility levels that goes with each. 0.10 M NH4NO3 0.10 M KCH3COO 0.10 M NH4Cl 0.10 M AgNO3 More soluble than in pure water. Similar solubility as in pure water. Less soluble than in pure water.
The solubility of strontium carbonate (SrCO3) is 0.0011 g/100 mL at 20ºC. Calculate the Kspvalue for this compound.
(a) I f t he molar solubilit y o f CaF2 at 35 °C i s1.24 x 10-3 mol/L, what is Ksp at this temperature? (b) It isfound that 1.1 x 10-2 g SrF2 dissolves per 100 mL of aqueoussolution at 25 °C. Calculate the solubility product forSrF2. (c) The Ksp of Ba(IO3)2 at 25 °C is 6.0 x 10-10. What isthe molar solubility of Ba(IO3)2?
2KMnO4 (aq) +5H2C2O4 (aq) + 3H2SO4 (aq) > 10CO2 (g) + K2SO4 (aq) +2MnSO4 (aq) + 8H2O (l) 90ml of 0.0150 M KMnO4 solution is mixed with 30 ml of 0.095 M H2C2O4 solution in a medium where there is excess sulfuric acid. Assume 100% yield Calculate the concentration of the following ions or molecules in the final solution a) Mn2+ b) K+ c) MnO4- d)H2C2O4
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7. 200.0 ml of 0.200 M Na3PO4, is added to 150.0 ml of 0.250 M Ca(NO3)2, and a precipitate result? What is the concentration of Ca2+ and PO43- after the precipitation occurs. (Ksp Ca3(PO4)2 = 6.3 X 10-15). Write chemical equations for the precipitation and Ksp reactions. Hint these RXNs are related and think about what the value of Ksp means and what assumptions we can make.
Consider a solution made by mixing 500.0 mL of 4.0M NH3 and 500.0mL of 0.40MAgNO3.Ag+ reacts with NH3, to form AgNH3+ and Ag(NH3)2+: Ag+(aq)+NH3(aq)AgNH3+(aq)+NH3(aq)⇌AgNH3+(aq)⇌Ag(NH3)2+(aq)K1=2.1×103K2=8.2×103 Determine the concentration of all species in solution. asap please.
This compound is only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product using the solubility in grams per 100 mL of water. BaSeO4 solubility = 0.0118 g/100 mL A) 1.65 x 10-7B) 1.77 x 10-7C) 1.77 x 10-8D) 1.50 x 10-7
A solution of 0.079 M CoBr2 is saturated with H2S. ([H2S] = 0.087 M. Assume saturation is maintained by bubbling H2S through the solution for the duration of the experiment.) CoS(s) Co2+(aq) + S2−(aq) Ksp = 4.0 ✕ 10−21 H2S(aq) + 2 H2O(l) 2 H3O+(aq) + S2−(aq) K = 8.9 ✕ 10−27 What is the minimum pH at which CoS begins to precipitate?
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