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- Use the following solubility data to calculate a value of Ksp for each compound: a) CdCO3 : 1.0 x 10^-6 M b) Ca(OH)2 : 1.06 x 10^-2 M c) PbBr2 : 4.34 g/L d) BaCrO4 : 2.8 x 10^-3 g/LWrite the solubility product constant for: A. BaCrO4 B. Ag2CrO4 C. Mg3(PO4)2The Ksp value for Calcium Phosphate [Ca3(PO4)2] is 1.00 x 10-26 so calculate the molar solubility in units of grams per liter of calcium ions [Ca2+(aq)] if a chemist only made 2.198 Liters. What would the new molar solubility in grams per liter of calcium ions [Ca2+(aq)] be if the chemist added 0.129 M of Calcium Sulfate [CaSO4] to the solution? Calculate the ion products (Q) for Calcium Phosphate [Ca3(PO4)2] after the addition of the 0.129 M of Calcium Sulfate [CaSO4] to the solution. Determine if the reaction will shift to the right (no precipitate will form), shift to the left (a precipitate will form), or is at equilibrium.
- The Ksp value for Calcium Phosphate [Ca3(PO4)2] is 1.00 x 10-26 so calculate themolar solubility in units of grams per liter of calcium ions [Ca2+(aq)] if a chemist only made 2.198 Liters. What would the new molar solubility in grams per liter of calcium ions [Ca2+(aq)] be if the chemist added 0.129 M of Calcium Sulfate [CaSO4] to the solution? Calculate the ion products (Q) for Calcium Phosphate [Ca3(PO4)2] after the addition of the 0.129 M of Calcium Sulfate [CaSO4] to the solution. Determine if the reaction will shift to the right (no precipitate will form), shift to the left (a precipitate will form), or is at equilibriumWrite the expression for the solubility product constant for PbI2 CO (g) + 3 H2 (g) CH4 (g) + H2O (g).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)2∙H2O, 0.30 g/100 mL(c) NH4MgAsO4∙6H2O, 0.038 g/100 mL(d) La2(MoO4)3, 0.00179 g/100 mL
- What is the solubility (in g/L) of BaF2 at 25ºC? The solubility product constant for BaF2 is 1.0 x 10–6 at 25ºC. 0.18 g/L 1.1 g/L 2.8 g/L 8.8 x 10–5 g/L 1.8 x 10–4 g/LUse the solubility rules to predict the water solubility of each of the following compounds. A. Na2S B. K2So4 C. PB(OH)2 D. Ba3(PO4)2 E. PbCl2 F. (NH4)2CrO4 G. Ca(NO3)2 H. ZnCl2The solubility of BaF2 is measured and found to be 1.28 g/L. Use this information to calculate a Ksp value for barium fluoride.Ksp = --- The solubility of Ag2CO3 is measured and found to be 3.42×10-2 g/L. Use this information to calculate a Ksp value for silver carbonate.Ksp =
- What is the solubility of Sr(IO₃)₂ in a solution that contains 0.0300 M Sr²⁺ ions? (Ksp of Sr(IO₃)₂ is 1.14×10⁻⁷) What is the solubility of Sr(IO₃)₂ in a solution that contains 0.0550 M IO₃⁻ ions? (Ksp of Sr(IO₃)₂ is 1.14×10⁻⁷)Choose the correct solubility constant expression for iron(II) hydroxide in water: Ksp = [Fe2+][OH−]2/[Fe(OH)2] Ksp = [Fe2+][OH−]/[Fe(OH)2] Ksp = [Fe2+][OH−]2 Ksp = [Fe2+][OH−]Tooth enamel consists of hydroxyapatite, Ca5(PO4)3OH (Ksp = 8 × 10−37). Fluoride ion added to toothpaste and also drinking water reacts with Ca5(PO4)3OH to form the more tooth decay–resistant fluorapatite, Ca5(PO4)3F (Ksp = 1.0 × 10−60). Fluoridated water has dramatically decreased cavities among children. Calculate the solubility of Ca5(PO4)3OH and of Ca 5(PO4)3F in water.