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Determine the solubility of TlBr in a solution of sodium nitrate when the ionic strength is 0.05 and Ksp= 3.4 E-6
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- Calculate the Ksp for silver sulfate if the molar solubility of Ag2SO4 in pure water is 0.0144 M. a. 1.2 × 10-5 b. 3.0 × 10-6 c. 4.2 × 10-4 d. 2.1 × 10-4Calculate the Ksp for magnesium fluoride if the solubility of MgF2 in pure water is 0.000234 M. a. 9.3 × 10-4 b. 5.8 × 10-5 c. 5.1 × 10-11 d. 1.3 × 10-11Calculate the solubility (in g/L) of Aluminum sulfide (Al2S3) In 0.25 M Al+3 solution. (standard conditions.) {Ksp for Al2S3 is 1.5×10-27}.
- Determine the solubility for PbI2 in a 500 millilitre solution containing 1.33 grams of Pb(NO3)2. Assume the Ksp to be 1.4 x 10-8.Calculate the solubility (in g/L) of Aluminum sulfide (Al2S3) at 25°C {Ksp for Al2S3 is 1.5x10^-27}. 1) in pure water 2) in 0.10 M H2S solution and in 0.25M Al^+3 solutionDetermine the solubility for a saturated solution of Tl2S. Ksp = 6.0 x 10-22
- Calculate the solubility of CrF3 in g /100mL . (Ksp of CrF3 6.6*10^ -11 )The Ksp of Fe3(PO4)2 is 2.70⋅10−252.70⋅10-25 M. Calculate the solubility of each ion in a saturated solution: M Fe2+ M PO43-At 25oC, Ksp for AgBr is 5.0 x 10-3 g. Calculate the solubility of AgBr in g L-1 at 25oC a) in pure water b) in the presence of 0.2mol L-1 NaBr solution
- Consider the equilibrium reaction: YZ2(s) ⇌ Y2+(aq) + 2Z-(aq). What is the molar solubility of YZ₂ (Ksp= 4.0 x 10⁻¹¹) at 25⁰C in a 0.03 M AZ₂ solution? Assume that AZ₂ is a strong electrolyte.Determine the solubility of Ag2SO3 (Ksp=1.5x10-14; MW=295.8 g/mole) in a 0.2 M solution of Na2SO3.The solubility of borax, which is made up of sodium tetraborate (Na2B4O5(OH)4 8H2O), was analyzed. The dissolution of borax is: Na2B4O5(OH)4 • 8H2O(s) ⇌ 2 Na+(aq) + B4O5(OH)42–(aq) + 8 H2O(l) A 50 mL saturated solution was prepared. After filtration of solution, 5 mL aliquot was transferred to a flask and titrated using 0.432 M HCl. The endpoint was found to be 4.73 mL of the titrant. Tetraborate anion (B4O5(OH)42-) is a weak base which reacts with HCl like the following reaction: B4O5(OH)42–(aq) + 2 H+(aq) + 3 H2O(l) ⇌ 4 H3BO3(aq) What is Ksp expression for the dissolution? What is the tetraborate ions concentration in the filtrate? What is the molar solubility and Ksp of borax if the titration was done at room temperature (298 K)?