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- Calculate the Ksp of the following compounds, given their molar solubilities. (a) CoS, 6.31 × 10-11 M (b) Cd(OH)2, 1.21 x 10-5 M (c) Ca3 (PO4)2, 1.14 × 10-7 MAt a particular temperature, 4.08 g of Gd2(SO4)3 will dissolve in 250 mL of water. What is the Ksp of Gd2(SO4)3?The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate Ksp for each of the slightly soluble solids indicated:(a) TlCl: [Tl+] = 1.21 × 10–2 M, [Cl–] = 1.2 × 10–2 M(b) Ce(IO3)4: [Ce4+] = 1.8 × 10–4 M, [IO3−] = 2.6 × 10–13 M(c) Gd2(SO4)3: [Gd3+] = 0.132 M, [SO42−] = 0.198 M(d) Ag2SO4: [Ag+] = 2.40 × 10–2 M, [SO42−] = 2.05 × 10–2 M(e) BaSO4: [Ba2+] = 0.500 M, [SO42−] = 2.16 × 10–10 M
- The value of Ksp for Cd(OH)2 is 2.5 x 10-14. (a) Whatis the molar solubility of Cd1OH22? (b) The solubilityof Cd(OH)2can be increased through formation of thecomplex ion CdBr42 - (Kf = 5 x 103). If solid Cd(OH)2 isadded to a NaBr solution, what is the initial concentrationof NaBr needed to increase the molar solubility of Cd(OH)2to 1.0 x 10-3 mol/L?The Ksp of Fe(OH)3(s) is 3x10-39. What concentration of Fe3+ can exist in solution at pH 3.0?Given that the Ksp for silver chloride is 1.76 x 10-10, and the Kf of silver(I) diammine cation [Ag(NH3)2 +] is 1.7 x 107, calculate the maximum number of grams of silver chloride that will dissolve in 250.0 mL of a 3.25 M solution of ammonia.
- at room temp. 0.00188 g AgCl dissolves in 1L of H2O. what is the ksp of AgCl?I need help solving this problem (see attached)(iv) The Ksp for zinc oxide is 3.5 x 1017. What concentration of zinc sulfate (in mol/L) must be dissolved in water in contact with solid zinc oxide to obtain a solution pH of 5.9?.
- Use the following data to calculate the Ksp value for each solid. (a) The solubility of FeCO3 is 5.6 ✕ 10−4 g/L.(b) The solubility of Cr(OH)3 is 1.3 ✕ 10−8 mol/L.If the equilibrium concentration of Ag1+ is 1.28 × 10-4 M, would the following set up for the Ksp value for Ag3PO be correct? Ksp - [Ag1+13(PO 3] = [1.28 × 10-413[(1.28 × 104 / 3)] is it true or false?(a) Given the Ksp of calcium phosphate, Ca3(PO4)2 is 1.3 ×10-32. Calculate the concentrations of Ca2+ and PO43- respectively.(b) If a hard water contains 75 mg/L of Ca2+, at what concentration of PO43− would a precipitate of Ca3(PO4)2 begin to appear?