1) Calculate the concentration of Ag+ left in solution after addition of 20 and 60ml of 0.1 M AGNO3 to 50ml of a solution containing 0.05M NaCl and 0.05M Na2S. Ksp AgCl= 1.8 x 10-10 for Ag2S = 6 x 10-51
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- On mixing 10.0 mL of 0.10 F CaCl₂ with 10.0 mL of 0.10 F Na₂SO4, what % of the CaSO4 formed dissolves? CaSO4: Ksp = 2.4 x 10-51. What is the molar solubility of PbCl2 in a solution of 0.23 M CaCl2? Ksp = 1.6 ✕ 10-5 for PbCl2. 2. What is the Qsp when 32.0 mL of 6.50 ✕ 10-7 M Na3PO4 are mixed with 41.4 mL of 5.50 ✕ 10-5 M CaCl2? Assume the volumes are additive. Ksp = 2.0 ✕ 10-29. 3. What is the Qsp when 61.0 mL of 1.50 ✕ 10-4 M AgNO3 are mixed with 80.0 mL of 5.20 ✕ 10-3 M CaCl2? Assume the volumes are additive. Ksp = 1.6 ✕ 10-10. 4. What [I-1] is needed to start the precipitation of AgI from a saturated solution of AgCl? Ksp = 2.9 ✕ 10-16 for AgI and Ksp = 1.2 ✕ 10-10 for AgCl.Calculate the pAg of the solution during the titration of of 40.00 mL of 0.2500 M NaCl with 0.500 M AgNO3 after the addition of the following volumes of reagent: (a) 12.50 mL, (b) 25.00 mL, (c) 28.00 mL. Ksp = 1.82 x 10-10
- Calculate pBr for the titration of 50 mL of 0.005 M NaBrWith 0.01 M AgNO3 after addition 0 mL, 5 mL, 25 mLand 25.1 mL. Ksp AgBr = 5.2 × 10^-13?Calculate the pAg values after the addition of 5.0, 40.0, and 50.0 mL of 0.050 M AgNO3 into 50.00 mL of 0.040 M KBr solution. Construct a titration curve for this titration. (Ksp = 5.0 x 10-13 for AgBr)Ksp of AgCl = 1.8 x 10^-10, how much volume of water would it take to dissolve 0.019g?
- What concentration of aqueous NH3 is necessary to just start precipitation of Mn(OH)2 from a 0.020 M solution of MnSO4? Kb for ammonia is 1.8 x 10-5, Ksp for Mn(OH)2 is 4.6 x 10-14 1.4 × 10-5 M 3.7 × 10-7 M 1.3 × 10-7 M 1.6 × 10-6 M 8.4 x 10-2 MFor the titration of 100mL of 0.001M NaCl (Cl-) with 0.0100M AgNO3 (Ag+), calculate the voltage at VAg+ = 0.5, 10.0, and 15.0mL Ksp (AgCl) = 1.8 x 10-10.What is the mole ratio of sodium acetate to acetic acid (Ka=1.8 x 10^-5) in a buffer with the pH of 4.00? Report to 3 sig figs
- 2. Calculate the solubility of silver acetate, AgCH3COO (s), in solutions buffered at pH = 2.00, 4.00, 6.00, 8.00, and 10.00 at 25◦ C. Take the value of Ksp for AgCH3 COO (s) to be 1.9 × 10−3 M2 at this temperature. Ka = 1.8 * 10^ -5The cations in an aqueous solution that contains 0.150 M Ba(NO3)2 and 0.0800 M Ca(NO3)2 are to be separated by taking advantage of the difference in the solubilities of their sulfates. Ksp(BaSO4) = 1.1 × 10-10 and Ksp(CaSO4) = 2.4 × 10-5 . What should be the concentration of sulfate ion for the best separation?Excess Ca(OH)2 is shaken with water to produce a saturatedsolution. The solution is filtered, and a 50.00-mL sampletitrated with HCl requires 11.23 mL of 0.0983 M HCl toreach the end point. Calculate Ksp for Ca(OH)2.