Which of the following compounds precipitates from a solution that has the concentrations indicated?  (a) KClO4: [K+] = 0.01 M, [ClO4-] = 0.01 M (b) K2PtCl6: [K+] = 0.01 M, [PtCl62-] = 0.01 M (c) PbI2: [Pb2+] = 0.003 M, [I–] = 1.3 x 10–3 M (d) Ag2S: [Ag+] = 1 x 10–10 M, [S2–] = 1 x 10–13 M

Consider an analyte solution of 50.0 mL of 0.050 M hydrochloric acid, HCl, titrated against 0.10 M sodium hydroxide, NaOH (d) After adding 12.50 mL of the NaOH, halfway to the equivalence point, what ions or molecules are present in the solution? (e) At the equivalence point, after adding 25.00 mL of NaOH, what ions or molecules are present in the solution? (f) Which of the species you identified in part (e) will determine the pH of the solution?

A solution is prepared by adding Cu2+, S2-, Na+, NO3-, and PO43- ions.  Identify each of the precipitates that could form under normal conditions:

Chemistry (Part -5) =============

Phosphoric acid dissociates to form phosphate anion and hydroniumcation. The K, for this reaction is 4.5 x 10 13. Choose the correct equation which expresses this reaction. 4.5 x 1013 - ([PO4³] × [H3O*J³ ) / ( [H3PO4] × [H2O] ) 4.5 x 1013 - ( [PO4®] × [H3O*] ) / [H3PO4] 4.5 x 1013 = ( [PO,³] × [H3O*]³ ) / [H3PO4] 4.5 x 1013 = [H3PO4) / ([PO4®] x [H3D*j$ ) Question 14 5 pts Cheesethe e for the loulmeler

Calculate the concentration (molarity) of Pb2+ ions in a solution made by adding 0.010 moles of Pb(NO3)2 to 1.0 L of a  2.0 M NaI solution.  (Kf = 3.0 x 104 for PbI42−) - 4.9 x 10−2 -3.3 x 10−5 - 2.1 x 10−7 -1.7 x 10−7 -2.3 x 10−8

Calculate the number of moles of CO2 that would be produced if 1.00 mL of vinegar completely reacts with a stoichiometrically equivalent amount of baking soda. NaHCo3+HC2H3O2--yields--NaC2H3O2+CO2+H2O

0.20 moles of CuSO4 are added to 1L of NH3 1.20M solution. Calculate the concentration of Cu2+ in the equilibrium.

2b

If the molar solubility of PbCrO4 at 25 oC is 5.48e-07 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 1.08e-09 g of Fe(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Fe(OH)3.Ksp = (c) The Ksp of Mg3(PO4)2 at 25 oC is 1.04e-24. What is the molar solubility of Mg3(PO4)2?solubility =  mol/L