calcium phosphate will form a precipitate:   a. Ca2+ [6 x 10-9] and [(PO4)-3]2 [5 x 10-5]2   b. Ca2+ [6 x 10-9] and [(PO4)-3]2 [8 x 10-7]2   c. Ca2+ [6 x 10-8] and [(PO4)-3]2 [5 x 10-4]2   If you know that the Ksp = l 1 x 10-23

22. What is the Ion Product number (Q value) when 0.150 L of 0.100 M Pb(NO3)2 and 0.100 L of 0.200 M NaCl are mixed? Will a precipitate form? (Ksp of PbCl2 = 1.2 x 10-5) %3D a. 3.84 x 10-4; no precipitate will form b. 3.84 x 10-4; precipitate will form c. 4.80 x 10-3; no precipitate will form d. 4.80 x 10-3; precipitate will form

a) The solubility product of AgBr is 10-13 mol² L-². Calculate the solubility in water Calculate the solubility in a 10-² M Br solution - How and why does the solubility change if instead of water a NaNO3 solution is employed? Please explain the reason for any change. b) The solubility product of Al(OH)3 equals 10-33. Please calculate the solubility. -

Which of the following compounds will have the highest molar solubility in pure water ? a. Pb3(PO4)2, Ksp = 3.0 x 10 ^-44 b. PbS, Ksp = 8.4 x 10^-28 c. PbCO3, Ksp = 1.5 x 10 ^-13 d. PbSO4, Ksp = 1.82 x 10 ^-8 e. PbI2, Ksp = 8.7 x 10 ^-9

2. Calculate the molar solubility of lead(II) phosphate in a pH 10 solution. Pb3(PO4)2(s) 3 Pb²+ (aq) + 2 PO4³- (aq) Pb²+ (aq) + 3 OH(aq) Pb(OH)3(aq) Ksp = 1.0 x 10-54 Kf = 8.0 x 1013 Pb3(PO4)2(s) + 9 OH(aq) 3 Pb(OH)3 (aq) + 2 PO4³- (aq)

1. A saturated solution of Mg(OH)2 is prepared having a large excess of Mg(OH)2. Sn(NO3)2 is added to the solution. Ksp = 2.0 ✕ 10-11 for Mg(OH)2 and Ksp = 5.3 ✕ 10-26 for Sn(OH)2. a) What [Sn2+] is required to start the precipitation of Sn(OH)2? b) What [Sn2+] is required so that the [Mg2+] in solution will be 0.12 M?   2. Solid NaI is added to a solution which is 0.025 M in TlNO3 and 0.015 M in AgNO3. Assume the volume remains constant. Ksp = 8.9 ✕ 10-8 for TlI and Ksp = 1.0 ✕ 10-16 for AgI. a) Which compound precipitates first TII or AgI?   b) What is the concentration of the first ion precipitated when the second ion starts to precipitate?       3. What is the molar solubility of PbSO4 in 0.19 M MgSO4? Ksp = 1.0 ✕ 10-8 for PbSO4.

[Review Topics] [References] Use the References to access important values if needed for this question. A solution contains 1.24x10-² M silver nitrate and 9.41x10-³ M calcium acetate. Solid ammonium sulfite is added slowly to this mixture. What is the concentration of silver ion when calcium ion begins to precipitate? [Ag+] = M Submit Answer Retry Entire Group 2 more group attempts remaining

pls complete the table using given dataEffect of Common Ions on the Solubility of Ca(OH)21. Add Ca(OH)2 to 250.0 mL of 0.010 M CaCl2 with stirring until equilibrium is achieved.2. Filter the undissolved precipitate. Measure out 50.0 mL of the filtrate in a 250-mL Erlenmeyer flask. 3. Add a few drops of phenolphthalein indicator and titrate with standardized HCl solution until endpoint is achieved. 4. Record the volume of HCl solution used. Perform two more trials.

A solution contains 1.22x10-2 M lead nitrate and 1.05x10-² M silver acetate. Solid sodium chloride is added slowly to this mixture. What is the concentration of silver ion when lead ion begins to precipitate? [Ag*]= Submit Answer Retry Entire Group 7 more group attempts remaining

The solubility product of Mg(OH)2 is 1.2x10-11. Predict whether a precipitate will beformed or not if 20.0 mL of 0.01 M MgCl2 solution is mixed with 30.0 mL of 1x10-3 MNaOH solution. Show supporting calculations