Formula AIPO4 Cd3(PO4)2 Ca3(PO4)2 Li3PO4 With which of the following solutions would a 3.5 x 10€ M solution of PO ³+ ions FORM a precipitate? (Assume the concentrations given are after mixing the solutions.) Ksp 9.84 x 10-21 2.53 x 10-33 2.07 x 10-33 2.37 x 10-4 A) 5.0 x 10-15 M A1³+ B) 5.0 x 10-15 M Cd²+ C) 5.0 x 10-15 M Ca²+ D) 5.0 x 10-15 M Li*

A lab scientist mixes 20.0 mL of a 0.670 M solution of CaCl2 with 10.0 mL of a 0.856 M solution of Li3PO4. How many grams of precipitate did he create and what is the identity of that precipitate (be careful with the balancing of this equation)?

suppose you wanted to remove the lead ions Pb2+ from drinking water without removing the calcium ions (Ca2+) which provided drinking water its distinctive taste. What is the maximuin amount of hydroxide you would add to precipitate out Pb2+ without removing Ca+2.  The Ksp for Ca(OH)2 and Pb(OH)2 are 5.5x10^-6 and 2x10^-15, respectively.

A solution contains 1.45x10-2 M sodium carbonate and 9.94x10-3 M ammonium sulfide. Solid copper(II) nitrate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of copper(II) ion when this precipitation first begins? [Cu²+] = M

Determine the mass, in grams, of precipitate that forms when 608, ml. of 0.499 M Na₂CO, reacts with 882. ml. of 0.455 M Ca(OH)₂. Round your answer to 3 significant figures. Ca(OH)₂ (aq) + Na₂CO, (aq) Caco, O.P - 2NaOH(aq) + CaCO, (s)

A solution contains 7.27x103 M lead nitrate and 1.16x102 M calcium acetate. Solid ammonium sulfate is added slowly to this mixture. What is the concentration of lead ion when calcium ion begins to precipitate? [Pb2*] =| M

If a student uses 1 mg K2CrO4 as indicator for 100 mL of NaCl sample solution, what is the concentration (M) of chloride ion in the solution when red precipitate (Ag2CrO4) starts to form?

There is a solution containing two metal cations. The goal is to separate them by slowly and carefully adding a solution of an anion, until one mental cation precipitates as a compound with that anion, leaving the other metal cation still in solution. M+ is Ag+, M2+ is Ca2+, anion is SO4 2-, first Ksp is 1.2 x 10-5, second Ksp is 6.1 x 10-5, and the starting concentrations of M+ is 1.50 x 10-2 M and M2+ is 3.50 x 10-2M. Using these values, predict which metal will precipitate first and what concentration of anion the precipitation will begin.

If we mix 45 mL of 1.5 M sodium iodide with excess lead nitrate, how many grams of precipitate will form? Pb(NO3)2 + 2 Nal —> Pb12 + 2NaNO3

4.) Regarding the fırst preliminary test, what concentration of AGNO3 is required to just cause SO32 ions to precipitate? Assume the concentration of SO32 is 0.10 M. [AGNO3] = _х 107 м