NOT form a precipitate in aqueous solution?

I have three solutions which is A, B, and C: calcium hydroxide, potassium sulfate, and sodium chloride. Combining B and C results in the formation of a precipitate, but neither solution forms a precipitate with A. Adding iron(II) nitrate to each solution only produces a precipitate with C. What are the unknowns? A: B: C:

CTO:2. Use solubility rules to determine the solubility of the following compounds: insol compound sol compound sol MgCl, Li₂SO4 KF CaSO4 AgBr K₂CO3 BaCl, Zn(NO3)2 AI(NO3)3 Pb(NO3)2 Hg(OAc)2 Pbl₂ CaS NaOAc CTO:3 insol compound sol ZnCO3 Cu(OH)2 NH₂OH Ni3(PO4)2 AIPO4 Na3PO4 AgNO3 insol

Does the following combination react to produce a precipitate? Can you explain to me how you can tell by using the chart given?

You have aqueous solutions of Ag* and PO43- that have equal concentrations. You mix them according to the following table: Test Tube # Number of drops Ag Number of drops PO4³- 01 0 4 2 1 3 3 9 2 t 8 3 6 4 Assuming the product of the reaction is insoluble, which test tube will contain the most. precipitate? 8 5 9 3

When aqueous solutions of ________ are mixed, a precipitate forms. A) NiBr2 and AgNO3 B) NaI and KBr C) K2SO4 and CrCl3 D) KOH and Ba(NO3)2

12) Which ion will precipitate all Group 2A Cations? a) Sulfate b) Sulfite c) Hydroxide d) Chloride e) Bromide C

Rb

Which combination will produce a precipitate? A) Pb(NO3)2 (aq) and HCI (aq) КОН (аq) and HNO3 (aq) c) Cu(NO3)2 (aq) and KC2H302 (aq) D) NaOH (aq) and Sr(NO3)2 (aq) E) AGC2H302 (aq) and HC2H302 (aq)

Complete and balance both sides of the following chemical reaction.  Place an (s) after any product, which is insoluble in water and would form a precipitate and (aq) after any product, which would remain dissolved using the Solubility Rules. a) AgNO3(aq)  +  NaCl(aq)  →   b) ZnBr2(aq)  +  K2S(aq)  →  c) Na3PO4(aq)  +  AlCl3(aq)  →  d) CaCl2(aq)  +  Na3PO4(aq)  →