Part A: A saturated solution of Ca3(PO4)2 has [Ca2+] = 2.06 ×108M and [PO34] = 1

Question

Part A: A saturated solution of Ca3(PO4)2 has
[Ca2+] = 2.06 ×108M and
[PO34] = 1.3 ×105M.
Calculate Ksp for Ca3(PO4)2.

Part B: Calculate the molar solubility of MgF2 in 0.13 M MgCl2 at 25 C.

PArt C: In an excess of NH3(aq), Cu2+ ion forms a deep blue complex ion, Cu(NH3)42+, which has a formation constant Kf=5.6×1011. Calculate the concentration of Cu2+ in a solution prepared by adding 4.6×103mol of CuSO4 to 0.520 L of 0.42 M NH3.
Express your answer using two significant figures.

Thanks for any help :)

Explanation / Answer

part A is not related to any of the other parts.

They are different questions and not a single question

I am allowed to answer only 1 question at a time

So I will answer only the 1at question

A)

Ca3(PO4)2 ----> 3Ca2+ + 2PO43-

Ksp = [Ca2+]^3 [PO43-]^2

= (2.06*10^-8)^3 (1.3*10^-5)^2

=1.48*10^-33

Answer: 1.48*10^-33

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