Which one is correct for the saturated solution of Ca3(PO4)2 salts if its Ksp is 2.05 × 10-33 ?

Ca3PO42(s)⇌3Ca2++2PO43− 3s 2s∴ Ksp=2.05×10−33=108s5∴ s=1.63×10−6M∴ Ca2+=3×1.63×10−6=4.9×10−6MPO43−=2×1.63×10−6=3.26×10−6MCa3(PO4)2eq=0,because all the salt is in ionic state.

Which one is correct for the saturated solution of Ca3(PO4)2 salts if its Ksp is 2.05 × 10-33 ?

Ca3PO42(s)⇌3Ca2++2PO43− 3s 2s∴ Ksp=2.05×10−33=108s5∴ s=1.63×10−6M∴ Ca2+=3×1.63×10−6=4.9×10−6MPO43−=2×1.63×10−6=3.26×10−6MCa3(PO4)2eq=0,because all the salt is in ionic state.

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Which one is correct for the saturated solution of Ca₃(PO₄)₂ salts if its K_sp is 2.05 × 10^-33 ?

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${[{Ca}^{2 +}]}_{eq.} = 4.9 \times 10^{- 6} M$

${[{Ca}_{3} {({PO}_{4})}_{2}]}_{eq} = Zero$

$Solubility of {Ca}_{3} {({PO}_{4})}_{2} is 1 .63 \times 10^{- 6} M$

${[{PO}_{4}^{3 -}]}_{eq.} = 3.26 \times 10^{- 6} m$

answer is A, B, C, D.

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Detailed Solution

${Ca}_{3} {({PO}_{4})}_{2} (s) ⇌ 3 {Ca}^{2 +} + 2 {PO}_{4}^{3 -}$

3s 2s

$\begin{array}{ll} ∴ K_{sp} = 2 .05 \times 10^{- 33} = 108 s^{5} \\ ∴ s = 1 .63 \times 10^{- 6} M \\ ∴ [{Ca}^{2 +}] = 3 \times 1 .63 \times 10^{- 6} = 4 .9 \times 10^{- 6} M \\ [{PO}_{4}^{3 -}] = 2 \times 1 .63 \times 10^{- 6} = 3 .26 \times 10^{- 6} M \end{array}$