In a saturated solution of calcium phosphate, the concentration of PO43- ions is 3.3 × 10-7 M. The Ksp of Ca3(PO4)2 will be

Question

In a saturated solution of calcium phosphate, the concentration of PO43- ions is 3.3 × 10-7 M. The Ksp of Ca3(PO4)2 will be (A) 1.32 × 10-31 (B) 1.32 × 10-32 (C) 1.32 × 10-33 (D) None of these

Tardigrade Admin · Accepted Answer

Ca3(PO4)4 arrow 3Ca2+ +2PO3-4 [Ca2+]=(3/2)[PO3-4]=(3/2)×(3.3×10-7)M =4.95×10-7 M Ksp=[Ca2+]3[PO3-4]2 =(4.95×10-7)3×(3.3×10-7)M =4.95×10-7 M Ksp=[Ca2+]3[PO3-4]2 =(4.95×10-7)3×(3.3×10-7)2=1.32×10-32

Q. In a saturated solution of calcium phosphate, the concentration of $P O_{4}^{3 -}$ ions is $3.3 \times 1 0^{- 7} M$ . The $K_{s p}$ of $C a_{3} (P O_{4})_{2}$ will be

$1.32 \times 1 0^{- 31}$

$1.32 \times 1 0^{- 32}$

$1.32 \times 1 0^{- 33}$

None of these

Q. In a saturated solution of calcium phosphate, the concentration of PO43−​ ions is 3.3×10−7M. The Ksp​ of Ca3​(PO4​)2​ will be

1.32×10−31

1.32×10−32

1.32×10−33

None of these

Ca3​(PO4​)4​→3Ca2++2PO3−4 [Ca2+]=23​[PO43−​]=23​×(3.3×10−7)M =4.95×10−7M Ksp​=[Ca2+]3[PO43−​]2 =(4.95×10−7)3×(3.3×10−7)M =4.95×10−7M Ksp​=[Ca2+]3[PO43−​]2 =(4.95×10−7)3×(3.3×10−7)2=1.32×10−32

Q. In a saturated solution of calcium phosphate, the concentration of $P O_{4}^{3 -}$ ions is $3.3 \times 1 0^{- 7} M$ . The $K_{s p}$ of $C a_{3} (P O_{4})_{2}$ will be

$1.32 \times 1 0^{- 31}$

$1.32 \times 1 0^{- 32}$

$1.32 \times 1 0^{- 33}$