Consider the reaction CaSO_4(s) Ca^2+(aq) + SO_2_4^2-(aq) At 25 degree C the equ

Question

Consider the reaction CaSO_4(s) Ca^2+(aq) + SO_2_4^2-(aq) At 25 degree C the equilibrium constant is K_c = 2.4 Times 10^-5 for this reaction. If excess CaSO_4(s) is mixed with water at 25 degree C to produce a saturated solution of CaSO_4, what is the equilibrium concentration of Ca^2+? Express your answer to two significant figures and include the appropriate units. If excess CaSO_4(s) is mixed with water at 25 degree C to produce a saturated solution of CaSO_4, what is the equilibrium concentration of SO_4^2-? Express your answer to two significant figures and include the appropriate units. If the resulting solution has a volume of 1.5 L, what is the minimum mass of CaSO_4(s) needed to achieve equilibrium? Express your answer to two significant figures and include the appropriate units.

Explanation / Answer

CaSO4----> Ca+2 + SO4-2

let x = [Ca+2] = [SO4-2]

Solubility product, KSp =[Ca+2] [SO4-2] =x2= 7.1*10-5

x= 0.008426 Moles/L

Ca+2= 0.008426 moles/L and SO4-2= 0.008426 moles/L

moles of CaSO4 in 1.5 L= 0.008426*1.5 =0.012639

molecular weight of CaSO4= 136

Mass of CaSO4= moles*Molecular weight= 136*0.012639=1.7189 gms

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