A 1.0M Na 2 SO 4 solution is slowly added to 10.0 mL of a solution...

A 1.0M Na 2 SO 4 solution is slowly added to 10.0 mL of a solution that is 0.20M in Ca 2+ and 0.30M in Ag + .

Part A Which compound will precipitate first: CaSO 4 ( K sp = 2.4× 10 −5 ) or Ag 2 SO 4 ( K sp = 1.5× 10 −5 )?

Part B How much Na 2 SO 4 solution must be added to initiate the precipitation? Express your answer using two significant figures.

Solutions

Expert Solution

Part A )

CaSO4 <--------------> Ca+2 + SO42-

0.20 SO42-

Ksp = [Ca+2][SO42-]

2.4× 10^−5 = 0.20 x [SO42-]

[SO42-] = 1.2 x 10^-4 M

Ag2SO4 <---------------> 2 Ag+ + SO42-

0.30 SO42-

Ksp = [Ag+]^2[SO42-]

1.5 x 10^-5 = (0.30)^2 x [SO42-]

[SO42-] = 1.67 x 10^-4 M

Since the concentration of SO42- needed to precipitate CaSO4 is slightly lower than that needed to precipitate Ag2SO4, so

the CaSO4 will precipitate first.

Part B )

volume = moles / molarity

= 1.2 x 10^-4 x 0.01 / 1.0

= 0.0012 mL

queen_honey_blossom answered 1 year ago

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