Consider a solution that contains Ca2+ and Pb2+ ions, both at 0.010 M. If solid Na2SO4 is slowly added to the solution, which precipitates first? What is the concentration of the first
ion that precipitates when the second salt begins to precipitate?
The Ksp for CaSO4 and PbSO4 are 6.1 × 10−5 and 1.3 × 10−8, respectively.

CaSO4 and PbSO4  =  CaS 45

Explanation:

solution, 0.0104  a 42 cos

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm

the correct answer is option d

explanation:

i was wrong its d because they dont use cm when calculating square roots