If excess caso4(s) is mixed with water at 25 ∘c to produce a saturated solution of caso4, what is the equilibrium concentration of ca2+?

The equlibrium concentration sof Ca+2 ion willl be 4.9×10∧-3 M

Data Given:

              Ksp of CaSO4 = 2.4 × 10∧-5

              CaSO4 ⇔ Ca+2   +  SO4∧-2

Solution:

                Ksp = [Ca+2].[ SO4∧-2]

                 2.4 × 10∧-5 = [x].[x]= x²

                 x =  4.9×10∧-3 M

Result:

the grams   of   barium that   are in   2.3 x 10^23   atoms of barium   is   52.4 g (answer c)

    calculation

mass = moles   of ba   x molar   mass of ba

  molar mass of ba from periodic table=   137.3 g/mol

  use the   avogadro's law   constant   to   calculate the moles of barium

  that   is     1 mole =   6.02   x 10^23 atoms

                    ? moles = 2.3 x 10^23   atoms

by cross   multiplication

=(1 mole   x 2.3x 10^23 atoms)   / 6.02   x10^23 atoms)=   0.382   moles

mass   is therefore = 137.3   g/mol x 0.382 mol = 52.4 ( answer c)

explanation: