A solution is made by adding 0.390 g Ca(OH)2(s), 50.0 mL of 1.00 M HNO3, and enough water to make a final volume of 75.0 mL. Part A Assuming that all of the solid dissolves, what is the pH of the final solution? Express your answer using three decimal places. pH = nothing Request Answer Provide Feedback

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:

c.

explanation: