Question

Write the mass balance equation AND charge balance equation for the following solutions (Don't forget about sig figs):

1.) NaHSO₄ ---> (H+) + (NaSO₄-)

Formal concentration: 0.020 (consider all forms)

2.) K₃PO4 ---> (3K+) + (PO₄-)

concentration: 0.100 (consider all forms)

Answer 1

Mass balance equation :

                                 The Quantity of all species in a solution containing a particular atom must must equal the amount of that atom delivered to the solution.

1)

NaHSO4 ---------> H⁺ + NaSO4^-

NaSO4^-   ----------------> Na⁺ + SO4^2-

TOT SO4 = [NaHSO4] + [Naso4^-] + [SO4^2-]

2)

K3PO4 ----------> 3K⁺ + PO4^3-

[K⁺] = 3 { [H3PO4] +[H2PO4^-]+[HPO4^2-]+[PO4^3-] }

Charge balance equation :

      Charge balance equation for aqueous solution is :

n₁[c₁] + n₂[c₂]+.......=m₁[A₁]+m₂[A₂]+.......

where , c is concentration of positively charged ions

           n is magnitude of positive charge

          A is concentration of negitively charged ions

         m is magnitude of negitive charge

1)

     [H⁺] + [Na⁺] = [NaSO4^-]+[SO4^2-]+[OH^-]

2)

   [H⁺]+[K⁺] = [H2PO4^-]+2[HPO4^2-]+3[PO4^3-]+[OH^-]