Answer to Question #134180 in Organic Chemistry for Vero Elo

Question

Calculate the concentrations of the major ionic species present in the 1.29 mL solution of 3.22 mg of Ba(HCO3)2.

Answer 1

Solution:

The molar mass of Ba(HCO₃)₂ is 259.36 g/mol.

Moles of Ba(HCO₃)₂ = Mass of Ba(HCO₃)₂ / Molar mass of Ba(HCO₃)₂

Moles of Ba(HCO₃)₂ = (0.00322 g) / (259.36 g/mol) = 0.0000124 mol

Molarity of Ba(HCO₃)₂ = Moles of Ba(HCO₃)₂ / Volume of solution

Molarity of Ba(HCO₃)₂ = (0.0000124 mol) / (0.00129 L) = 0.0096 mol/L = 0.0096 M

Dissociation reaction:

Ba(HCO₃)₂ ⟶ Ba²⁺ + 2HCO₃^-

The major ionic species: Ba²⁺; HCO₃^-

[Ba²⁺] = Molarity of Ba(HCO₃)₂ = 0.0096 M (according to the dissociation reaction)

[HCO₃^-] = 2 × Molarity of Ba(HCO₃)₂ = 2 × (0.0096 M) = 0.0192 M (according to the dissociation reaction)

Answer: The concentrations of the major ionic species: [Ba²⁺] = 0.0096 M; [HCO₃^-] = 0.0192 M.