Question #134180
Calculate the concentrations of the major ionic species present in the 1.29 mL solution of 3.22 mg of Ba(HCO3)2.
Expert's answer
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.
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