NaCl is purified by adding HCl to a saturated solution of NaCl (317 g/L). Will pure NaCl precipitate when 10mL of 13.0 M HCl is added to 0.2 L of saturated solution?

Yes, pure NaCl will precipitate out of the solution

Explanation:

The parameters of the NaCl solution and HCl mixture are;

The saturation of the NaCl solution = Saturated solution

The mass concentration of the NaCl solution = 317 g/L

The volume of the HCl added = 10 mL

The concentration of the HCl added = 13.0 M HCl

The volume of the saturated NaCl solution = 0.2 L

The molar mass of NaCl = 58.44 g/mol

The number of moles of NaCl per liter = (317 g/L)/(58.44 g/mol) = 7925/1461 moles ≈ 5.42 moles

The ionization of the molecules in solution are;

HCl (aq) + H₂O (l) → H₃O⁺ (aq) + Cl⁻ (aq)

NaCl (s) ↔ Na⁺ (aq) + Cl⁻ (aq)

The number of moles of the Cl⁻ ion from the HCl is 13 moles per liter, the number of moles of Cl⁻ ion from the saturated solution of NaCl is approximately 5.42 moles, therefore, ionic product I.P. of the solution of Cl⁻ ions is larger than the solubility product of the solution, of the NaCl and according to Le C h a t e l i e r's principle, NaCl will precipitate out of the solution

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