NaCl is purified by adding HCl to a saturated solution of NaCl (317 g/L). Will pure NaCl precipitate when 30 mL of 4.5 M HCl is added to 0.15 L of saturated solution? Group of answer choices NaCl will precipitate from solution No NaCl will precipitate

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Rebekah Snow

Chemistry

9 December, 13:15

NaCl is purified by adding HCl to a saturated solution of NaCl (317 g/L). Will pure NaCl precipitate when 30 mL of 4.5 M HCl is added to 0.15 L of saturated solution? Group of answer choices NaCl will precipitate from solution No NaCl will precipitate

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Goon · Answer 1

If you add concentrated HCl solution to a saturated NaCl solution, you will drive the equilibrium of equation 1) back to the left by increasing the concentration of Cl - (aq). As a result, NaCl will re-crystallize in the solution. This is a demonstration of Le Châtelier's principle that states: if a system in equilibrium is disturbed, it will shift the equilibrium to counteract the disturbance.

1) NaCl (s) ↔ Na + (aq) + Cl - (aq)

2) HCl (aq) ↔ H + (aq) + Cl - (aq)

K = Ksp = [Na + (aq) ][Cl - (aq) ]

Ka =

[Cl - (aq) ] = Ka[HCl (aq) ]/[H + (aq) ]

Ksp / [Na + (aq) ] = Ka[HCl (aq) ]/[H + (aq) ]