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A 1.100 L sample of HCl gas at 25∘C and 732.0 mm Hg was absorbed completely...

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Chemistry

A 1.100 L sample of HCl gas at 25∘C and 732.0 mm Hg was absorbedcompletely in an aqueous solution that contained 6.900 g of Na2CO3and 265.0 g of water.

What is the pH of the solution?

What is the freezing point of the solution?

What is the vapor pressure of the solution? (The vapor pressureof pure water at 25 ∘C is 23.76 mm Hg.)

Answer & Explanation Solved by verified expert
3.8 Ratings (557 Votes)

The number of mols of HCl = n = PV / RT = (732/760) atm*1.100 L /(0.0821*298)

                                             = 0.0433 mol

Thus, concentration of the solution = 0.0433 mol / 0.265 L = 0.163 mol/L

pH = -log [H+] = -log (0.163) = 0.786

--------------------------------------------------------------------------------------------------------------------------------------------------

Depression in freezing point = Kf* m

                                         = (1.860C) (6.9 g / 106 g/mol) (1000 / 265)

                                         = 0.450C

Hence - Freezing point of the substance = -0.450C

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