We dissolve 4.44 g of an unknown acid, HA, in enough water to produce 25.0 mL...

We dissolve 4.44 g of an unknown acid, HA, in enough water to produce 25.0 mL of solution. The pH of this solution of HA(aq) is 1.44. We titrate this solution with a 0.250 M solution of NaOH. It takes 38.8 mL of the NaOH solution to reach the equivalence point. The temperature is 25^oC.

(a) What is the molar mass of HA?

(b) What is the pK_a value of HA(aq)?

(c) What is the pH at the equivalence point?

(d) What is the pH at the midpoint in the titration when you have as much HA(aq) as A^-(aq)?

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Expert Solution

queen_honey_blossom answered 1 year ago

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