Please please please show all work for a 5 star rating!!!! Consider the titratio

Question

Please please please show all work for a 5 star rating!!!!


Consider the titration of 43.2 mL of .220M HF with .220M NaOH. Calculate the pH at each of the following points.

a) How many milliliters of base are required to reach the equivalence point?
b) Calculate pH after the addition of 10.8 mL base.
c) Calculate the pH at halfway to the equivalence point.
d) Calculate the pH at the equivalence point.
e) Calculate the pH after the addition of 86.4 mL of base.

Explanation / Answer

HF(aq) --> H+(aq) + F-(aq) Ka = 7.08 * 10^-4 you add 10 ml 0.2 M NaOH [HF] initial = 0.25 mole/L = x moles/ 0.040 L ==> x moles = 0.01 moles HF 10ml * 0.2 moles NaOH/1000ml = 0.002 moles OH- by adding the base you deplete the HF but you add F- so you are now building a buffer mole HF left = 0.01 - 0.002 moles = 0.008 moles HF moles F- generated = 0.002 final volume = 40 ml + 10 ml = 50 ml = 0.050 L [HF] final = 0.008 moles HF/0.050 L = 0.16 M [F-] final = 0.002 moles F-/0.050 L = 0.04 M pH = pKa + log[F-]/[HF] = 3.15 + log(0.04/0.16) = 2.55

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