Calculate the pH of a solution prepared by mixing 0.0870 mol of chloroacetic acid plus 0.0250 mol of sodium chloroacetate in 1.00 L of water. First do the calculation by assuming that the concentrations of HA and A- equal their formal concentrations. The pK, of chloroacetic acid is 2.865. pH = 2.323 Then do the calculation with [HA] and [A-] from Equations 9-21 and 9-22. [HAJ = FHA – [H*]+ [OH¯] (9-21) [A-] = FA + [H*]- [OH-] (9-22)
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![Calculate the pH of a solution prepared by mixing 0.0870 mol of chloroacetic acid plus 0.0250 mol of sodium chloroacetate in
1.00 L of water.
First do the calculation by assuming that the concentrations of HA and A- equal their formal concentrations. The pK, of
chloroacetic acid is 2.865.
pH =
2.323
Then do the calculation with [HA] and [A-] from Equations 9-21 and 9-22.
[HA] = FHA – [H*]+ [OH¯]
(9-21)
[A] = FA- + [H*] – [OH-]
(9-22)
8.54 x103
pH =
Incorrect
Using first your head, and then the Henderson-Hasselbalch equation, find the pH of a solution prepared by dissolving all the
following compounds in one beaker containing a total volume of 1.00 L: 0.250 mol CICH,CO,H, 0.090 mol CICH,CO, Na,
0.080 mol HNO,, and 0.080 mol Ca(OH),. Ca(OH), provides 2 OH-.
pH =
2.865](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc02bfde4-a78d-4551-93f6-03d589a5c8dc%2F33fab5ff-ed5b-4539-8883-f5b22f11ac6f%2Fovoblrs_processed.png&w=3840&q=75)
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