You require 0.100 L of a buffer with pH = 4.35. On the shelf is a bottle of benzoic acid/sodium benzoate buffer with pH = 3.95. ??
The label also says [C7H5O2-] = 0.200 M. What mass of which substance (benzoic acid or sodium benzoate) should you add to 0.100 L of the buffer to obtain the desired pH? Ka of HC7H5O2 = 6.5 x 10-5 .
How would I solve this? I am running short on time...
The label also says [C7H5O2-] = 0.200 M. What mass of which substance (benzoic acid or sodium benzoate) should you add to 0.100 L of the buffer to obtain the desired pH? Ka of HC7H5O2 = 6.5 x 10-5 .
How would I solve this? I am running short on time...
1 Answer
You must add 4.4 g of sodium benzoate.
Explanation:
You have a buffer with pH = 3.95.
You need a buffer with pH = 4.35 ( more basic).
Thus, you must add a base ( sodium benzoate) to the buffer.
Step 1. Calculate the amounts of benzoic acid and sodium benzoate in 100 mL of the original buffer
The equilibrium involved is
#"HA" + "H"_2"O" ⇌ "H"_3"O"^"+" + "A"^"-"#
We can apply the Henderson-Hasselbalch equation:
#color(blue)(bar(ul(|color(white)(a/a)"pH" = "p"K_text(a) + log((["A"^"-"])/(["HA"]))color(white)(a/a)|)))" "#
For benzoic acid,
The original buffer contains 0.0330 mol of benzoic acid and 0.0200 mol of sodium benzoate.
Step 2. Calculate the additional moles of sodium needed for pH 4.35
Step 3. Calculate the mass of the additional sodium benzoate