Asked by Cj
What are the concentrations of benzoic acid and sodium benzoate in a solution that is buffered with a pH of 4.55 and has a freezing point of -2.0 degrees Celsius? (assume complete dissociation and a density of 1.01g/mL for the solution.)
Answers
Answered by
DrBob222
Several steps to this problem. Here is an outline.
1. Use the HH equation and solve for the ratio of base/acid; i.e., sodium benzoate to benzoic acid. Then convert that to percent of each.
2. Use the percents to calculate a van't Hoff factor. That is 2*%base + 1*%acid = total = i
3. Use delta T = iKf*m and solve for m
4. Use density to convert molality to molarity
5. Use the percents to convert to M of each component.
Good luck. Post your work if you get stuck.
1. Use the HH equation and solve for the ratio of base/acid; i.e., sodium benzoate to benzoic acid. Then convert that to percent of each.
2. Use the percents to calculate a van't Hoff factor. That is 2*%base + 1*%acid = total = i
3. Use delta T = iKf*m and solve for m
4. Use density to convert molality to molarity
5. Use the percents to convert to M of each component.
Good luck. Post your work if you get stuck.
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