I am a winemaker and in the course of my work I simply do not understand how to do a calculation of this sort. We usually express acidity (in wine) in terms of titratable acidity in grams tartaric acid per liter. Here is the information that I have:
If 500 mg/L of lactic acid is added to distilled water and NaOH is added until the pH = 3.1, what are the final amounts of each species in the acid equilibrium? What would be expressed as titratable acidity in grams/L of tartaric acid? I know that the formula for lactic acid is C3H6O3 and the pKa = 3.86. The formula for tartaric acid is C4H606.
Any guidance or direction on how to perform this calculation this would be most appreciated.© BrainMass Inc. brainmass.com October 16, 2018, 4:48 pm ad1c9bdddf
First I am going to include some standard home work problems for equilibrium and some of my explanations regarding these sort of problems which should be very ...
This solution provides a very detailed response which illustrates how to complete this problem. Furthermore, this solution provides an additional example set of problems which are similar to the one being asked in this case, so that further practice can be done on these types of questions. To access both the solution and additional question set, two Word documents need to be opened.
Plotting a titration curve for Ala and His
Here is the problem:
1. Assume you have a solution containing 0.1 mol of Ala adjusted to pH = 0.5 with HCl. You begin adding 1.0 M NaOH. Plot (do not sketch) the resulting titration curve (pH vs. moles NaOH added) showing all inflection points. Show your calculations and be sure to state your assumptions.
2. Plot a similar titration curve for a solution containing 0.1 mol of His at pH = 0.5. (pKa values: Ala: alpha-COOH = 2.3, alpha-NH2 = 9.7; His: alpha-COOH = 1.8, alpha-NH2 = 9.2, Imidazole = 6.0).View Full Posting Details