The dissociation of lactic acid to lactate is shown in the reaction. Lactic acid has a pK₂ of 3.86. 0 OH Lactic acid [lactate] [lactic acid] OH 0.3548 Incorrect A solution containing a mixture of lactic acid and lactate was found to have a pH of 3.62. Calculate the ratio of the lactate concentration to the lactic acid concentration in this solution. What fraction of the lactic acid/lactate mixture is lactic acid? fraction lactic acid = 0.79 OH Incorrect Lactate 0 + H+

The dissociation of lactic acid to lactate is shown in the reaction. Lactic acid has a pK₂ of 3.86. 0 OH Lactic acid [lactate] [lactic acid] OH 0.3548 Incorrect A solution containing a mixture of lactic acid and lactate was found to have a pH of 3.62. Calculate the ratio of the lactate concentration to the lactic acid concentration in this solution. What fraction of the lactic acid/lactate mixture is lactic acid? fraction lactic acid = 0.79 OH Incorrect Lactate 0 + H+

Organic Chemistry

9th Edition

ISBN:9781305080485

Author:John E. McMurry

Publisher:John E. McMurry

Chapter20: Carboxylic Acids And Nitriles

Section20.4: Substituent Effects On Acidity

Problem 7P: Dicarboxylic acids have two dissociation constants, one for the initial dissociation into a...

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12. Bicine is an organic compound used as a buffering agent. It is one of Good's buffers and has a pKa of 8.354 at 25 °C. The molecular formula of bicine is C6H13NO4. Bicine can react with Ba(OH)2 according to the following reaction. 2 C6H13NO4 + Ba(OH)2 → Ba(C6H12NO4)2 + 2 H₂O It took a student worker 3 steps to make a buffer solution. First, a bicine solution is made by dissolving 37.47 grams bicine in enough water. The total volume is 200.00 mL. Then 250.00 mL Ba(OH)2 solution is prepared by adding 36.57 grams Ba(OH)2 solid and enough water. At the end, a buffer solution is made by mixing 157.89 mL of the above bicine solution and 89.32 mL of the above Ba(OH)2 solution. A. B. C. Determine the equilibrium concentration of bicine in the buffer solution. Please provider your answer below. A of Ba(C6H12NO4)2 in the buffer solution. Check answer Determine the equilibrium concentration M Please provider your answer below. A pH = Please provider your answer below. A $ Check answer…
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Lactic acid, CH3CH(OH)COOH, is a weak monoprotic acid with a melting point of 53 C. It exists as two enantiomers (Sec. 7-2f) that have slightly different Ka values. The D form has a Ka of 1.5 104 and the L form has a Ka of 1.6 104. The D form is synthesized by some bacteria. The L form is produced in muscle cells during anaerobic metabolism in which glucose molecules are broken down into lactic acid and molecules of adenosine triphosphate (ATP) are formed. When lactic acid builds up too rapidly in muscle tissue, severe pain results. (a) Which form of lactic acid (D or L) is the stronger acid? Explain your answer. (b) Determine the pKa that would be measured for a 50:50 mixture of the two forms of lactic acid in aqueous solution, pKa = log Ka (c) A solution of D-lactic acid is prepared. Use HL as a general formula for lactic acid, and write the equation for the ionization of lactic acid in water. (d) If 0.100-M solutions of these two acids (D and L) were prepared, calculate what the pH of each solution would be. (e) Before any lactic acid dissolves in the water, what reaction determines the pH? (f) Calculate the pH of a solution made by dissolving 4.46 g D-lactic acid in 500. mL of water. (g) Calculate the volume (mL) of 1.15-M NaOH(aq) required to completely neutralize 4.46 g of pure lactic acid. (h) Calculate the pH of the solution when exactly enough NaOH was added to neutralize all of the lactic acid for (i) the D form; (ii) the L form; and (iii) a 50:50 mixture of the two forms.
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