2. 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 Check answer Determine the equilibrium concentration of Ba(C6H12NO4)2 in the buffer solution. M Please provider your answer below. 000 A ← pH = Please provider your answer below. M से Check answer Determine the pH of the buffer solution.

2. 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 Check answer Determine the equilibrium concentration of Ba(C6H12NO4)2 in the buffer solution. M Please provider your answer below. 000 A ← pH = Please provider your answer below. M से Check answer Determine the pH of the buffer solution.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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please help with this question. it's not an assay, but calculation. thanks
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Time to purify biochemisfunase! To do this, you’ll need to make MORE buffers. One of the buffers that you need to make requires 150 mM Tris (pH 8), 250 mM sodium chloride (NaCl) and 2 mM dithiothreitol (DTT, a reducing agent that prevents the formation of disulfide bonds in proteins). Your jolly postdoc friend wants you first to make 500 ml of a1.0M Tris stock solution before making the buffer. Describe how you would make this stock solution, and show all calculations.
C. A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) = H* (aq) + A¯(aq) The equilibrium concentrations of the reactants and products are [HA] = 0.120 M, [H*] = 3.00 x 10-4 M, and [A- = 3.00 x 10-4 M. Calculate the Ka value for the acid HA. Ka : Incorrect
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Consider the quilibrium reaction between X and Y, as shown below: X=Y AG The reaction is started with 10 mmol of X; no Y is initially present. After 48 hours, analysis reveals the presence of 10 mmol of X and 0 mmol of Y. Which is the most likely explanation? = −1 - 45 kJ mol X and Y have reached equilibrium concentrations. An enzyme has shifted the equilibrium toward X. Formation of Y is kinetically slow; equilibrium has not been reached by 48 hours. Formation of Y is thermodynamically unfavorable. Two of the above explanations are reasonable.
Good hand written explanation Asap