The organic compound trishydroxymethylaminomethane is abbreviated Tris and is basic. The conjugate acid (TrisH+) has a pKa of 8.10.TrisHt+ H20= Tris + H30+Tris is commonly used as a component in buffer solutions to study biochemical reactions.Part AA buffer solution is prepared by mixing 12.5 mL of 0.100 mol L'HCl with 25 mL of 0.100 mol L-lTris. What is the pH of this buffer?Express your answer using two decimal places.femplates Symbols uado redo reset keyboard shortcuts help,pH =SubmitRequest AnswerPart BThe buffer was used to study an enzyme-catalyzed reaction in which 0.00030 mol of H30+was produced. What is the pH of the solution after the acid reacted with the buffer?Express your answer using two decimal places.Templates Symbols uado redo reset keyboard shortcuts helppH =

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The organic compound trishydroxymethylaminomethane is abbreviated Tris and is basic. The conjugate acid (TrisH+) has a pKa of 8.10. TrisH++ H20 = Tris + H30+ Tris is commonly used as a component in buffer solutions to study biochemical reactions. Part A A buffer solution is prepared by mixing 12.5 mL of 0.100 mol L-'HCI with 25 mL of 0.100 mol L-'Tris. What the pH of this buffer? Express your answer using two decimal places. Templates Symbols uado redo reset keyboard shortcuts help pH = Submit Request Answer • Part B The buffer was used to study an enzyme-catalyzed reaction in which 0.00030 mol of H30+ was produced. What is the pH of the solution after the acid reacted with the buffer? Express your answer using two decimal places. Templates Symbols uado redo reset keyboard shortcuts help, pH =

The organic compound trishydroxymethylaminomethane is abbreviated Tris and is basic. The conjugate acid (TrisH+) has a pKa of 8.10. TrisH++ H20 = Tris + H30+ Tris is commonly used as a component in buffer solutions to study biochemical reactions. Part A A buffer solution is prepared by mixing 12.5 mL of 0.100 mol L-'HCI with 25 mL of 0.100 mol L-'Tris. What the pH of this buffer? Express your answer using two decimal places. Templates Symbols uado redo reset keyboard shortcuts help pH = Submit Request Answer • Part B The buffer was used to study an enzyme-catalyzed reaction in which 0.00030 mol of H30+ was produced. What is the pH of the solution after the acid reacted with the buffer? Express your answer using two decimal places. Templates Symbols uado redo reset keyboard shortcuts help, pH =

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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10. One characteristic of blood that we rarely give a thought to is its pH. The pH of blood must be held remarkably constant, varying only by a few hundredths of a pH unit from 7.36 to 7.40. Blood pH is kept constant primarily through the buffering action of the bicarbonate ion, HCO3-, and dissolved carbon dioxide, commonly represented as H2CO3. The second ionization is negligible in blood so that H2CO3 can be treated as a monoprotic acid. A) If the Ka1 for H2CO3 is 4.2 * 10-7, what ratio of HCO3- to H2CO3 is necessary to produce a buffer of pH 7.40? B) What is the pH of a buffer that is 1.0 M NaHCO3 and 1.0 M H2CO3? C) If you have 1.00 L of the buffer described above (1.0 M NaHCO3 and 1.0 M H2CO3) and 10.0 mL of 0.100 M HCl is added to it, what is the new pH? D) Just to prove that the buffer helps minimize changes in pH, calculate the pH of a solution prepared by adding 10.0 mL of 0.1 M HCl to 1.00 L of pure water.
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1) You are given a solution wherein [OH^-] is 1/4th of the concentration of [H^+]. What is the pH of this solution? 2)What is the change in pH when a few drops of strong base containing 3.0 x 10^-3moles of [OH^-] is added to a liter of either of the following two buffered solutions at pH6.4 (you can assume the volume remains approximately constant) i) a 250 mM solution of buffer A (pKa = 5.0) ii) a 250 mM solution of buffer B (pKa = 7.2) 3. Which solution is the more effective buffer at pH 6.40(provide a rationale for your answer)?
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A solution is made by mixing 0.400M in formic acid, HCOOH, and 1.00M in sodium formate, HCOONa? Ka=1.80x10-4. The total volume is 1.00L. What is the pH of this solution?