The amino acid glycine is often used as the main ingredient of a buffer in biochemical experiments. The amino group of glycine, which has a pK, of 9.6, can exist either in the protonated form -NH equilibrium or as the free base -NH₂, because of the reversible RÃNH →R-NH, + H* In what pH range can glycine be used as an effective buffer due to its amino group? How much 5 M KOH must be added to 1.0 L of 0.1 M glycine at pH 9.0 to bring its pH to 10.0? In a 0.1 M solution of glycine at pH 9.0, what fraction of glycine has its amino group in the-NH; form? When 99% of the glycine is in its -NH3 form, what is the numerical relation between the pH of the solution and the pK, of the amino group?

You have 1 M (1 mol/L) solution of amino acid. This amino acid has an alpha carboxyl group with pKa = 2.0 and an alpha- amino group with pKa = 10.0. The pH of the solution is 7.0. Calculate the concentration of the molecular form of this amino acid that has carboxyl group protonated (COOH) and, at the same time, the amino group deprotonated (NH2).

An analytical chemist is titrating 184.0 mL of a 0.5400M solution of propylamine (C,H,NH,) with a 0.8600M solution of HNO3. The p K, of propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 60.2 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places.

An analytical chemist is titrating 191.3 mL of a 0.2000 M solution of propylamine (C,H,NH,) with a 0.1100 M solution of HNO3. The p K, of propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 416.1 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places.

The pl of the amino acid leucine is 5.98. A sample of leucine is placed in a solution buffered at a pH of 5.98. Then two electrodes are placed into the solution and connected to a battery. Toward which electrode will the majority of the leucine migrate?

An analytical chemist Is titrating 248.1 mL of a 0.3600M solution of diethylamine ((C,H,) NH) with a 0.5000M solution of HNO,. The p K, of diethylamine 3' is 2.89. Calculate the pH of the base solution after the chemist has added 191.9 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. 3. Round your answer to 2 decimal places. do PH = Ar Explanation Check 2021 McGraw-Hill Education. All Rights Reserved Terms of Use Privacy Accessibility i 3:20 Chp ぐ う esc ( backs & # $ 8. 9. 4 1

An analytical chemist is titrating 173.3 mL of a 0.1600M solution of diethylamine ((C₂H)2NH) with a 0.05100M solution of HCIO4. The pK, of diethylamine is 2.89. Calculate the pH of the base solution after the chemist has added 602.7 mL of the HCIO solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HCIO solution added. Round your answer to 2 decimal places.

An analytical chemist is titrating 75.2 mL of a 0.5800 M solution of trimethylamine ((CH3)N) with a 0.2600M solution of HNO3. The p K₂ of trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 197.6 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH = 0 X 5 4

An analytical chemist is titrating 83.2mL of a 0.6200M solution of diethylamine C2H52NH with a 0.3300M solution of HNO3 . The pKb of diethylamine is 2.89 . Calculate the pH of the base solution after the chemist has added 28.7mL of the HNO3 solution to it.   Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added.   Round your answer to 2 decimal places.

Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.62 M in this salt. The desired pH of the buffer should be equal to 4.5. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula Ammonia Methylamine Ethylamine Aniline NH3 CH;NH2 CH;NH2 CH;NH, C;H;N NH,+ CH;NH;* CH$NH;* CH;NH;* C;H;NH* 1.8 × 10-5 4.38 x 10-4 5.6 x 10-4 3.8 x 10-10 1.7 x 10-9 Pyridine 3. Compute the concentration of the weak base in Molarity. (Write your answer in 3 decimal places without the unit).