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- For the amino acid glutamate, what fraction of the side-chain (R-group) will be ionized at pH = 3.5? At pH = 5.0?What is the pH, along with the concentration of each form of serine, in a 0.020 M solution of serine?For a weak acid with a pKa of 6.0, show how you would calculate the ration of acid to salt at pH 5.
- 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 Name Formula Acid Kb Ammonia NH3 NH4+ 1.8 x 10-5 Methylamine CH3NH2 CH3NH3 + 4.38 x 10-4 Ethylamine C₂H5NH₂ C₂H5NH3+ 5.6 x 10-4 Aniline C6H5NH3 + 3.8 x 10-10 CH;NH, C,H,N Pyridine CH;NH* 1.7 x 10-⁹ 1. Compute the poH of the buffer solution. (Supply answer up to the 1st decimal point)Describe three effects of pH on ionization of a weak acid or base that impact biological stability of a protein.Calculate [H2Asc], [HAsc-], [Asc2-], and the pH of 0.050 Mascorbic acid H2C6H6O6, H2Asc. (Ka1= 1.0x10-5and Ka2= 5x10-12).
- A dilute (~0.10 M) butanoic acid solution (aka butyric acid) has a pH of 4.6. To the nearest hundredth of a unit, what is the ratio of the acidic form to basic form of the molecules at this pH? (The pKa of butanoic acid is 4.82.)In the laboratory, a general chemistry student measured the pH of a 0.527 M aqueous solution of methylamine, CH3NH₂ to be 12.159. Use the information she obtained to determine the Kb for this base. Kb (experiment) = Show Transcribed Text In the laboratory, a general chemistry student measured the pH of a 0.524 M aqueous solution of pyridine, C,HSN to be 9.461. Use the information she obtained to determine the K, for this base. Kb (experiment) =n the laboratory, a general chemistry student measured the pH of a 0.354 M aqueous solution of diethylamine, (C2H5)2NH to be 12.177. Use the information she obtained to determine the Kb for this base. Kb(experiment) =
- what is the ph of 0.29 M of alanine1. Draw a structural formula for the major ionic form of the amino acid shown below when in aqueous solution at pH 3.0. 2. Draw a structural formula for the major ionic form of the amino acid shown below when in aqueous solution at pH 9.8.Valine (HV) is a diprotic amino acid with Ka1=5.18×10-3 and Ka2=1.91×10-10. Determine the pH of each of the solutions. a) A 0.216 M valine hydrochloride (H2V+CI-) solution. pH= b) A 0.216 M valine (HV) solution. pH= c) A 0.216 M sodium valinate (Na+V-) solution. pH=