Histidine has ionizable groups with pKa values of 1.8, 6.0, and 9.2, as shown below (His 5 imidazole group). A biochemist makes up 100 mL of a 0.100 M solution of histidine at a pH of 5.40. She then adds 40 mL of 0.10 M HCl. What is the pH of the resulting solution?
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Histidine has ionizable groups with pKa values of 1.8,
6.0, and 9.2, as shown below (His 5 imidazole group). A biochemist
makes up 100 mL of a 0.100 M solution of histidine at
a pH of 5.40. She then adds 40 mL of 0.10 M HCl. What is the
pH of the resulting solution?
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- For a weak acid with a pKa of 6.0, show how you would calculate the ration of acid to salt at pH 5.Give typed full explanation not a single word hand written otherwise leave it Calculate the isoelectric point of the amino acid histidine by plotting the titration curve. (pka values α-COOH=1.82, α-NH2= 9.17, imidazole= 6.0)The measured pH of a 0.100 M solution of triethylamine (NEt3) is 11.68. What pKa of triethylammonium (HNEt3+) is implied by this data? Enter your response to the nearest 0.01.
- 1) You are asked to prepare a buffer for a protein assay. This protein works best at a slightly acidic pH of 5.5. a. From the list of Acids and conjugate bases which pair would you pick. (The list is in the attached image) b. You are asked to make a 1M stock solu on of the Buffer, how many grams of each acid and base would you need to make a 500mL stock. c. For the experiment, the final concentra on of the buffer should be 50mM. How many mL of your stock would you need to make 2L. Hint: M1V1=M2V2Given that pKb for iodate ion (IO-3) is 13.83, find the quotient [HIO3]/[IO-3] in a solution of sodium iodate at (a) pH 7.00; (b) pH 1.00.Tyrosine is a triprotic weak acid, with pKa1=2.41, pKa2=8.67, and pKa3=11.01. a) calculate the final [OH-] of a solution that starts with .30M of the fully basic form. Do not assume the concentration of base is constant. b) at what pH range(s) would tyrosine act best as a buffer? c) calculate the pH of a solution at equilibrium which started with 0.043M at the monoprotonated H2A- form *Please show all work and not just answers, I'm looking to understand how to solve problems like these! TIA
- describe the curve and why pH = pka at half equivalence pointWhat is the pKa of the conjugate acid of a base that has a Kb value equal to 2.1 × 10-7? Report your answer to the hundredths place. Assume the temperature is 25ºC.Calculate the pH of 50mls of 0.1100M arginine to which 20 mls PH of 0.1005M Hcl have been added.
- Properties of a Buffer 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 of 9.6, can exist either in the protonated form or as the free base , because of the reversible equilibrium In what pH range can glycine be used as an effective buffer due to its amino group? In a 0.1 m solution of glycine at pH 9.0, what fraction of glycine has its amino group in the form? 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 exactly 10.0? When 99% of the glycine is in its form, what is the numerical relation between the pH of the solution and the of the amino group? Please answer all of these questions, especially C please write in detail.To purify a certain protein, you were required to prepare a 0.10 M glycine buffer at pH 9.4. Unfortunately, the stockroom has run out of glycine. However, the lab aides were able to find two 0.10 M glycine solutions with pH of 9.0 and 10.0. What volumes of the solutions must you mix to obtain 200.0 mL of the required buffer?The pKa values of 4 acids are given below. Acid HA1 HA2 HA3 HA4 pKa 4.76 3.45 7.63 5.23 Which of the following solutions does have the highest pH? Choose one option only. Options: a. 0.30 M A2- (aq) (conjugate base of HA2) b. 0.30 M A3- (aq) (conjugate base of HA3) c. 0.30 M A1- (aq) (conjugate base of HA1) d. 0.30 M A4- (aq) (conjugate base of HA4) e. All the 0.30 M bases in this question have the same solution pH.