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Calculate the pH of 50mls of 0.1100M arginine to which 20 mls PH of 0.1005M Hcl have been added.
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- Calculate the pH of 50.0 mLs of 0.10 M arginine to which 20.0 mLs of 0.10 M HCI have been added.Ethylamine (C2H5NH2) has a Kb value of 4.5x10–4. Calculate the pH of a buffer solution that is 0.00789 M ethylamine and 0.00546 M ethylammonium chloride.calculate the pH of 50.0 mLs of 0.10 M arginine hydrochloride to which 50.0 mLs of 0.10 M NaOH have been added.
- Sketch a titration curve of the amino acid isoleucine with pH on the y-axis and volume of titrant on the x-axis. Label each axis appropriately. Draw the chemical structures of the 3 possible forms of isoleucine in aqueous solution. Indicate on the graph the following: where each of the species predominates, the pKa values and the isoelectric point.What volume of 0.12 M HCl must be added to 1.5 g glycine amide to make buffer at pH 8.5? What volume of 0.08 M NaOH must be added to 1.1 g glycine amide hydrochloride to get a pH of 7.5?Suppose you want to make 250 mL 0.0700 M glycine buffer at pH 8.00. What mass of glycine amide and glycine amide HCl are needed? Hint: you need 2 eqns w/ 2 unknowns. Use the mb eqn and HH eqn. What mass of glycine amide and what volume of 0.400 M HCl are needed? What mass of glycine amide HCl and what volume of 0.600 M NaOH are needed?30ml of 0.06M solution of protonated form of anion amino acid methionine (H2A+) is treated with0.09M NaOH.calculate pH after addition of 20 ml of base.pKa1=2.28 and pKa=9.2 please answer this question .with explanation
- In titrating 10 ml of 0.1 M neutral amino acid (pKa1= 2, pKa2 8),the pH after the addition of 5 ml 0.1N NAOH will be 8.0 9.0 7.0 5.0 2.0 05AT PH O O OCalculate the volume, in liters, of 1.617 M KOH that must be added to a 0.111 L solution containing 9.17 g of glutamic acid hydrochloride (H3 Glu+CI, MW = 183.59 g/mol) to achieve a pH of 10.31. Glutamic acid (Glu) is an amino acid = 4.42, and with pKa values of pKal pka3 = 9.95. volume: = = 2.23, pKa2 L + NH3 Cг HC—CH 2 —CH₂—C—OH C=O OH Glutamic Acid HydrochlorideYou are given 0.7 M solution of the amino acid Lysine. pK1 (α-carboxyl group) = 2.18 pK2 (α- amino group) = 8.95 and pK3 (Side chain) = 10.53 Answer the following questions. a. Determine the pH of the solution if you add 26 mL 0.3 M HCl to 12 mL of the 0.7 M Lysine. Assume that Lysine is in isotonic state. Show all calculations. b. Draw the structure of the amino acid at the pH determined in question a
- The pK₂ of acetic acid, HC₂H3O2, is 4.96. A buffer solution was made using an unspecified amount of acetic acid and 0.1 moles of NaC2H3O2 in enough water to make 1.82 liters of solution. Its pH was measured as 4.04. How many moles of HC2H3O2 were used? Report your answer with 2 places past the decimal point. Do not put unit in your answer.An analytical chemist is titrating 99.1mL of a 0.7900M solution of aniline C6H5NH2 with a 0.2500M solution of HNO3 . The pKb of aniline is 9.37 . Calculate the pH of the base solution after the chemist has added 39.3mL 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.A compound has two carboxyls and one aminium group. The pKas of the groups are 1.9, 4.2, and 9.3, respectively. A biochemist has 100 mL of a 0.10 M solution of this compound at a pH of 5.6. She adds 39 mL of 0.1 M NaOH. To the nearest hundredth of a unit, what will be the pH of the solution after addition of the NaOH (assume full stirring to reach a new equilibrium)?
