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Derive the Henderson- Hasselbalch equation for the dissociation of a weak base, B, in terms of pOH and pKb.
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- Write the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ionThe concentration of acetylcholine (a neurotransmitter) in a sample can be determined from the pH changes that accompany its hydrolysis. When the sample is incubated with the enzyme acetylcholinesterase, acetylcholine is converted to choline and acetic acid, which dissociates to yield acetate and a hydrogen ion. CНз CHз Нао — сHz— CH "N— снз но-сн— сH,-"N-CH; + CH;— с-о+ н* CH3-C-0- сHз CHз Choline Acetylcholine Acetate In a typical analysis, 11 mL of an aqueous solution containing an unknown amount of acetylcholine had a pH of 7.70. When incubated with acetylcholinesterase, the pH of the solution decreased to 6.89. Assuming there was no buffer in the assay mixture, determine the number of moles of acetylcholine in the 11 mL sample.(a) The PH of rain water collected from two cities A and B was found to be 6 and 5 respectively. Water of which city is more acidic? Find out the ratio of hydrogen ion concentration in the two samples of rain water?
- In the laboratory, a general chemistry student measured the pH of a 0.470 M aqueous solution of methylamine, CH3NH2 to be 12.163. Use the information she obtained to determine the Kh for this base. Ку(еxperiment) = 6.53x10^_4 An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer.A 0.018 M solution of salicylic acid, HOC6H4CO2H, has the same pH as 0.0038 M HNO3solution. (a) Write an equation for the ionization of salicylic acid in aqueous solution. (Assume only the –CO2H portion of the molecule ionizes.) (b) What is the pH of solution containing 0.018 M salicylic acid? (c) Calculate the Ka of salicylic acid.Three acids found in foods are lactic acid, LA, (in milk products), oxalic acid, OA, (in rhubarb), and malic acid, MA (in apples). The pKa values are LA =3.88, OA =1.23, and MA =3.40. Which list has the conjugate bases of these acids, lactate, oxalate, and malate, in order of decreasing strength? O lactate > malate > oxalate lactate > oxalate > malate malate > lactate > oxalate oxalate > malate > lactate
- Chemical Principles:The Quest for Insight 6H.18 50.0 mL of 0.25 M CH3NH2(aq) was appropriate at 0.35 M HCl(aq).(a) What is the initial pH of 0.25 M CH3NH2(aq)?(b) What is the pH after adding 15.0 mL of 0.35 M HCl(aq)?(c) What is the volume of 0.35 M HCl (aq) required to reach the midpoint of the stoichiometric point?(d) Calculate the pH at this midpoint.(e) What is the volume of 0.35 M HCl(aq) required to reach the stoichiometric point?(f) Calculate the pH at the stoichiometric point.(g) Using Table 6H.2, select the appropriate indicator for this application.The ionization constant Ka, for HCN(aq) is 4.3 x 10^-10. What is the pH of a 0.22 molar solution of sodium cyanide, which contains the cyanide ion?Consider the dissociation of hydrocyanic acid in aqueous solution HCN - CN + H* for which K, is 4.9 x 101°. (i) Find the pH of a solution initially 102 M in HCN, and the degree of dissociation of the HCN, a. (ii) To this solution is added more CN' until [CN'] = (0.1 M. What is the new pH of the solution? (ii) Without making a new numerical cakculation, explain qualitatively how the degree of dissociation would change if the solution is diluted.
- The value of K for acetylsalicylic acid (aspirin) is 3.00x104. What is the value of Kp, for its conjugate base, CH,04? An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer.Propionic acid, HC3H5O2, has Ka= 1.34 x 10–5. (a) What is the molar concentration of H3O+ in 0.15 M HC3H5O2 and the pH of the solution? (b) What is the Kb value for the propionate ion, C3H5O2–? (c) Calculate the pH of 0.15 M solution of sodium propionate, NaC3H5O2. (d) Calculate the pH of solution that contains 0.12 M HC3H5O2 and 0.25 M NaC3H5O2.Solubility of gases in water increases with increasing mass. Explain? What is the relationship between the value of pKa and the strength of a weak acid?