3. A typical vitamin C tablet contains pure ascorbic acid H2C6H606 (a weak, diprotic acid).If 2 tablets are dissolved in about a cup of water, the resulting concentration of theascorbic acid is 0.0115 M.a. Give the equation for the dissociation for the first ionization (loss of the first acidicarlt el todW baiH broosz arit otH). This ionization has a Ka of 8.00 x 10°.b. What is the equilibrium concentration for all species from the first ionization? c. Give the equation for the dissociation for the second ionization (loss of the secondacidic H from the CB of step a).(blsp sire Non)0 Mboon eniatrI4 5 497d. What is the equilibrium concentration for all species in the second ionization if the Kafor the second H is 1.6 x 10-122Drertamine eT srir men es llo nol nor onon murndilups orit ai toriW de. Combining your answers from b and d, what is the total H3O* concentration, pH, pOH,and % ionization?

a.) To write the dissociation equation , we just ionise the given compound into its ions . b.) To…

3. A typical vitamin C tablet contains pure ascorbic acid H2C6H6O6 (a weak, diprotic acid). If 2 tablets are dissolved in about a cup of water, the resulting concentration of the ascorbic acid is 0.0115 M. a. Give the equation for the dissociation for the first ionization (loss of the first acidic H). This ionization has a Ka of 8.00 x 10-5. b. What is the equilibrium concentration for all species from the first ionization?

3. A typical vitamin C tablet contains pure ascorbic acid H2C6H6O6 (a weak, diprotic acid). If 2 tablets are dissolved in about a cup of water, the resulting concentration of the ascorbic acid is 0.0115 M. a. Give the equation for the dissociation for the first ionization (loss of the first acidic H). This ionization has a Ka of 8.00 x 10-5. b. What is the equilibrium concentration for all species from the first ionization?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 57QAP: Chromic acid, H2CrO4, is commonly obtained by adding concentrated H2SO4 to a dichromate. It is used...

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Consider a solution prepared by mixing a weak acid HA. HCl, and NaA. Which of the following statements best describes what happens? a. The H+ from the HCl reacts completely with the A from the NaA. Then the HA dissociates somewhat. b. The H+ from the HCl reacts somewhat with the A from the NaA to make HA, while the HA is dissociating. Eventually you have equal amounts of everything. c. The H+ from the HCl reacts somewhat with the A from the NaA to make HA while the HA is dissociating. Eventually all the reactions have equal rates. d. The H+ from the HCl reacts completely with the A from the NaA. Then the HA dissociates somewhat until too much H+ and A are formed, so the H+ and A react to form HA, and so on. Eventually equilibrium is reached. Justify your choice, and for choices you did not pick, explain what is wrong with them.
Benzoic acid (K a=6.6105)is present in many berries. Calculate the pH and % ionization of a 726-mL solution that contains 0.288 mol of benzoic acid.
. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?
A buffer is prepared in which the ratio [ H2PO4 ]/[ HPO42 ]is 3.0. (a) What is the pH of this buffer? (b) Enough strong acid is added to convert 15% of HPO42- to H2PO4-. What is the pH of the resulting solution? (c) Enough strong base is added to make the pH 7.00. What is the ratio of [H2PO4-] to [HPO42-] at this point?
At 25C, a 0.327 M solution of a weak acid HX has a pH of 5.12. What is G for the dissociation of the weak acid?
A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?
Chromic acid, H2CrO4, is commonly obtained by adding concentrated H2SO4 to a dichromate. It is used to clean glass. For chromic acid, Ka is 1.8101 and 3.2107 for its first and second dissociation, respectively. Write the overall equation and calculate K for the complete dissociation of chromic acid.
. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
The titration of Na2CO3 with HCl bas the following qualitative profile: a. Identify the major species in solution at points AF. b. Calculate the pH at the halfway points to equivalence, B and D. (Hint: Refer to Exercise 113.)
Write the Lewis structures of the reactants and product of each of the following equations, and identify the Lewis acid and the Lewis base in each: (a) CS2+SHHCS3 (b) BF3+FBF4 (c) I+SnI2SnI3 (d) Al(OH)3+OHAl(OH)4 (e) F+SO3SFO3