Identify the species represented by each curve in the fractional composition diagram of a tetraprotic acid (H₂A) with pK, valuesof 2.00, 5.00, 7.00, and 10.00.Fractional composition#H₂A=1.00-0.90-0.80-0.70-0.60-0.50-0.40-0.30.₁+ =0.20-0.10-aH₂A =H₂A²- =aHA¹ =0Calculate the fraction of the tetraprotic acid in each of its forms at pH 4.90.H₂A™H₂A¹-XXO0.010.650H₂A0.320.02HA¹-8 9 10 11 12 13 14PHA+Answer Bank00

Identify the species represented by each curve in the fractional composition diagram of a tetraprotic acid (H₂A) with pK, values of 2.00, 5.00, 7.00, and 10.00. Fractional composition HA 1.00- 0.90- = 0.80- 0.70- 0.60- 0.50- 0.40- 0.30. H₂A™ H₂A¹- XXO 0.20- 0.10- 0 H₂A HA¹ 0.01 Calculate the fraction of the tetraprotic acid in each of its forms at pH 4.90. - 8 9 10 11 12 13 14 PH A+ Answer Bank 00

Identify the species represented by each curve in the fractional composition diagram of a tetraprotic acid (H₂A) with pK, values of 2.00, 5.00, 7.00, and 10.00. Fractional composition HA 1.00- 0.90- = 0.80- 0.70- 0.60- 0.50- 0.40- 0.30. H₂A™ H₂A¹- XXO 0.20- 0.10- 0 H₂A HA¹ 0.01 Calculate the fraction of the tetraprotic acid in each of its forms at pH 4.90. - 8 9 10 11 12 13 14 PH A+ Answer Bank 00

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 99QAP: Each box represents an acid solution at equilibrium. Squares represent H+ ions. Circles represent...

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Tartaric acid is a weak diprotic fruit acid with Ka1 = 1.0 103 and Ka2 = 4.6 105. a Letting the symbol H2A represent tartaric acid, write the chemical equations that represent Ka1 and Ka2. Write the chemical equation that represents Ka1 Ka2. b Qualitatively describe the relative concentrations of H2A, HA, A2, and H3O+ in a solution that is about 0.5 M in tartaric acid. c Calculate the pH of a 0 0250 M tartaric acid solution and the equilibrium concentration of [H2A]. d What is the A2 concentration in solutions b and c?
For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)
Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
Using the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?
Each box represents an acid solution at equilibrium. Squares represent H+ ions. Circles represent anions. (Although the anions have different identities in each figure, they are all represented as circles.) Water molecules are not shown. Assume that all solutions have the same volume. (a) Which figure represents the strongest acid? (b) Which figure represents the acid with the smallest Ka? (c) Which figure represents the acid with the lowest pH?
Are solutions of the following salts acidic, basic, or neutral? For those that are not neutral, write balanced chemical equations for the reactions causing the solution to be acidic or basic. The relevant Ka and Kb values are found in Tables 13-2 and 13-3. a. NaNO3 b. NaNO2 c. C5H5NHClO4 d. NH4NO2 e. KOCl f. NH4OCl
Two strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?
The following illustration displays the relative number of species when an acid, HA, is added to water. a. Is HA a weak or strong acid? How can you tell? b. Using the relative numbers given in the illustration, determine the value for Ka and the percent dissociation of the acid. Assume the initial acid concentration is 0.20 M.
Values of Kw as a function of temperature are as follows: Temperature(C) Kw 0 1.14 1015 25 1.00 1014 35 2.09 1014 40. 2.92 1014 50. 5.47 1014 a. Is the autoionization of water exothermic or endothermic? b. Calculate [H+] and [OH] in a neutral solution at 50.C.