O Macmillan Learning For the diprotic weak acid H₂A, Kal = 2.1 x 10-6 and Ka2 = 7.2 × 10-9. What is the pH of a 0.0600 M solution of H₂A? pH= 3.95 Incorrect Answer What are the equilibrium concentrations of H2A and A² in this solution? 7.2 x10-9 [H₂A] = Incorrect Answer [A²-]= 1.12 x10 4 Incorrect Answer M M

O Macmillan Learning For the diprotic weak acid H₂A, Kal = 2.1 x 10-6 and Ka2 = 7.2 × 10-9. What is the pH of a 0.0600 M solution of H₂A? pH= 3.95 Incorrect Answer What are the equilibrium concentrations of H2A and A² in this solution? 7.2 x10-9 [H₂A] = Incorrect Answer [A²-]= 1.12 x10 4 Incorrect Answer M M

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases

Section16.2: Water And Ph Scale

Problem 3RC: If the pH of a solution containing the strong base Sr(OH)2 is 10.46 at 25C, what is the...

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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.
8-107 Following are pH ranges for several human biological materials. From the pH at the midpoint of each range, calculate the corresponding [H3O+]. Which materials are acidic, which are basic, and which are neutral? (a) Milk, pH 6.6-7.6 (b) Gastric contents, pH 1.0-3.0 (c) Spinal fluid, pH 7.3-7.5 (d) Saliva, pH 6.5-7.5 (e) Urine, pH 4.8-8.4 (f) Blood plasma, pH 7.35-7.45 (g) Feces, pH 4.6-8.4 (h) Bile, pH 6.8-7.0
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.
Find [OH+], [OH-] and the pH of the following solutions. (a) 30.0 mL of a 0.216 M solution of HCI diluted with enough water to make 125 mL of solution. (b) A solution made by dissolving 275 mL of HBr gas at 25C and 1.00 atm in enough water to make 475 mL of solution. Assume that all the HBr dissolves in water.
8-18 Which of these acids are monoprotic, which are diprotic, and which are triprotic? Which are amphiprotic? (a) H2PO4- (b) HBO32- (c) HCIO4 (d) C2H5OH (e) HSO3- (f) HS- (g) H2CO3
If the pH of a solution containing the strong base Sr(OH)2 is 10.46 at 25C, what is the concentration of Sr(OH)2? (a) 3.5 1011 M (b) 2.9 104 M (c) 6.9 104 M (d) 1.4 104 M
Using the acid ionization constant information given in Table 10-3, indicate which acid is the stronger in each of the following acid pairs. a. H3PO4 and H2PO4 b. H3PO4 and H2CO3 c. HPO42 and H2PO4 d. HC2H3O2 and HCN
How is acid strength related to the value of Ka? What is the difference between strong acids and weak acids (see Table 13-1)? As the strength of an acid increases, what happens to the strength of the conjugate base? How is base strength related to the value of Kb? As the strength of a base increases, what happens to the strength of the conjugate acid?
8-16 For each of the following, tell whether the acid is strong or weak. (a) Acetic acid (b) HCI (c) H3PO4 (d) H2SO4 (e) HCN (f) H2CO3
You mix a solution of a strong acid with a pH = 4.0 and an equal volume of another strong acid solution having a pH = 6.0. Is the final pH less than 4.0, equal to 4.0, between 4.0 and 5.0, equal to 5.0, between 5.0 and 6.0, equal to 6.0, or greater than 6.0? Explain.
Calculate [OH-] and pH in a solution in which the hydrogen sulfite ion, HSO3-, is 0.429 M and the sulfite ion is (a) 0.0249 M (b) 0.247 M (c) 0.504 M (d) 0.811 M (e) 1.223 M
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