11. Solutions in which the... a. [H3O+] is greater than 1 x 10-7M are acidic [Choose one: acidic, basic, or neutral] b. [H3O+] is less than 1 x 107 M are basic c. [OH-] is greater than 1 x 10-7 M are basic [Choose one: acidic, basic, or neutral] [Choose one: acidic, basic, or neutral] d. [OH-] is less than 1 x 107 M are acidic [Choose one: (acidic, basic, or neutral] e. [H3O+] is equal to 1 x 10-7 M are neutral [Choose one: acidic, basic, or neutral] 12. What is the concentration of H3O+ and OH for each of the following conditions? a. pH=8.0 [₂07] = 1x10 m [04²] = 1x10 m b. pH=6.50 [₂07] =3.2 X10 m [H] = c. pH = 10.60 3.1X108m -8 -4 H₂0]= 2.5x10m [H] = 4,0x10 m 13. If the pH> pKa in a buffer solution, which is larger, the concentration of the acid form or the concentration of base form. Bast form [A]

11. Solutions in which the... a. [H3O+] is greater than 1 x 10-7M are acidic [Choose one: acidic, basic, or neutral] b. [H3O+] is less than 1 x 107 M are basic c. [OH-] is greater than 1 x 10-7 M are basic [Choose one: acidic, basic, or neutral] [Choose one: acidic, basic, or neutral] d. [OH-] is less than 1 x 107 M are acidic [Choose one: (acidic, basic, or neutral] e. [H3O+] is equal to 1 x 10-7 M are neutral [Choose one: acidic, basic, or neutral] 12. What is the concentration of H3O+ and OH for each of the following conditions? a. pH=8.0 [₂07] = 1x10 m [04²] = 1x10 m b. pH=6.50 [₂07] =3.2 X10 m [H] = c. pH = 10.60 3.1X108m -8 -4 H₂0]= 2.5x10m [H] = 4,0x10 m 13. If the pH> pKa in a buffer solution, which is larger, the concentration of the acid form or the concentration of base form. Bast form [A]

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 129E: Are solutions of the following salts acidic, basic, or neutral? For those that are not neutral,...

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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
Both HF and HCN ionize in water to a limited extent. Which of the conjugate bases. F“ or CN”, is the stronger base? See Table 14.2.
Consider 50.0 mL of a solution of weak acid HA (Ka = 1.00 106), which has a pH of 4.000. What volume of water must be added to make the pH = 5.000?
The pH of a 0.20-M solution of HP is 1.92. Determine Ka far HF from these data.
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?
. Consider 0.25 M solutions of the following salts: NaCl. RbOC1, KI, Ba(ClO4),, and NH4NO3. For each salt, indicate whether the solution is acidic, basic, or neutral.
The pH of a 0.15-M solution of HSO4- is 1.43. Determine Ka for HSO4- from these data.
Which base in Table 14.3 is must appropriate for preparation of a buffer solution with a pH of 10.65? Explain your choice.
In a particular solution, acetic acid is 11% ionized at 25 C. Calculate the pH of the solution and the mass of acetic acid dissolved to yield 1.00L of solution.
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?
Sketch two graphs: (a) percent dissociation for weak acid HA versus the initial concentration of HA ([HA]0) and(b) H+ concentration versus [HA]0. Explain both.