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11 Dec 2019

Calculate the pH of each of the following solutions and determine whether the solutions are neutral, acidic, or basic.

a. [H⁺]= 4.8x10^-4 M b. [OH^-]=2.5x10^-9 M c. [OH^-]= 3.2x10^-6 M

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9.35 Determine the pH of water solutions with the following characteristics. Classify

each solution as acidic, basic, or neutral.

a) [H+] = 1.0 x10-4 M

b) [OH-] = 5.0 x10-2 M

c) [H+] = [OH-]

d) [H+] = 8.0 x10-9 M

e) [OH-] = 4.0 x10-10 M

Calculate [H⁺] for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (a) [OH^-] = 0.00045 M; (b) [OH^-] = 8.8 × 10^-9 M; (c) a solution in which [OH^-] is 100 times greater than [H⁺].

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Calculate the pH of each of the following solutions and determine whether the solutions are neutral, acidic, or basic.

a. [H⁺]= 4.8x10^-4 M b. [OH^-]=2.5x10^-9 M c. [OH^-]= 3.2x10^-6 M

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Calculate the pH of each of the following solutions and determine whether the solutions are neutral, acidic, or basic. a. [H+]= 4.8x10-4 M b. [OH-]=2.5x10-9 M c. [OH-]= 3.2x10-6 M

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Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

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Calculate the pH of each of the following solutions and determine whether the solutions are neutral, acidic, or basic.

a. [H⁺]= 4.8x10^-4 M b. [OH^-]=2.5x10^-9 M c. [OH^-]= 3.2x10^-6 M