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54 For each of the following solutions, calculate [OH ] from [H;O*], or [H30*] from [OH]. Classify each solution as acidic, basic, or neutral. (a) [H3O*] = 3.4 × 10-9 M (c) [OH] = 1.0 x 10-10 M (b) [OH¯] = 0.010 M (d) [H3O*] = 1.0 × 10-7 M %3D %3D %3D

54 For each of the following solutions, calculate [OH ] from [H;O*], or [H30*] from [OH]. Classify each solution as acidic, basic, or neutral. (a) [H3O*] = 3.4 × 10-9 M (c) [OH] = 1.0 x 10-10 M (b) [OH¯] = 0.010 M (d) [H3O*] = 1.0 × 10-7 M %3D %3D %3D

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Can you please question 14.54 and all of the sub problems and show all of the steps to the solution 

**Dissociation of Water; pH (Sections 14.4-14.6)** **Exercise 14.54** For each of the following solutions, calculate \([OH^-]\) from \([H_3O^+]\), or \([H_3O^+]\) from \([OH^-]\). Classify each solution as acidic, basic, or neutral. (a) \([H_3O^+]\) = \(3.4 \times 10^{-9}\) M (b) \([OH^-]\) = 0.010 M (c) \([H_3O^+]\) = \(1.0 \times 10^{-10}\) M (d) \([H_3O^+]\) = \(1.0 \times 10^{-7}\) M (e) \([H_3O^+]\) = \(8.6 \times 10^{-5}\) M **Exercise 14.55** For each of the following solutions, calculate \([OH^-]\) from \([H_3O^+]\). Classify each solution as acidic, basic, or neutral. (a) \([OH^-]\) = \(5.6 \times 10^{-9}\) M (b) \([H_3O^+]\) = \(2.0\) M (c) \([OH^-]\) = \(1.0 \times 10^{-10}\) M (d) \([OH^-]\) = \(1.5 \times 10^{-3}\) M Note: The exercises require calculations based on the concentrations of hydronium \([H_3O^+]\) and hydroxide \([OH^-]\) ions to determine the nature of the solution (acidic, basic, or neutral).
Transcribed Image Text:**Dissociation of Water; pH (Sections 14.4-14.6)** **Exercise 14.54** For each of the following solutions, calculate \([OH^-]\) from \([H_3O^+]\), or \([H_3O^+]\) from \([OH^-]\). Classify each solution as acidic, basic, or neutral. (a) \([H_3O^+]\) = \(3.4 \times 10^{-9}\) M (b) \([OH^-]\) = 0.010 M (c) \([H_3O^+]\) = \(1.0 \times 10^{-10}\) M (d) \([H_3O^+]\) = \(1.0 \times 10^{-7}\) M (e) \([H_3O^+]\) = \(8.6 \times 10^{-5}\) M **Exercise 14.55** For each of the following solutions, calculate \([OH^-]\) from \([H_3O^+]\). Classify each solution as acidic, basic, or neutral. (a) \([OH^-]\) = \(5.6 \times 10^{-9}\) M (b) \([H_3O^+]\) = \(2.0\) M (c) \([OH^-]\) = \(1.0 \times 10^{-10}\) M (d) \([OH^-]\) = \(1.5 \times 10^{-3}\) M Note: The exercises require calculations based on the concentrations of hydronium \([H_3O^+]\) and hydroxide \([OH^-]\) ions to determine the nature of the solution (acidic, basic, or neutral).
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