A 0.063 M solution of a base has a pH of 11.40. a What are the hydronium and hydroxide ion concentrations of this solution? [H3O+]= [OH-] = M M

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Chapter1: Chemical Foundations
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**Problem Description:**

A 0.063 M solution of a base has a pH of 11.40.

**Question:**

What are the hydronium and hydroxide ion concentrations of this solution?

**Solution:**

- \([H_3O^+]\) = _____ M
- \([OH^-]\) = _____ M

**Details:**

This exercise involves calculating the concentrations of hydronium ions \([H_3O^+]\) and hydroxide ions \([OH^-]\) in a basic solution, given the pH. The relationship between pH, pOH, and the ion concentrations can be used to find these values:

1. **Calculate pOH**: Use the formula \( \text{pOH} = 14 - \text{pH} \). 

2. **Find Hydroxide Ion Concentration**: The concentration of hydroxide ions is determined by the formula \([OH^-] = 10^{-\text{pOH}}\).

3. **Find Hydronium Ion Concentration**: Use \([H_3O^+] = 10^{-\text{pH}}\).

The calculated values will provide the molarity (M) for both hydronium and hydroxide ions in the solution.
Transcribed Image Text:**Problem Description:** A 0.063 M solution of a base has a pH of 11.40. **Question:** What are the hydronium and hydroxide ion concentrations of this solution? **Solution:** - \([H_3O^+]\) = _____ M - \([OH^-]\) = _____ M **Details:** This exercise involves calculating the concentrations of hydronium ions \([H_3O^+]\) and hydroxide ions \([OH^-]\) in a basic solution, given the pH. The relationship between pH, pOH, and the ion concentrations can be used to find these values: 1. **Calculate pOH**: Use the formula \( \text{pOH} = 14 - \text{pH} \). 2. **Find Hydroxide Ion Concentration**: The concentration of hydroxide ions is determined by the formula \([OH^-] = 10^{-\text{pOH}}\). 3. **Find Hydronium Ion Concentration**: Use \([H_3O^+] = 10^{-\text{pH}}\). The calculated values will provide the molarity (M) for both hydronium and hydroxide ions in the solution.
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