https://file.aiquickdraw.com/mathbot/file/1728074546321dq9mw1ka.jpg

The problem asks for the concentration of \( OH^- \) given that the \( H_3O^+ \) concentration is \( 2.0 \times 10^{-7} \, M \) at 25°C.

To solve this, we can use the relationship between the hydronium ion concentration \( [H_3O^+] \) and hydroxide ion concentration \( [OH^-] \) in water at 25°C:

\[
K_w = [H_3O^+][OH^-]
\]

Where:
- \( K_w \) is the ionization constant for water at 25°C, which is \( 1.0 \times 10^{-14} \).

Rearranging the equation to solve for \( [OH^-] \):

\[
[OH^-] = \frac{K_w}{[H_3O^+]}
\]

Now substituting the given values:

\[
[OH^-] = \frac{1.0 \times 10^{-14}}{2.0 \times 10^{-7}} = 5.0 \times 10^{-8} \, M
\]

Thus, the concentration of \( OH^- \) is \( 5.0 \times 10^{-8} \, M \).

Would you like more details or have any further questions?

Here are 5 related questions:
1. What is the relationship between pH and \( [H_3O^+] \)?
2. How does temperature affect the value of \( K_w \)?
3. Can you derive the formula for pH given \( [H_3O^+] \)?
4. What happens to \( [OH^-] \) if the \( [H_3O^+] \) increases?
5. How would this calculation change at a different temperature?

**Tip:** Remember that at 25°C, the product of \( [H_3O^+] \) and \( [OH^-] \) is always \( 1.0 \times 10^{-14} \).

An aqueous solution at 25°C has a H₃O⁺ concentration of 2 × 10⁻⁷ M. Calculate the OH⁻ concentration. Be sure your answer has the correct number of significant digits.

Learn how to calculate the OH⁻ concentration given the H₃O⁺ concentration of 2 × 10⁻⁷ M at 25°C. This chemistry problem covers key concepts such as the ionization constant of water (Kw) and proper use of significant digits. Suitable for students in Grades 9-12.

Math Problem Statement

Solution

Ask a new question for Free

By Image

Math Problem Analysis

Mathematical Concepts

Formulas

Theorems

Suitable Grade Level

Related Recommendation