Solve for the OH- of a 0.05 M HCI solution 

To solve for the hydroxide ion concentration \([OH^-]\) in a 0.05 M HCl solution, follow these steps:

### Step 1: Determine the concentration of \(H^+\) (or \(H_3O^+\)) in the solution.
Since HCl is a strong acid, it dissociates completely in water:
\[
\text{HCl} \rightarrow H^+ + Cl^-
\]
So, the concentration of \(H^+\) in the solution is equal to the concentration of HCl, which is 0.05 M.

### Step 2: Use the ion product of water \((K_w)\) to find \([OH^-]\).
The ion product of water at 25°C is:
\[
K_w = [H^+][OH^-] = 1 \times 10^{-14}
\]
Substitute \([H^+] = 0.05 \text{ M}\) into the equation:
\[
[OH^-] = \frac{K_w}{[H^+]} = \frac{1 \times 10^{-14}}{0.05}
\]

### Step 3: Calculate the \([OH^-]\) concentration.
\[
[OH^-] = \frac{1 \times 10^{-14}}{0.05} = 2 \times 10^{-13} \text{ M}
\]

### Final Answer:
The hydroxide ion concentration \([OH^-]\) in a 0.05 M HCl solution is \(2 \times 10^{-13}\) M.

Would you like more details on any of these steps, or have any further questions?

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Here are five related questions:

1. How would you calculate the pH of the 0.05 M HCl solution?
2. What would be the pOH of this solution?
3. How does the concentration of \(OH^-\) change with increasing HCl concentration?
4. What is the relationship between pH and pOH in any aqueous solution?
5. How would the \([OH^-]\) concentration change if the temperature were increased?

**Tip:** Remember that for strong acids, the concentration of \(H^+\) is the same as the concentration of the acid because they dissociate completely in solution.

Solve for the OH- of a 0.05 M HCI solution.

Learn how to calculate the hydroxide ion concentration ([OH-]) in a 0.05 M HCl solution. This problem involves key concepts in acid-base chemistry, including the use of the ion product of water (Kw) formula. Suitable for students in Grades 10-12.

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