The concentration of NaOH in a solution is 7.00 10-6 M.

What is the [H3O+] in the solution?
_______________M
What is the [OH-] in the solution?
__________M
What is the pH of the solution?

What is the pOH of the solution?

HELPP?? i don't understand any of this...

http://answers.yahoo.com/question/index?qid=20100514143449AAOciaj

No problem, I'm here to help you understand! Let's break down these questions step by step.

1. What is the [H3O+] in the solution?
To find the concentration of H3O+ ions in the solution, we need to use the concept of the pH scale, which measures the acidity or alkalinity of a solution. However, in this case, we are not given any information about the acidity or alkalinity of the solution. Therefore, we cannot directly calculate the concentration of H3O+ ions from the given information.

2. What is the [OH-] in the solution?
To determine the concentration of OH- ions in the solution, we need to use the concept of Kw, which is the ion product constant of water and is equal to 1.0 x 10^(-14) at 25°C.

The formula for Kw is:
Kw = [H3O+][OH-]

Since the concentration of OH- ions is not given, we can use Kw and the concentration of NaOH to calculate it. Since NaOH is a strong base, it fully dissociates in water to give OH- ions.

In this case, the concentration of NaOH is given as 7.00 x 10^(-6) M. Therefore, the concentration of OH- ions is also 7.00 x 10^(-6) M.

3. What is the pH of the solution?
The pH of a solution is a measure of its acidity. It is calculated using the formula:

pH = -log[H3O+]

Since we don't have the concentration of H3O+ ions, we cannot directly calculate the pH of the solution.

4. What is the pOH of the solution?
The pOH of a solution is a measure of its alkalinity. It is calculated using the formula:

pOH = -log[OH-]

Since we know the concentration of OH- ions (7.00 x 10^(-6) M), we can calculate the pOH using this formula.

Now you have the steps to calculate the pOH of the solution. Let me know if you would like more help or have any other questions!