Each row of the table below describes an aqueous solution at about 25°C.Complete the table. That is, fill in any missing entries in the second and third columns. Round your entries for H3O+ to 2 significant digits, and your entries for pH to 2 decimal places.solution H3O+ pHA ×1.910−7mol/L B mol/L 0.42C ×5.210−10mol/L

The table you provided is not fully visible. However, I can explain how to fill in the missing entries based on the information given.

The concentration of H3O+ ions and pH are inversely related. The formula to calculate pH is:

pH = -log[H3O+]

Where:

• pH is the measure of acidity or alkalinity of a solution.
• [H3O+] is the concentration of hydronium ions in the solution.

Let's fill in the missing entries:

1. For solution A, the H3O+ concentration is given as 1.91 x 10^-7 mol/L. To find the pH, we use the formula:

   pH = -log(1.91 x 10^-7) = 6.72 (rounded to 2 decimal places)

2. For solution B, the pH is given as 0.42. To find the H3O+ concentration, we rearrange the formula to:

   [H3O+] = 10^-pH = 10^-0.42 = 0.38 mol/L (rounded to 2 significant digits)

3. For solution C, the H3O+ concentration is given as 5.21 x 10^-10 mol/L. To find the pH, we use the formula:

   pH = -log(5.21 x 10^-10) = 9.28 (rounded to 2 decimal places)

Please provide the complete table if you need more specific help.