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. Be sure each entry you write includes the correct number of significant digits. solution H3O+ pH A 0.0078mol/L   B mol/L 7.32 C ×4.910−12mol/L

Hydrochloric acid (24.9 mL of 0.195 M) is added to 466.0 mL of 0.0830 M Ba (OH), solution. What is the concentration of the excess H+ or OH ions left in this solution? Molarity = M Drag and drop your selection from the following list to complete the answer: OH H+

8 + An aqueous solution at 25 °C has a OH concentration of 1. × 10¯³M. Calculate the H₂O* concentration. Be sure your answer has the correct number of significant digits. M X Ś

An aqueous solution at 25 °C has a OH concentration of 2.3 x 10 -12 M. Calculate the H,0` concentration. Be sure your answer has 2 significant digits. M x10

Please submit answers with correct number of Significant figures

You are asked to dilute 10.0 mL of 12.0 M HCl with enough water to make a 1.09 solution. How much water is added for the dilution? Answer in mL to one decimal place.

Suppose a 0.036M aqueous solution of phosphoric acid (H3PO4) is prepared. Calculate the equilibirum molarity of HPO4^2- Round your answer to 2 significant figures.

Complete this table to show the pH and pOH of each solution. Solution A Solution B Solution C Solution D Solution A [OH-] = Solution B [H+] = Solution C [OH-] = Solution C pOH = 1.0 x 10-6 1.0 × 10-11 [OH-] 1.0 × 10-10 M pH M 6 9 Solution A pOH = M Solution B pH= Solution C pH = Solution D [H+] = POH 10 17 M

How many grams of calcium (Ca^2+) ion would be present in this solution  How many grams of sulfate (SO4^2-) ion would be present in this solution

To make 525mL of the 0.15M NaOH solution, how much water do you need to add to the 31.5mL of the 2.50M solution?