The H⁺ concentration in an aqueous solution at 25 °C is 4.5 × 10⁻⁴. What is [OH⁻]?

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

What is the percentage of HCl in the solution if the molarity is 0.268398000?  Assume the density of the solution is 1.00 g/mL.

A solution in which [H+] is 1000 times greater than [OH-]. Express the molarity to two significant digits.

Calculate the hydronium concentration of a 5.59x10–5 M HCl solution. Enter your answer as x.x*10^# (where x represents digits of the number and # represents the exponent and its sign)

Complete the table

If it takes 50.00 mL of 0.500 M KOH solution to completely neutralize 125 mL of sulfuric acid solution (H2SO4), what is the concentration of the H2SO4 solution?

An aqueous solution at 25 °C has a OH concentration of 1.2 × 10 M x10 × 8 3 M. Calculate the H3O+ concentration. Be sure your answer has 2 significant digits.