Calculate the theoretical pH of 10 mM NaOH using the data below: • NaOH is a strong base, dissociates completely, thus [OH] is equal to [NaOH] • ion product of water [H+][OH-]=1.0 X 10-14 M2 • pH = -log [H+]

What is the pH of an aqueous solution with [H3O+] = 2×10−14 M? Express the pH numerically using one decimal place.

Calculate the pH, pOH, hydronium ion (+) or hydroxyl ion (-)of the solutions below.   pH= 7.5   pOH= 9.2   pH= 3.7   pOH = 13.9

A Determine the [H+], pH, and pOH of a solution with an [OH-] of 0.00011 M at 25 °C. [H*] = pH = pOH = Determine the [H+], [OH-], and pOH of a solution with a pH of 3.79 at 25 °C. [H+] = [OH-] = pOH = Determine the [H]. [OH-], and pH of a solution with a pOH of 4.43 at 25 °C. [H+] = [OH-] = pH = M M M M M

Calculate the [OH−] if the [H+] = 0.002128 M.

Calculate the pH of a solution  with [H+]  = 1.8 x 10-5 M

Which of the following statements is true?   a basic solution has an H3O+ concentration greater than 1.0 x 10-7 M and a pH value lower than 7.0.   a basic solution has an OH- concentration greater than 1.0 x 10-7 M and a pH value lower than 7.0.   a basic solution has an H3O+ concentration greater than 1.0 x 10-7 M and a pH value greater than 7.0.   a basic solution has an OH- concentration lower than 1.0 x 10-7 M and a pH value greater than 7.0.   a basic solution has an H3O+ concentration lower than 1.0 x 10-7 M and a pH value greater than 7.0.

Which of the following indicates the most basic solution? [OH ]= 7x 10 M РОН 3 6.7 pH = 4.2 [H*]=1 x 10¬10 M At least two of the solutions are equally basic

Determine the [OH-], pH, and pOH of a solution with a [H+] of 4.7 × 10-¹² M at 25 °C. [OH-] = pH: = POH Determine the [H+], pH, and pOH of a solution with an [OH-] of 6.7 x 10-7 M at 25 °C. [H+] = pH : = = POH = M M

Calculate the molarity for a solution with the following pH.   pH = 4.56 Formulas: pH = -log [H3O+] [H3O+] = 10-pH