The autoionization constant for water at 35 °C is 2.2 × 10−14. Use this information to answer the following questions. a)What is the [H3O+] and pH of neutral water at 35 °C? b)Determine if the following solutions are acidic, neutral, or basic at 35 °C. Explain your answer. i)[H3O+] = 9.8 × 10−6 M ii)pH = 6.95 iii)[OH−] = 5.1 × 10−7 M iv)pOH = 9.24

In an aqueous solution at 25 °C, if [H₃O⁺] = 7.2 × 10⁻⁴ M, then [OH⁻] is

The molar concentration of OH- in a water solution is 1.5 × 10−9 M. Determine the concentration of proton in M.

For each of the following strong base solutions, determine [OH−],[H3O+],pH, and pOH. Determine [OH−] and [H3O+] for a 1.7×10−3M Ca(OH)2 solution.

Calculate the pH of a solution with an H+ concentration of 3.25 x 10^-3 M.

Find the pH of the following solution and state whether the solution is acidic, basic or neutral. [OH-] = 5.8 x 10^-11

What is the pH of a 4.7 × 10⁻⁶ M KOH solution?

What is the pH of a solution in which [OH⁻] = 0.000005 M?

Determine the [H+] , [OH−] , and pH of a solution with a pOH of 8.95 at 25 °C.

Use the following information to complete the table. pOH + pH = 14.0 pH = -log[H+] pOH = -log[OH-]   Complete the table below.   [H+] [OH-] pH Acidic, Basic or Neutral 1) 1 X 10-9       2)     10.0   3)   4.9 X 10-11     4) 9.2 X 10-5       5)       Neutral 6)     4.561