15.2 Auto ionization of Water

H₃O⁺ → H⁺ relates to _______ (Acids, bases)

Acids

OH^- relates to _______ (acids, bases).

Bases

H₃O⁺ and H₂O are a ______________.

Conjugate acid-base pair

H₂O and OH^- are a __________________

Conjugate acid base pair

T/F: both H3O+ and OH- exist in water.

True

Equilibrium constant for the auto ionization of water is denoted as Kw which equals ________?

1.0 E-14

What is the concentration of H3O+ in pure water at 25 degrees C

1.0 E-7

The same applies for hydroxide

1. Calculating hydronium and hydroxide concentrations

   Calculate the concentration (M) of hydronium in a solution that contains 0.054 M hydroxide.

1.85E-13

T/F: the end product of [H3O+] and [OH-] is equal to Keq

F: it is always equal to Kw = 1.0E-14

Calculate the [OH-] in a solution with a [H3O+] of 3.6E-3.

[OH-] = 2.8E-12

Calculate the hydrogen ion concentration [H3O+] of a solution in which [OH-] = 0.025M

Is this solution acidic, basic or neutral?

4E-13 M

In pure water [H3O+] = [OH-] = 1.0E-7

= basic?

pH = -log[H₃O]

Calculate the pH of a solution that has a 0.0034 M [H3O].

2.47

Calculating [H₃O⁺] form pH

Calculate the hydrogen ion concentration [H₃O⁺], in a solution having a pH of 3.52

[H3O+] = 3.0E-4

2. The pH scale

   Fill in the blanks below with a preceding bolded term.

   A solution with more hydronium than hydroxide is considered (acidic, basic) ________.

   A solution with more hydroxide than hydronium is considered (acidic, basic) ________.

   Like hydronium and hydroxide concentrations, pH can also be used to describe the acidity or basicity of a solution.

   A solution with a pH below 7 is considered (acidic, basic) _______.

   A solution with a pH above 7 is considered (acidic, basic) _______.

Acidic

Basic

Acidic

Basis