Grade 12 Chem | pH + pOH = 14 | Inversely Related H3O+ and OH- Concentrations | Acidic-Basic-Neutral

Measure acid present using hydronium ion concentration
Measure acid present using [H3O+]
Measure base present using hydroxide ion concentration
Measure base present using [OH-]
In aqueous solution, the hydronium ion concentration and hydroxide ion concentration are inversely related
Equation that relates hydronium and hydroxide concentrations: [H3O+][OH-] = 1.0 E-14
Which solution is more acidic based on hydronium ion concentration
Which solution is more acidic based on [H3O+]
Which solution is more basic based on hydroxide ion concentration
Which solution is more basic based on [OH-]
pH scale
pH level
Concentrations should be in molarity
Molarity = mole of solute / Liter of solution
pH = - log [H3O+]
How to calculate hydronium ion concentration from pH
How to calculate [H3O+] from pH
Types of Aqueous Solution:
Neutral solution (pH = 7.0)
Acidic solution (pH is less than 7.0)
Basic solution (pH is greater than 7.0)
pOH
pOH = - log [OH-]
How to calculate hydroxide ion concentration from pOH
How to calculate [OH-] from pOH
pH + pOH = 14.0
pH and pOH are inversely related