Acids and bases can be classified as either strong or weak electrolytes based on their strengths.
Concept #1: Strong acids are strong electrolytes that completely ionize while weak acids are weak electrolytes that partially ionize.
Concept #2: When looking at the strength of binary acids we look at the electronegativity of the nonmetal or the atomic size of the nonmetal.
Example #1: Which is the weakest acid from the following?
a) H2S b) HF c) H2Te d) All would have the same acid strength.
Example #2: Which of the following acids would be classified as the strongest?
a) CH4 b) NH3 c) H2O d) HF e) PH3
Concept #3: The strength of oxyacids is based on the number of oxygens or the electronegativity of the nonmetal excluding oxygen.
Concept #4: When comparing the strengths of oxyacids we can rely on two important rules.
Concept #5: Oxalic acid, iodic acid and amphoteric species are the exceptions in determining the strength of oxyacids.
Example #3: Rank the following oxyacids in terms of increasing acidity.
a) HNO3 b) HC7H5O2 c) H2CO3 d) HClO3