Summary
Highlights
The video starts by introducing the general rules for naming acids. If an acid contains a polyatomic ion ending in 'ate', it's replaced with 'ic'. If it ends in 'ite', it's replaced with 'ous'. For monoatomic ions ending in 'ide', the prefix 'hydro' and suffix 'ic' are added.
The first example, H2SO4, contains the sulfate ion. Since 'ate' becomes 'ic', the acid is named Sulfuric Acid.
For H2SO3, which contains the sulfite ion, the 'ite' is changed to 'ous', resulting in Sulfurous Acid.
The example H2S, containing the sulfide ion, follows the rule for monoatomic ions. It becomes Hydrosulfuric Acid by adding 'hydro' and 'ic'.
Additional examples are provided, demonstrating the naming of perchloric acid (from perchlorate), hypochlorous acid (from hypochlorite), and hydrochloric acid (from chloride).
The video further illustrates the naming convention with nitric acid (from nitrate) and nitrous acid (from nitrite).
Examples of hydroiodic acid (from iodide) and acetic acid (from acetate) are presented, reinforcing the previously discussed rules.
The video then shifts to working backward from the acid name to its formula, starting with Phosphoric Acid. By identifying the 'ic' suffix, it's linked to the phosphate ion (PO4^3-), and three hydrogens are added to neutralize the charge, resulting in H3PO4.
Further examples of deriving formulas include Phosphorous Acid (from phosphite, H3PO3) and Carbonic Acid (from carbonate, H2CO3).
The final examples demonstrate deriving formulas for hydrobromic acid (from bromide, HBr) and hydrocyanic acid (from cyanide, HCN), highlighting an exception where cyanide is a polyatomic ion but still follows the 'hydro-ic' naming convention.