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Regents Chem - Acids/Bases/Salts

Acid proton donor. Has hydrogen (H+) or hydronium (H3O+) as the only positive ion in a solution
Base proton acceptor. Has hydroxide (OH-) as the only negative ion in solution.
Ternary acids Acid containing an ion from table E. It ends with "ic," or "ous."
Acids on the pH scale pH lower than 7. The lower you go, the stronger the acid. Each number is a 10x change in [H+]. Strong acids have [H+] is greater than [OH-]
Bases on the pH scale pH higher than 7. The higher you go, the stronger the base is. Strong bases have [OH-] is greater than [H+]
Compare a pH 4 to pH of 6 pH 4 is 100x more acidic or 100x less basic. PH 4 has 100x more [H+]
Amphiprotic (amphoteric). PH’s around neutral so this substance can act as acid or base, depending on what it’s combined with. PH’s around neutral so this substance can act as acid or base, depending on what it’s combined with.
Neutralization acid + base makes salt + water. pH approaches neutral.
Electrolysis of salts salt + water makes acid + base. If acid and base produced are both strong it will be neutral; If acid is stronger, pH will still be acidic. If base is stronger will be basic.
Indicators chemicals on table M that tell us the pH.
Binary acids Acid containing H+ and just one other element. Name starts with "hydro" and ends in "ic."
Buffer A chemical that resists changes in pH by neutralizing small amounts of added acid or base, keeping the pH of the solution relatively stable
Created by: etucci