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What is the key difference between Arrhenius and Brønsted-Lowry acids?
Arrhenius acids increase H+ in water; Brønsted-Lowry acids are proton donors (not limited to water).
How does the strength of an acid relate to the strength of its conjugate base?
Stronger acids have weaker conjugate bases; weaker acids have stronger conjugate bases.
What is the effect of adding an Arrhenius acid to water?
The concentration of H+ ions increases.
What is the effect of adding a Brønsted-Lowry base to a solution?
It accepts a proton (H+) from an acid.
What happens to the pH of a solution as the concentration of H3O+ increases?
The pH decreases.
What happens to the pOH of a solution as the concentration of OH- increases?
The pOH decreases.
What happens to the pH at half equivalence point?
pH = pKa
Define Arrhenius acid.
A substance that increases the concentration of H+ ions in solution.
Define Arrhenius base.
A substance that increases the concentration of OH- ions in solution.
Define Brønsted-Lowry acid.
A proton (H+) donor.
Define Brønsted-Lowry base.
A proton (H+) acceptor.
Define conjugate acid.
The species formed when a base gains a proton (H+).
Define conjugate base.
The species formed when an acid loses a proton (H+).