Recall that acids react with reactive metals to release hydrogen. Deduce equations for reactions of reactive metals with dilute HCl and H2SO4.
Deduce equations for the reactions with water of the oxides of group 1 and group 2 metals, carbon, and sulfur. Recall the formation of acid rain by gaseous non-metal oxides, and the acidification of oceans by increasing CO2levels.
Define a Brnsted-Lowry acid as a proton donor and a Brnsted-Lowry base as a proton acceptor. Deduce the Brnsted-Lowry acid and base in a reaction. Distinguish between the terms base and alkali.
Define a pair of species differing by a single proton as a conjugate acid-base pair. Deduce the formula of the conjugate acid or base of any Brnsted-Lowry base or acid.
Understand that some species can act as both Brnsted-Lowry acids and bases. Interpret and formulate equations to show acid-base reactions of these species.
Define the pH scale as pH = -log[H+] and [H+] = 10-pH. Perform calculations involving the logarithmic relationship between pH and [H+]. Estimate the pH using a universal indicator, and precisely measure pH using a pH meter/probe.
Explain how strong and weak acids and bases differ in the extent of ionization. Recognize that acid-base equilibria lie in the direction of the weaker conjugate. Recall that HCl, HBr, HNO3, and H2SO4are strong acids, and group 1 hydroxides are strong bases. Distinguish between strong and weak acids or bases and concentrated and dilute reagents.
Recall that acids react with bases in neutralization reactions. Formulate equations for the reactions between acids and metal oxides, metal hydroxides, hydrogen carbonates, and carbonates. Identify the parent acid and base of different salts.
Recognize, sketch, and interpret pH curves of neutralization reactions involving strong acids and bases. Identify appropriate intercepts with the pH axis and equivalence point.