Study Guide for Acid-Base Chemistry, Buffers, Titrations, and Ksp

These flashcards cover key concepts of acid-base chemistry, including definitions, equations, and examples that will help in reviewing for exams.

In a Brønsted-Lowry acid-base reaction, the H+ is transferred from the to the .

acid; base

The six strong acids to memorize are __, __, __, __, __, and __.

HCl; HBr; HI; HNO3; HClO4; H2SO4

Examples of weak acids include __, __, __, __, __, and __.

HOCl; HClO2; HF; H2CO3; H3PO4; HC2H3O2

A weak acid (HA) undergoes dissociation as follows: HA ⇄ __ + __.

H+; A–

The equation for the percent ionization of an acid is: percent ionization = (equilibrium [H+]/initial [HA]) x __% .

100

The Henderson-Hasselbalch equation is given as pH = __ + log([A-]/[HA]).

pKa

The Ksp expression for BaSO4(s) is __ = [Ba2+][SO42-].

Ksp

If Q < Ksp, then a __ will not form.

precipitate

The auto-ionization of water can be represented by the equation __.

2 H2O(l) ⇄ H3O+(aq) + OH–(aq)

Within a group, acid strength can be predicted based on __ energies.

bond

The common ion effect describes how the solubility of a slightly soluble salt is __ by the presence of a second solute that contains a common ion.

decreased

When comparing two different acids, the acid that has the greater value for Ka is the __ acid.

stronger

When a weak acid is diluted, the percent ionization will __ .

increase