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By the end of this section, you will be able to:
Identify acids, bases, and conjugate acid-base pairs according to the Brønsted-Lowry definition
Write equations for acid and base ionization reactions
Use the ion-product constant for water to calculate hydronium and hydroxide ion concentrations
Describe the acid-base behavior of amphiprotic substances
By the end of this section, you will be able to:
Explain the characterization of aqueous solutions as acidic, basic, or neutral
Express hydronium and hydroxide ion concentrations on the pH and pOH scales
Perform calculations relating pH and pOH
By the end of this section, you will be able to:
Assess the relative strengths of acids and bases according to their ionization constants
Rationalize trends in acid–base strength in relation to molecular structure
Carry out equilibrium calculations for weak acid–base systems
By the end of this section, you will be able to:
Predict whether a salt solution will be acidic, basic, or neutral
Calculate the concentrations of the various species in a salt solution
Describe the acid ionization of hydrated metal ions
By the end of this section, you will be able to:
Extend previously introduced equilibrium concepts to acids and bases that may donate or accept more than one proton
By the end of this section, you will be able to:
Describe the composition and function of acid–base buffers
Calculate the pH of a buffer before and after the addition of added acid or base
By the end of this section, you will be able to:
Interpret titration curves for strong and weak acid-base systems
Compute sample pH at important stages of a titration
Explain the function of acid-base indicators
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