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Ch.16 - Aqueous Equilibrium WorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch.17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
Intro to Buffers
Henderson-Hasselbalch Equation
Intro to Acid-Base Titration Curves
Strong Titrate-Strong Titrant Curves
Weak Titrate-Strong Titrant Curves
Acid-Base Indicators
Titrations: Weak Acid-Strong Base
Titrations: Weak Base-Strong Acid
Titrations: Strong Acid-Strong Base
Titrations: Diprotic & Polyprotic Buffers
Solubility Product Constant: Ksp
Ksp: Common Ion Effect
Precipitation: Ksp vs Q
Selective Precipitation
Complex Ions: Formation Constant

Acid-Base Indicator is a weak acid or base that helps determine the pH at the endpoint of a titration.

Concept #1: Acid-Base Indicator

Indicators have a pH range of pKa+/- 1.

Example #1: Pick the best indicator for the following titration

a) bromothymol blue pKa = 7.2

b) thymolphthalein pKa = 9.2

c) phenolphthalein pKa = 9.5

d) methyl red pKa = 5.1

e) bromophenol blue pKa = 4.1

Practice: Chemistry student is using an indicator with a pKa of 4.7 for the titration of a strong acid with strong base. Calculate the pH range at which the indicator will change colors.

a) 2.7–3.5                      b) 10–11                        c) 4.7–8.7                      d) 3.7–5.7                      e) 2.7–5.8

Practice: Bromophenol blue (pKa = 4.1) is a common acid-base indicator. It is yellow in its acidic form and blue in conjugate base form. If the solution being titrated has a pH = 4.0, what color would the bromophenol blue indicator possess?

a) yellow                       b) orange                      c) blue                          d) green                      e) purple