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

Solution: An indicator changes from red to blue going from its acidic (nonionized) form to its basic (ionized) form. The indicator has a Ka of 3.2 × 10−5 . What color would be visible in a solution with this in

Solution: An indicator changes from red to blue going from its acidic (nonionized) form to its basic (ionized) form. The indicator has a Ka of 3.2 × 10−5 . What color would be visible in a solution with this in

Problem

An indicator changes from red to blue going from its acidic (nonionized) form to its basic (ionized) form. The indicator has a Ka of 3.2 × 10−5 . What color would be visible in a solution with this indicator at pH 5.62?

1. red

2. purple

3. blueish-purple

4. reddish-purple

5. blue

 

Solution

We’re being asked to determine the color of an indicator at pH 5.62

The indicator changes from red to blue when going from its acidic (nonionized) form to its basic (ionized) form.


HA (acidic form)  A (basic form); Ka = 3.2 × 10–5


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