Week 8&9 - Buffers and Titration Curves_POSTED
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23 Terms
Titration
A technique used to determine the concentration of an acid or base by reacting it with a solution of known concentration.
Strong Acid + Strong Base
The reaction between a strong acid and a strong base produces water and a neutral solution.
Weak Acid + Strong Base
The reaction between a weak acid and a strong base produces a weak base and water.
Indicators
Organic dyes used to show the endpoint of a titration by changing color.
Equivalence Point
The point in a titration where equivalent amounts of acid and base have reacted.
Endpoint
The point at which the indicator changes color during a titration.
pKa
The negative logarithm of the acid dissociation constant (Ka); a measure of acid strength.
Strong Acid
An acid that completely dissociates in solution.
Weak Acid
An acid that partially dissociates in solution.
Buffer Solution
A solution that resists changes in pH when small amounts of acid or base are added.
Stoichiometric Point
Another name for the equivalence point in a titration.
Methyl Orange
An acid-base indicator that changes color from red to yellow at a pH of 3.1 to 4.4.
Phenolphthalein
An indicator that changes from colorless to pink as pH increases from about 8.2 to 10.
Bromothymol Blue
An indicator that changes from yellow to blue at a pH of 6.0 to 7.6.
Titration Curve
A graph showing the change in pH of a solution as a titrant is added.
HIn
The form of a weak acid used in indicator reactions.
In–
The conjugate base form of an indicator.
pH at Equivalence Point
The pH value at which the reaction of an acid and base is complete.
Hydronium Ion (H3O+)
The ion that represents the acidity of a solution.
Hydroxide Ion (OH–)
The ion that represents the basicity of a solution.
Ka
The acid dissociation constant, a measure of the strength of an acid in solution.
Kw
The ion product constant of water, equal to 1.0 x 10^-14 at 25°C.
DISSOCIATE
To break apart into ions when in solution; refers to how acids and bases behave in water.