Chapter 16+ Key Terms Flashcards
Acid Base Titration
When a solution of unknown concentration is reacted with a solution of known concentration to determine original concentration
Buffer Capacity
The amount of acid or base that cam be added to a buffer without becoming ineffective
Buffer
Solution with both weak acid and conjugate base that resists pH change by neutralizing added acid or base
Common ion effect
Tendency for a common ion to decrease solubility of a weaker acid or base
Complex ion
Ion containing a central metal with one+ ligands
Endpoint
Point of pH change where an indicator changes color
Equivalence point
Point in a titration at which added solute has completely reacted
Formation Constant (Kf)
Equilibrium constant of reactions that form complex ions
Henderson-Hasselbalch Equation
Equation to find pH of a buffer using “x is small”
pH=pKa+log(base/acid)
Indicator
a dye whose color depends on the pH of the solution it is dissolved in
Ligand
a neutral molecule or an ion that acts as a Lewis base within a complex ion
Molar Solubility
Solubility of a compound in moles/liter
Qualitative Analysis
A systematic way to determine the ions present in an unknown solution
Selective Precipitation
A process involving adding a reagent to a solution that precipitates out only one ion
Solubility Product Constant (Ksp)
Equilibrium expression for an equation representing the dissolution of something moderately soluble
