Please enable JavaScript.
Coggle requires JavaScript to display documents.
Chapter 4.5-4.6 - Coggle Diagram
Chapter 4.5-4.6
4.6 - Solution Stoichiometry
and Titrations
Stoichiometric Conversion Chart
Grams of A <- Molar Mass -> Moles of A <- M = mol/L -> Volume or molarity of A
/\
|⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀
Mole Ratio⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀
|⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀
\/⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀⠀
Grams of B <- Molar Mass -> Moles of B <- M = mol/L -> Volume or molarity of B
Titrations
An analytical technique during which a reagent solution of known concentration is used to determine a solution of unknown concentration
Acid Base Titrations
A pH indicator is used to determine whether nutrialization has been reached and titration is complete
Equivalence point - At which the amount of titrant added is just enough to completely neutralize the analyte solution
Titrant is added to a buret, along with a few drops of indicator. A precise amount of analyte is pipetted into an erlenmeyer flask. Titrant is added dropwise while continually stirring until the equivalence point is reached.
Titrant - Known solution
Analyte - Unknown solution
4.5 - Solution Calculations
Using Concentration
Concentration
Solute
Lesser quantity of solution
Solvent
Greater quantity of solution
Molarity (M)
Molarity = Moles of solute/Liters of solution
Concentration of Ions
1.0M solution of H2SO4
2.0M of H+ Ions
1.0M of SO4 2+ Ions
Dilutions
Taking stock solution and adding more solvent (typically water)
M1
*
V1 = M2
*
V2