Titration Flowchart

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Methyl orange pH indicator

Has a pH range between 3.1 and 4.4, which is where the pH of the titration would be in

Known volume Ammonia base

Clean all glassware

To completely get rid of residue that could affect pH analysis

Rinsing with tap water

Rinse again with deionized water

Titrant

Volume of concentrated HCL solution needed to make up given volume of the dilute HCL solution stoichiometrically

Pour small amount of HCL into both glassware to rinse them

Some deionized water into graduated cylinder

Have to add water first to prevent splashing

Volume of needed concentrated solution with cylinder

Volumetric flask using the decanting method

Waste beaker

Need to know the molar concentration of diluted solution for further stoichiometric work

Primary Standard

Deionized water

It reaches fill line

Measure and record mass of Borax

3x with deionized water

250 mL beaker

Mix solute until all Borax solute is dissolved

Solution into volumetric flask by decanting

Beaker with deionized water

All solution is transferred

Funnel on top of beaker

Place glass rod on top of beaker

Pour solution into flask carefully

Diluted HCL solution reaches meniscus of fill line

Begin standardization

n=m/mm, c=n/v

It helps determine a more accurate concentration of the titrant for calculations

Needed molar concentration of titrant is determined

Standardized HCL into burette

Begin Titration

Erlenmeyer Flask

Until solution changes colour completely

Equivalence Point

Concentration of ammonia

C1V1=C2V2

1:1 molar ratio, ICE box, Kb/Ka

Moles of titrant equal moles of analyte, right before endpoint

Solution has reached end point due to a pH change, moles of titrant exceed moles of analyte

Borax solution in volumetric flask reaches meniscus of fill line

Need to have a reference molar mass for titration

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