titration formal lab reportimages.pcmac.org/sisfiles/schools/sc/georgetown/waccamawhigh/...titration...

Titration Formal Lab Report

Solution #1 Titrant

Solution #2 Analyte

In titration, one solution (solution #1) is added to another solution (solution #2) until a chemical reaction between the components in the solutions has run to completion. Solution #1 is called the titrant, and we say that it is used to titrate solution #2. The completion of reaction is usually shown by a change of color caused by a substance called an indicator.

A titration is a technique where a solution of known concentration is used to determine the concentration of an unknown solution. Typically, the titrant (the known solution) is added from a burette to a known quantity of the analyte (the unknown solution) until the reaction is complete. Knowing the volume of titrant added, allows the determination of the concentration of the unknown. Often, an indicator is used to usually signal the end of the reaction, the endpoint.

A successful tiration always begins with a priming of the glassware.


Reading the Burette

A burette is a piece of volumetric glassware used to deliver variable liquid amounts.

The burette is etched with calibration markings at 0.10mL intervals allowing the estimation of variable liquid levels to the hundredths of a milliliter (0.00 mL).

The numbering of the markings begins at the top of the burette. Therefore, the volume delivered can be determined from the difference between initial and final liquid levels.


Be careful when using pH probe! • Do not bang it against the side of the glassware and make sure to rinse in between use with distilled water. • pH probe measures to two decimal places.

Rules for significant figures for determining concentration when using pH:

The number of decimal places in pH dicatates the number of significant figures in concentration.

Example: pH reading of 5.46 would mean a concentration reading of 3.5 x 106 M not 3.47 x 106 M.

Do not look at the tens place.... only the number of decimal places determines the significant figures in the concentration.


30 mL of 0.10M NaOH neutralised 25.0mL of hydrochloric acid. Determine the concentration of the acid.

Write the balanced chemical equation for the reaction

NaOH(aq) + HCl(aq) > NaCl(aq) + H2O(l)

Extract the relevant information from the question:

NaOH V = 30mL , M = 0.10M HCl V = 25.0mL, M = ?

What formula can we use to solve for this?

Mtitrant Vtitrant = M analyte Vanalyte

Can we solve for the pH?

Determining Concentration of Unknown, the Analyte

titration formal lab reportimages.pcmac.org/sisfiles/schools/sc/georgetown/waccamawhigh/...titration...

Documents