Notes

Titration:
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 know solution) is added from a burette to a known quantity of the analyte (the unknown solution) until the reaction is complete.

REFERENCES
http://www.google.co.uk/search?q=what+is+titration&oq=what+is+titration&aqs=chrome..69i57j0l5.8380j0j8&sourceid=chrome&es_sm=122&ie=UTF-8&gws_rd=ssl&safe=active&surl=1#safe=active&q=what+is+titration
http://www.bbc.co.uk/schools/gcsebitesize/science/add_ocr_pre_2011/chemical_synthesis/calculationsrev3.shtml
http://chemwiki.ucdavis.edu/Analytical_Chemistry/Quantitative_Analysis/Titration

The apparatus needed includes a:
• pipette to accurately measure a certain volume of acid or alkali
• pipette filler to use the pipette safely
• conical flask to contain the liquid from the pipette
• burette to add small, measured volumes of one reactant to the other reactant in the conical flask
• wash bottle contains distilled water

CONCLUSION
How accurate was your standard solution?
What errors were there in your experiment you must identify at least two procedural errors?
Errors:
- Drops getting stuck to the side of the beaker, thus decreasing the number of moles that reach the solution, increasing molarity
- A small amount of HCl in it because last lab or as it wasn’t washed thoroughly. This would mean that the molarity is much smaller, because there are other impurities in the same amount of solution. This results in a too low calculated molarity.
Comment on how you would attempt to reduce these procedural and measurement error?
- When you see drops at the side of the beaker you could tap the beaker gently to release the drops.
- To avoid excess HCl you could clean the beaker thoroughly to make sure its cleaned before use to not mess up your calculation

An Alternative to the Standard Acid-Base Titration
Thermometric titration:
You will use thermometric titration to determine the concentration of hydrochloric acid
METHOD:
A) Stand an insulated cup in a beaker for support.

B) Using a pipette and safety filler, transfer 20 cm3 (or 25 cm3 ) of the sodium hydroxide solution into the cup, and measure the steady temperature

C) Using the burette, add a small portion (3 – 5 cm3) of dilute hydrochloric acid to the solution in the cup, noting down the actual volume reading. Stir by swirling the cup and measure the highest temperature reached.

D) Immediately add a second small portion of the dilute hydrochloric acid, stir, and again measure the highest temperature and note down the volume reading.

E) Continue in this way until there are enough readings to decide the maximum temperature reached during this experiment. You will need to add at least 30 cm3 of the acid.

Advantages:
- proven method
- rapid results
- easy to carry out