Flashcards in Titration - SODIUM THIOSULFATE Deck (29):
Explain how iodine, a non-polar substance of very low water solubility is brought into aqueous solution
Reacts with iodide [potassium iodide]
The iodine solution was made up in a 500cm^3 volumetric flask. Describe the procedure for measuring 25.0cm^3 of this solution into a conical flask
Pour iodine solution into a clean,dry beaker
Use pipette which was rinsed with deionised water and solution to be contained
Fill using pipette filler until bottom of meniscus is on graduation mark and read at eye level
Tap pipette against wall of conical flask
Name a suitable indicator for this titration
At what stage is the indicator added
Colour in conical flask is pale yellow - indicates close to end point
State the colour change at the end point in the presence of the indicator
Blue/black -> colourless
Explain why the use of distilled water instead of deionised water throughout this experiment would be likely to ensure a more accurate result
Deionised - only has ions removed and could therefore contain non-ionic substances that could be oxidised/reduced
Describe how the crystalline thiosulfate was dissolved, and how the solution was transferred to the volumetric flask and made up to exactly 500cm^3
Add crystals to beaker and rise from clock glass into beaker. Stir and dissolve
Pour using funnel into volumetric flask and washings of beaker
Add deionised water until bottom of meniscus is at graduation mark at eye level
Stopper and invert several times
Pure iodine is almost completely insoluble in water. What must be added to bring iodine into aqueous solution?
Potassium iodide [source of iodide]
What sequence of colours was observed in the conical flask from the start of the titration until the end point was reached
Why is hydrated sodium thiosulfate not suitable as a primary standard?
It loses water of crystallisation readily
It is not stable
Why are iodine solutions made up using potassium iodide solution?
Iodine is fairly soluble in water, however it reacts with iodide to form I^3- ions which are very soluble
Why does starch solution have to be freshly prepared?
It detiorerates quickly on standing
Why is starch indicator added close to the end point?
To give a sharp end point, while avoiding the formation of excess starch complex which would be difficult to decompose
Describe the appearance of the sodium thiosulfate crystals
Colourless crystalline solid
Give one advantage of using a clock glass rather than paper when weighing out the sodium thiosulfate crystals
Clock glass is more suitable than paper since any sodium thiosulfate remaining on the clock glass can be washed off, this is not possible with paper
Why is it necessary to remove the funnel from the burette prior to carrying out the titration
Failure to remove the funnel may introduce an error into the readings as drops of liquid may fall from the funnel into the course of the titration. This causes the titration result to be inaccurate
Why is it advisable to use deionised water rather than tap water when making up solutions in this experiment
Tap water contains many dissolved ions which could interfere with the reactions taking place
Describe how you would take the reading in the pipette when using KMnO4?
The reading should be taken from the top of the mensicus
Why is it not possible to make up a solution of I2 directly? How is this overcome?
Iodine vaporises slightly at room temperature. In addition iodine does not dissolve in water
A standard solution of iodine is obtained by reacting a standard solution of acidified potassium permanganate with excess potassium iodide
What colour change is observed in the conical flask when the dilute sulfuric acid and potassium iodide solution are added to the KMnO4
Purple - reddish/brown colour
What colour change is observed at the end point of the titration
Blue/Black -> Colourless
Why is it not necessary to know precisely the exact number of KI added
The KI is present in excess in order to ensure that the amount of iodine formed during the titration depends only on the amount of potassium permanganate present. In addition, I-ions are necessary in order to keep in solution the I2 that is formed
How is a standard solution of iodine generated?
Reacting a standard solution of potassium permanganate with excess potassium iodide in conical flask
What is the apperance of the iodine solution?
How can a sodium thiosulfate solution be standardised?
Standard solution of iodine
How can an iodine solution be standardised?
Standard solution of sodium thiosulfate
What is found in the conical flask during the titration?
Potassium permanganate + dilute sulfuric acid + potassium iodide
What is in the burette and pipette
Burette - Sodium thiosulfate
Pipette - Iodine solution