To see where the equivalent point is
Answer this question... dnt know
iv done the titration and the preferred indicator for such a solution is phenalphaline, use a few drops to make it go a bright luminous pink and titrate till clear, not 'cloudy'
A few drops of any indicator is generally enough to get a reading.
6.3x10-9
Because that is all you need; any more and it can make it harder to see some of the changes, as the substance shall end up too dark. Plus it'll just be a waste of indicator. That's what my science teacher's taught me in the past.
Answer this question... dnt know
iv done the titration and the preferred indicator for such a solution is phenalphaline, use a few drops to make it go a bright luminous pink and titrate till clear, not 'cloudy'
A few drops of any indicator is generally enough to get a reading.
The Starch-Iodide complex is not very soluble in water, so the starch is added near the endpoint of an Iodine titration, when the Iodine concentration is low. This eliminates errors due to the fact that some Iodine may remain adsorbed on the complex and go undetected. so if you add the starch indicator only right near the end point when the solution is a light yellow colour the starch shouldn't complex and go lumpy.
Its Ph value is less than 7, so it is acidic. The exact colour change needs to be compared visually with a standard universal indicator chart to determine the precise Ph value associated with that particular shade of red.
It drops during hibernation
use the pH scale by adding 1 or 2 drops of universal indicator in an acid or an alkali
bill
6.3x10-9
It is a substance used to determine the strengths of acids and alkali.It changes color according to the pH of the material its in. It is so useful because the color also tells you how strong the substance is. As an example, if you were to put a few drops of the indicator in water it would go green. A few drops of it in cleaning products and it would go a deep purple.A universal indicator can give various colors to a huge variety of pH ranges.
Firstly place 100 to 150 mg of aspirin into a 125 ml conical flask. Next proceed to mix in 15 ml of 95% ethanol solution and add 2 drops of phenolphthalein indicator. Then use the titration method to mix this solution against a standard solution of sodium hydroxide from a burette. Using the value obtained from the titration calculate the molarity of the aspirin. Then calculate the ratio of the observed molarity of aspirin with its theoretical molarity and finally multiply this ratio with 100 to obtain the percentage purity of the aspirin sample.
I believe you should wait until the service indicator drops to around 15%.