Acid/base titration.? - heaps of acid in stomach
hey guys,
In any proof of why it is important that the concentration of acids and bases to close enough?
Thank you heaps
Saturday, January 30, 2010
Heaps Of Acid In Stomach Acid/base Titration.?
4 comments:
The reason for this is useful for the effective implementation of the evaluation. It is common for 25 ml conical or unknown, and then determine the volume of solution required for neutralization. Consider whether the stranger was a solution of NaOH 1M. If you are using 0.1 M HCl as a solution, the acid 250 ml, which is very laborious and requires requires many parts of the burette, which would normally ml in 50th This leads to inaccuracies and disadvantages of working with very large quantities, and finally in the absorber.
Consider the opposite extreme. Will you evaluate NaOH 0.1 M, again in 25-ml Erlenmeyer flask. With 1.0 M HCl. This would be 2.5 ml HCl, a volume so low that the possibility that the inaccuracy is high.
It's much better to use solutions with similar concentrations, so that consumed in the titration volumes are used similarly to known and unknown.
Look at the Henderson-Hasselbalch equation:
pH = pK a + log [base] / [acid]
when the concentrations of acid and base are similar, then the ratio would be, eg, 1 the logarithm of 1 is zero. So if you find a buffer of pH 5, is an acid, the pKa of about 5 and the concentrations of acid and base on them.
In an acid / base should the valuation of securities in the two acid-base rather narrow, or it is dominated in pH to change the other.
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