Buffers made from a weak acid and a strong base
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- เผยแพร่เมื่อ 5 ก.พ. 2025
- Chemistry cookery! Learn how you can make an acidic buffer by taking an excess amount of a weak acid and add a small amount of a strong base. Find out more by watching this vital video.
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Could you please explain to me the action of this buffer when you add OH- ions? Does the OH- ions react with H+ or CH3COOH? Or it doesn't matter either way?
@Rose87 OH- ion reacts with H+ to make H2O. Since some H+ s used up to make H2O, the buffer tries to compensate by pushing the reaction equilibrium more towards the right side, turning CH3COOH acid into its conjugate base and H+ (in order to make up for the loss of H+ when OH- was added to the solution)
Just a question! I don't know if this was a misconception I had but anyways I thought that if an acid and a base reacted together then they would react in such a way that no excess of either the acid or base would be left over irrespective of the fact that the reaction was with a weak acid and strong base or strong acid and weak base. Does it still count as neutralization if you have an excess left of either the acid/base (depending on what's in the beaker)? Sorry if this sounds weird but I was genuinely confused. Other than that thanks for all these videos, they're great!!
+Mel tansz Yes, if you have more H+ ions than OH- ions then you will have an excess of acid. A neutralisation reactions has till taken place though as a salt has been formed. You effectively need less moles of a strong base to neutralise a weak acid than if it was a strong acid of the same moles. This is because a weak acid dissociates weakly and less H+ ions are produced. Hope this helps!
When you say at 5:50 amounts are equal, is this in concentration or moles
moles