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strong and weak acids

Posted: Tue Feb 12, 2019 9:26 pm
by Cynthia Ulloa
Can someone explain why solutions of weak acids have a higher pH?

Re: strong and weak acids

Posted: Tue Feb 12, 2019 9:58 pm
by Becky Belisle 1A
Solutions of strong acids have a higher pH than solutions of weak acids of the same the molarity. For weak acids: the weaker the acid, the greater the pKa.

Re: strong and weak acids

Posted: Tue Feb 12, 2019 10:00 pm
by Irene Zhou 1E
Solutions of weak acids have a higher pH value than solutions of strong acids because it has a lower concentration of hydronium ions, so it is less acidic.

Re: strong and weak acids

Posted: Thu Mar 07, 2019 12:16 am
by Alysa Rallistan 2G
Weak acids tend to have higher pH because they do not tend to fully dissociate into hydronium ions and their respective anions. When you calculate the pH of a solution, you take the -log of the concentration of Hydronium ions, for weak acids this concentration will be relatively low compared to strong bases, so when taking this calculation the smaller the number in the -log the higher the overall value (and thus pH) becomes

Re: strong and weak acids

Posted: Fri Mar 15, 2019 1:26 pm
by Shibhon_Shepard
the more H3O+ ions there are the stronger the acid, so lower H3O+ ions means higher pH. (It's completely based on the H3O+ ions)

Re: strong and weak acids

Posted: Fri Mar 15, 2019 3:01 pm
by Catly Do 2E
A weak acid has less % dissociation (less of the acid, or the [HA] is breaking down), so that means when you take the pH, the value will be higher.