Strong vs. Weak

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Sophie 1I
Posts: 51
Joined: Fri Sep 29, 2017 7:04 am

Strong vs. Weak

Postby Sophie 1I » Wed Dec 06, 2017 6:34 pm

How can you tell the difference between a strong and a weak acid and strong and weak base by looking at the reaction equation?

Ashley Chipoletti 1I
Posts: 20
Joined: Fri Sep 29, 2017 7:04 am

Re: Strong vs. Weak

Postby Ashley Chipoletti 1I » Wed Dec 06, 2017 6:43 pm

Usually, acids with elements on the far right side of the periodic table are strong acids because of their high electronegativity.

Sophie 1I
Posts: 51
Joined: Fri Sep 29, 2017 7:04 am

Re: Strong vs. Weak

Postby Sophie 1I » Wed Dec 06, 2017 7:38 pm

Okay thank you!

Erik Khong 2E
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Joined: Fri Sep 29, 2017 7:07 am

Re: Strong vs. Weak

Postby Erik Khong 2E » Thu Dec 07, 2017 9:50 pm

It also relates to the fact that the ions of elements on the right and lower side of the periodic table grow progressively larger and result in longer, weaker bonds with H. Hence, HF is a weaker acid than HCl and HI. The strength of acidity increases across with electronegativity but downwards with size.

Guangyu Li 2J
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Been upvoted: 1 time

Re: Strong vs. Weak

Postby Guangyu Li 2J » Sat Dec 09, 2017 3:51 am

From the equation, you can see how many hydrogen atoms are protonated.

Typically, all the hydrogen atoms in strong acid are protonated; on the other hand, a small fraction of hydrogen atoms in weak acid are protonated.

Hope this helps.

AnuPanneerselvam1H
Posts: 52
Joined: Fri Sep 29, 2017 7:07 am

Re: Strong vs. Weak

Postby AnuPanneerselvam1H » Sat Dec 09, 2017 8:45 pm

Strong acids will have more electronegative/electron withdrawing atoms in their formulas. This will allow the proton to break away more easily and for the resulting anion to be stable.


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