Cations as acids

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Cations as acids

Postby makenzie2K » Tue Jan 15, 2019 8:23 pm

How do we know when a cation will act as an acid in a reaction and predict their relative strength?

Miriam Sheetz 2B
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Joined: Fri Sep 28, 2018 12:25 am

Re: Cations as acids

Postby Miriam Sheetz 2B » Tue Jan 15, 2019 8:45 pm

Cations are always going to act as acids, but as far as strength, you have to memorize the strong acids: HCl, HNO3, H2SO4, HBr, HI, HClO4, HClO3 . If you know the strong acids, the others are weak acids.

Arianna Ko 2E
Posts: 33
Joined: Fri Sep 28, 2018 12:20 am

Re: Cations as acids

Postby Arianna Ko 2E » Wed Jan 16, 2019 11:23 am

Small highly charged metal cations can produce acidic solutions. These cations are basically those with a charge of 3+ for example. These small cations can exert the greatest pull on the electrons in surrounding H20 molecules, resulting in a greater number of hydrogen ions to be lost from the water molecules, producing a more acidic solution. The larger Group 1 and 2 cations are too large and have too low of a charge and thus does not have any effect on pulling electrons from the surrounding H20 molecules and will not cause the H20 molecules to release their H protons to form acidic solution.

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