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Michael Du 1E
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Joined: Sun Sep 22, 2019 12:16 am


Postby Michael Du 1E » Wed Dec 04, 2019 8:31 pm

In the lecture, Professor Lavelle mentioned that Cl- in NH4+Cl- does not affect the ph and therefore we leave it out. Can someone explain how and why the Cl- does not affect the pH?

Prasanna Padmanabham 4I
Posts: 111
Joined: Thu Jul 25, 2019 12:17 am

Re: Lecture

Postby Prasanna Padmanabham 4I » Wed Dec 04, 2019 8:39 pm

Cl- does not affect the pH of a solution because Cl- is a really stable atom; it does not need to bind to a Hydrogen. While NH3- is a weak base so it's conjugate acid, NH4 will lose a few Hydrogens in the NH4 and act as an acid by donating its extra Hydrogen.

Sanjana Borle 2K
Posts: 111
Joined: Fri Aug 09, 2019 12:15 am

Re: Lecture

Postby Sanjana Borle 2K » Wed Dec 04, 2019 8:47 pm

Since Cl- has a octet, it will not have an affinity to other ions or water so it won't affect the pH

Junwei Sun 4I
Posts: 125
Joined: Wed Oct 02, 2019 12:16 am

Re: Lecture

Postby Junwei Sun 4I » Thu Dec 05, 2019 5:09 pm

Cl- ion does not affect pH of water because it is a stable ion. It will not tend to bind to hydrogen atoms in water because itself is already stable. Therefore it will not cause any change in pH. And typically group one and group two cations metals are neutral.

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