KBr

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Meachelle_Lum_1I
Posts: 92
Joined: Fri Sep 28, 2018 12:24 am

KBr

Postby Meachelle_Lum_1I » Mon Dec 03, 2018 11:21 pm

Why is KBr neutral when dissolved in water, but KF is not?
For 6th edition 12.65, how can we tell by looking at the salt, if it will release H+ or OH- in water?
salts:
AlCl3
Cu(NO3)2

Andre_Galenchik_2L
Posts: 69
Joined: Fri Sep 28, 2018 12:23 am

Re: KBr

Postby Andre_Galenchik_2L » Tue Dec 04, 2018 11:20 am

It may be because bromine is a bigger element than fluorine.

harshitasarambale4I
Posts: 58
Joined: Fri Sep 28, 2018 12:26 am

Re: KBr

Postby harshitasarambale4I » Tue Dec 04, 2018 11:35 am

Since bromine is bigger than fluorine, the bond length is going to be longer and weaker. This means it will be a stronger acid.

Parth Mungra
Posts: 72
Joined: Fri Sep 28, 2018 12:28 am

Re: KBr

Postby Parth Mungra » Tue Dec 04, 2018 11:42 am

The above answers are correct; bromine is bigger, therefore forming a smaller, weaker bond, allowing the bond to be broken easier.
For the salt part of your question: If you have NH4+, for example, this will give a proton (an H+) because then it can form to a NH3. This extra proton will then form a hydronium ion when it is dissolved in water

dgerges 4H
Posts: 65
Joined: Fri Sep 28, 2018 12:24 am

Re: KBr

Postby dgerges 4H » Tue Dec 04, 2018 11:47 am

"KBr dissociates into K+ and Br-. Br- reacts to make HBr, a strong acid. Since Br- is the conjugate base of HBr, it is weak. K+ is also weak so the two weak components sort of offset and have no real effect on the pH, making it neutral."

Catherine Kim 3K
Posts: 31
Joined: Fri Sep 28, 2018 12:26 am

Re: KBr

Postby Catherine Kim 3K » Tue Dec 04, 2018 12:59 pm

Br is below F on the periodic table, so it is bigger.


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