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