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HCN + H20 <-> H3o+ + CN-
Ka = 6.2 x 10^-10
ka = [h3o+][CN-]/[HCN] = x^2/0.1m
x^2 + 6.2 x 10^-10x - 6.2 x 10^-11
x = 7.87 x 10^-6
pH = -log[x] = -log[7.87x 10^-6 = 5.1
- log(0.1 M)
= 1
14 - 1
= 13 pH
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It is a weak base.So pH depends on Kb value.
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Yes. An aqueous solution of ammonium carbonate would consist of dissociated ammonium ions and carbonate ions.
Silver chloride, which is very insoluble, would precipitate out of the solution
5.0 molar
It would be basic.
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Yes. An aqueous solution of ammonium carbonate would consist of dissociated ammonium ions and carbonate ions.
the pH would be 5 and the strength would be 1 X 10-5 molar
No. Generally, (I'm not a chemistry prof) it would be considered an aqueous solution. For instance, if salt were dissolved in water, it would be an aqueous solution of NaCl (aq).
Silver chloride, which is very insoluble, would precipitate out of the solution
5.0 molar
5.o molar
It would be basic.
5.0 molar
The formula mass of KCl is 75.5 so when 94.375g of it are dissolved in i litre water the solution prepared is 1.25 molar
Yes, in this case you would have an aqueous solution of sodium chloride and acetic acid.
Crystals of sugar are obtained.