How to predict whether the aqueous solution for the following salts are acidic , basic or neutral (a)NH4Br (b)KClO4 (c)NaHC2O4 (d)CsBr (e)KHSO4 (f)[CH3NH3]Cl?

Md Ariful Islam

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Md Ariful Islam

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You have weak acids, ammonium bromide, sodium oxalate, potassium bisulfate, and ammonium bromide. And neutral salts: potassium perchlorate, and caesium bromide. The only potential problem is sodium oxalate.

The parent acid, oxalic acid, has $pK_(a1) =1.25$ and $pK_(a2) =4.14$. Of course, $pK_(a2)$ is the one that concerns us. Compare $pK_(a2)$ to $pK_a$ ammonium bromide, $4.76$ (that's from memory, I could not find my old notes, so check on me!). So sodium oxalate is a stronger acid than ammonium bromide, and will thus give also a slightly acidic solution in water.

Another way to look at this is by the strong acid/weak base formalism. Since we are chemists, physical scientists (hopefully!), I would always prefer to get the numbers, and find the $pK_a's$.

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