Determine which solution in each pair is more acidic.
(A) 0.0100 M in HCl and 0.0100 M in KOH
(B) 0.0100 M in HF and 0.0100 M in KBr
(C) 0.0100 M in NH4 Cl and 0.0100 M in CH3 NH3 Br
(D) 0.100 M in NaCN and 0.100 M in Caci2
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The correct option in (B) due to the following reasons:
- In the first reaction as HCl is strong acid and KOH is a strong base. So, when a strong acid reacts with strong base then salt and water is formed and the reaction is called Neutralization reaction.
- As, In option A the reaction is neutralization. so, it is not acidic.
- In option C , As both NH4^(+) ion has +1 charge and Cl^(-) and Br^(-) both ion have +1 charge . So, Due to comman ion effect presence result in suppressing the acidity.
- On the other hand, In option D due to the presence of CN^(-) ion basic nature is observed in the combination.
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