Assume the following substances form solutions at the same concentration, which one would provide an aqueous solution of the highest pH value? A) HCN (Ka=4.9×10^-10) B) HClO ( Kb= 2.9 × 10^-8) C) NH4 + (Ka= 5.6 × 10^-10) D) HF (Ka= 6.4×10^-4) E) HCl
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Assume the following substances form solutions at the same concentration, which one would provide an aqueous solution of the highest pH value?
A) HCN (Ka=4.9×10^-10)
B) HClO ( Kb= 2.9 × 10^-8)
C) NH4 + (Ka= 5.6 × 10^-10)
D) HF (Ka= 6.4×10^-4)
E) HCl
Given acids with their Ka values:
- HCN (Ka=4.9×10-10)
- HClO (Kb= 2.9 ×10-8)
- NH4+ (Ka= 5.6 × 10-10)
- HF (Ka= 6.4×10-4)
We have to find the acid that would provide an aqueous solution of the highest pH value when all the acids have the same concentration.
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