Without calculating \(\mathrm{pH}\) values, list these solutions in order of acidity, from lowest \(\mathrm{pH}\) to highest \(\mathrm{pH}\) : (a) \(0.10 \mathrm{M} \mathrm{LiNO}_{3}\) (b) \(0.10 \mathrm{M} \mathrm{NaF}\) (c) \(0.10 \mathrm{M} \mathrm{KOH}\) (d) \(0.10 \mathrm{M} \mathrm{HCN}\) (e) \(0.10 \mathrm{M} \mathrm{HNO}_{3}\) (f) \(0.20 \mathrm{M} \mathrm{HCl}\)

First, let's analyze each solution and classify them as containing strong acids, weak acids, strong bases, or weak bases: (a) \(0.10 \mathrm{M} \mathrm{LiNO}_{3}\) - LiNO3 is a soluble salt, and neither of its ions has acidic or basic properties, so it does not affect the acidity. (b) \(0.10 \mathrm{M} \mathrm{NaF}\) - NaF is the salt of a weak acid (HF) and a strong base (NaOH). Therefore, the solution tends to be basic (due to the F- ion). (c) \(0.10 \mathrm{M} \mathrm{KOH}\) - KOH is a strong base. (d) \(0.10 \mathrm{M} \mathrm{HCN}\) - HCN is a weak acid. (e) \(0.10 \mathrm{M} \mathrm{HNO}_{3}\) - HNO3 is a strong acid. (f) \(0.20 \mathrm{M} \mathrm{HCl}\) - HCl is a strong acid, but with higher concentration than HNO3.

Now, let's order the solutions based on their acid-base properties: 1. Strong acids: these have the lowest pH values. Here, we have two - (e) and (f). However, (f) has a higher concentration than (e), so it will have a lower pH value. 2. Weak acid: these have higher pH values than strong acids, but lower than neutral or basic solutions. The only weak acid we have is (d). 3. Neutral solution: These have a pH value around 7. We have only (a). 4. Basic solution: these have higher pH values than neutral solutions. Here, we have one basic solution - (b). 5. Strong base: these have the highest pH values. The only strong base we have is (c). Based on this classification, the order of acidity (from lowest to highest pH) will be: (f) > (e) > (d) > (a) > (b) > (c).