Relationship of acids and bases with pH. (Proportional Relationship) [duplicate]

Can someone please clarify the relationship between acidic-basic strength and pH? I have come across conflicting information and am unsure about the correct understanding.

Some people including my chemistry teacher say that

$$\text{Acidic Strength} ∝ \frac{1}{pH} \\ \text{Basic Strength} ∝ pH$$

According to my research, it's called proportional relationship. Well, I'm asking whether this information is accurate or not. If not? show me the correct one.

• Express the relations quantitatively and decide yourself. E.g. the simplified equation for weak acid is pH=0.5(pKa - log c), for weak base pH= 14 - 0.5(pKb - log c). Jul 18 at 3:43
• There is either a wrong terminology at play, or something lost in translation/definition. pH is not how acidic/basic strength is quantified at all. Jul 18 at 5:53

In pH p stands for "potenz" Which means taking negative logarithm of active mass of hydronium ion $$pH = -log(a)$$ where a is the active mass of hydronium ions. As we know that the acidic strength increases with the increase of active mass of hydronium ions the negative logarithm of active mass i.e., pH should decrease with acidic strength. Therefore,$$Acidic Strength ∝ 1/pH And Basic Strength ∝ pH$$
• The p for pH as $Potenz$ is nothing but a common myth. Jul 18 at 8:22