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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.

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    $\begingroup$ 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). $\endgroup$
    – Poutnik
    Jul 18 at 3:43
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    $\begingroup$ 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. $\endgroup$
    – andselisk ♦
    Jul 18 at 5:53

1 Answer 1

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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,$$Acidic Strength ∝ 1/pH And Basic Strength ∝ pH$$

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    $\begingroup$ Chem+Math Expression formatting reference: MathJax Basics / Chem+Math expressions/formulas/equations / Upright vs italic / Math SE Mathjax tutorial // MathJax is preferred not to be used in CH SE Q titles. $\endgroup$
    – Poutnik
    Jul 18 at 5:30
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    $\begingroup$ Nothing written here is coherent or correct from the point of logic, formatting or facts, and does not address the main point (flaw) in OP's question at all. $\endgroup$
    – andselisk ♦
    Jul 18 at 5:48
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    $\begingroup$ The p for pH as $Potenz$ is nothing but a common myth. $\endgroup$
    – AChem
    Jul 18 at 8:22

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