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I understand till we get “f” And also why f is directly proportional to PH. But I don’t understand why f is multiplied in solubility product with solubility of salt of weak acid.

(Sorry for poor english) (couldn’t find link of pdf of this book online)

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  • $\begingroup$ What is this book? $\endgroup$ – andselisk Jan 12 '18 at 16:42
  • $\begingroup$ 11th class ncert chemistry “acids bases and salts” $\endgroup$ – Fawad Jan 12 '18 at 16:49
  • $\begingroup$ The notations are very poorly picked. Upright "S" stands for both sulfur element and solubility, brackets "[]" are used both for concentrations and to enclose variables, the font makes it impossible to distinguish between { and (, and so on (and this is only from what you photocopied). I've never seen this book before, but I'd rather get something better than this. $\endgroup$ – andselisk Jan 12 '18 at 18:54
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Notice that $f$ is equal to the maximum concentration of $\ce{M}$, which is unchanged as part of the acid-base equilibrium. On the other hand, the pH changes the concentration of the counterion in proportion to $f$. Therefore, the second term in the solubility product is scaled accordingly.

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