$pH$ of mixtures
Tutorial 1
Influence of ions on pH
Cations
Most metal cations have no effect on pH.
Examples: $ Na^+, K^+, Ca^{2+}, Mg^{2+} ....... $
Exception: Some hydrated cations are weak acids (see → this table ).
Examples: $ Al^{3+}, Fe^{3+}, Zn^{2+} $
Anions:
Anions corresponding to strong acids do not influence pH.
Examples: $ Cl^- $, $ Br^- $, $ I^- $, $ ClO_4^- $, $ NO_3^- $
Some anions are both weak acids and weak bases. They therefore belong to two acid-base pairs with the constants $ pK_{a1} $ and $ pK_{a2} $ (see → this table ). They are called ampholythes.
Examples: $ HCO_3^- $, $ HSO_3^- $, $ H_2PO_4^- $, $ HPO_4^{2-} $, $ HS^- $, ...
The pH of their solutions is calculated as follows:
$pH$ $=$ $\frac{1}{2}pK_{a1}$ $+$ $\frac{1}{2}pK_{a2}$
The other anions are weak bases. (See → this table )
Examples: $ F^- $, $ CN^- $, $ PO_4^{3-} $, $ ClO_3^- $, $ ClO_2^- $, $ ClO^- $, ......
What is the pH of a solution obtained by reacting $ 2.0 \; mol\; HCl $ with $ 1.0 \; mol \; NaOH $ in a volume of $ 1 \; L $?
What is at the end of the reaction? What are the ions then present?
For answers, use (possibly several times) the arrows ↑ Down! and ↓ Up!
Complete please this question before moving on to the next one!
At the end of the reaction,
The product of the reaction: $1.0; mole\; NaCl $
The rest: $ 1.0 \; mole\; HCl $
Ions:
$Na^+$
$Cl^-$
$H^+$
Characterize these ions from the acid-base point of view !
$Na^+$ : no influence
$Cl^-$ : no influence
$H^+$ : strong acid
Quel est le pH de cette solution?
$[H^+]=1.0\; \frac{mol}{L}$
$pH$ $=$ $-log1.0$ $=$ $0.0$
