Are my protolysis equations right? We had the task to solve several salts in water and measure the pH value of the solution. After that we should "create" the protolysis equation and to tell about Chemical equilibrium[s].

I get some possible result equations, but I'm really unsure about them. The [] brackets were used to make the ionic loads easier visible. solving equations:


$\ce{KNO3 &lt;=&gt; [NO3]- + [K]+}$
$\ce{FeCl3 &lt;=&gt; [Fe]^{3+} + [Cl]-}$
$\ce{NH4Cl &lt;=&gt; [NH4]+ + [Cl]-}$`
$\ce{NaHSO4 &lt;=&gt; [HSO4]- + [Na]+}$


my protolysis equations:


$\ce{[NO3]- + H2O &lt;=&gt; HNO3 + [OH]-}$
$\ce{[Fe(H2O)6]^{3+} + H2O &lt;=&gt; [Fe(H2O)5OH]^{2+} + [H3O]+}$
$\ce{[NH4]+ + H2O &lt;=&gt; NH3 + [H3O]+}$
$\ce{[HSO4]- + H2O &lt;=&gt; [SO4]^{2-} + [H3O]+}$


I would say that all equations run bi-directional, because the result of solving equations can vary dependent on temperature for example, and the protolysis equations should be bi-directional because we're having a solution, which isn't a pure acid.

Additionally, I got the question if I can draw conclusions on the pH-change through those protolysis reactions. I would say yes, but not very well, depending on the sum of all hydrogen-containing ions like $\ce{H3O+}$
yes, they are, all of them are bidirectional.
It is not possible to draw conclusions about the pH value, because of the different abilities to solve in water and because those reaction may cause an increased or a decreased temperature.

(Source: my teacher)