Thanks for all the responses.
A point on sulphate :
Na2SO4 • 10H2O : 322.20 g/mol (decahydrate)
NaHSO4 • H2O :138.07 g/mol (monohydrate)
H2SO4 : 98.079 g/mol
I'm presuming that when we talk about sodium sulphate, we mean the decahydrate. Let's see what concentration of sulphate ions that would be:
50g L-1 / 322.20 g mol-1 = 0.155 M
My recipe calls for 55g of sodium bisulfate :
55g L-1 / 138.07 g mol-1 = 0.398 M
Using Ilford's bleach, which calls for 10mL of conc. sulfuric acid, which contains about 18 mol L-1 :
18 mol L-1 * 0.01L / 1L = 0.18 M
If I assumed correctly that the figure of 50g/L sodium sulphate is referring to the decahydrate salt, then it does seem that the sulphate concentrations in the bleaches would have an effect, and the bisulphate bleach would have a stronger effect than a sulfuric acid one (as more sulphate ions are added to solution to produce the same drop in pH). As Rudi said, the anti-swell effectiveness of sulphate is counteracted by the very low pH, so this is all probably irrelevant.
In order to avoid increasing the bleach time due to the hardener, could the hardener be used later in the process, perhaps after the clearing bath, after a thorough wash? If I used formalin, how much would I need?