Short answer: Sure.
Long answer: The formula given above errs on the conservative side, i.e., it actually has more sodium thiosulfate than is necessary to get the job done, as a safety factor. The balanced equation for the reaction is this:
4 NaClO + Na2S2O3 + 2 NaOH → 4 NaCl + 2 Na2SO4 + H2O
In simple English, this means that you need 1 sodium thiosulfate molecule to neutralize 4 sodium hypochlorite molecules. The molar mass of sodium hypochlorite is 74.442, and the molar mass of sodium thiosulfate pentahydrate (the crystal form we use) is 248.18. So, that means that for every 1 gram of sodium hypochlorite we need to neutralize, we need (248.18 / 4) / 74.442 = 0.8335 grams of sodium thiosulfate pentahydrate crystals.
For the 8.5% bleach example given above, that would mean 8.5 * 0.8335 = appx. 7 grams per 100 mL would be the correct amount of sodium thiosulfate for a 1:1 ratio, however, conventional wisdom is to bump that up a bit for safety's sake. Simply removing the "* 0.8335" part will give a solution that is about 1.2 times stronger than is necessary, which is a nice, conservative safety factor.
Simply put, if you make the sodium thiosulfate pentahydrate solution the exact same concentration as your bleach solution, and use it at a 1:1 ratio, you will have a dechlor solution that has a 20% margin of safety built in. At the concentrations we are using to bleach, the extra thiosulfate should not be a concern.