NaClO Concentration

In my previous occupation the usage of bleach--$NaClO$--I found was quite staggering, and based off of the health issues that I and other coworkers were having, I wanted to see how close we were cutting it to being over exposure limits. Taking the definition, $$ 1 \, \, ppm = \frac{1 \,\,mg \,\,solute}{1 \,\,L \,\,solvent} = \frac{1 \,\,g \,\,solute}{1 \,\,m^3 \,\,solvent} $$


I have a $ 946 \,\,mL $ bottle of solution labeled to be $.65\%$ Sodium Hypochlorite. This leads me to calculate the presence of $6.149 \,\,mL$ of the entire mixture being $NaClO$. Subtracting that from the total volume to get the volume of the solvent, I obtain $.940 \,\,L \,\,solvent$. Using the fact that the density of $NaClO$ is $ \rho =1.11 \frac{g}{mL}$, I obtained $6.83\,\,g$ or $6830\,\,mg\,\,solute$. Plugging these values in for the concentration in $ppm$ I obtain $\frac{6830\,\,mg}{.940\,\,L}= 7265.957\,\,ppm$ ($\frac{g}{m^{3}}$). 


The American Industrial Hygiene Association only recommends $2\,\,ppm$ for short term exposure, which leads me to believe that my calculations might be in error in some way. Is this calculation correct or do I have some fundamental misunderstanding about the concept of molarity? I just don't feel like something that's $3633$ times more concentrated than the AIHA recommends wouldn't even make it off the drawing board, let alone into workplaces.




The recommended *Workplace Environmental Exposure Level* (WEEL) refers to the concentration of airborne substances in the workplace air. This value is not applicable to the concentration in cleaning agents or other products.


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0.65% NaClO is lower than normal household bleach, which about 5%. 


[Guidelines for the Use of Chlorine Bleach as
a Sanitizer in Food Processing Operations](http://ucfoodsafety.ucdavis.edu/files/26437.pdf)


maybe helpful to you.


Apparently, in the USA, it is permissible to wash fruits and vegetables in upto 2000 ppm NaClO. 


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