Posted by **Hilary** on Sunday, October 30, 2011 at 12:04pm.

I'm doing the calculations on the lab "Oxidizing Power of Laundry Bleach," and I'm stuck on one part. This is what I have so far:

My average volume of sodium thiosulfate is 6.94 ML. I then converted that into moles and got 6.94X10^-4 moles. That means that NaClO is equal to that. Then I converted that to grams and got .0258 grams NaClO. I am stuck on determining the mass of NaClO per gram of bleach. What do I do?

- Ap Chemistry -
**DrBob222**, Sunday, October 30, 2011 at 1:34pm
What was the mass of the sample?

mass NaClO/g bleach = mass NaClO/mass sample

- Ap Chemistry -
**Hilary**, Sunday, October 30, 2011 at 4:32pm
The mass of bleach? Well, 5 ml was 2.947 grams, but I need the amount per 50 ml sample to do a stoichiometry equation.

- Ap Chemistry -
**Hilary**, Sunday, October 30, 2011 at 6:58pm
The mass of the sample was .0258 grams. then I divide that by 50 ml, multiple by 250 ml bleach sol'n, divide by 5 ml bleach, and divide by density of bleach (.5894). And then I get .0438 grams of ClO. Then I divide .0258 grams and .0438 and get .589, and multiple by 100 to get 58.9%. However, my answer should be around 5%.

- Ap Chemistry -
**DrBob222**, Sunday, October 30, 2011 at 10:51pm
You lost me. I can' tell what you did.

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