# Chemistry 2

The bottle of bleach lists the percentage of sodium hypochlorite as 6.0%. If the density of commercial bleach is 1.084 g/mL, how many mL of .150 M sodium thiosulfate is required to reach the endpoint in a titration if a student analyzed a 2.0 mL sample of bleach.

1. The first thing I would do is calculate the molarity of the bleach.
That is 1.084 g/mL x 1000 mL x 0.06 = 65.04 g and that divided by the molar mass NaOCl = 65.04/74.44 = 0.874M. Therefore, a 2 mL sample will have mols = M x L = 0.874 x 0.002L = 0.00175 mols.

Are you treating the NaOCl with I^- to oxidize it to I2 then titrating the liberated I2 with thiosulfate?
OCl^- + 2I^- ==>I2 + Cl^-
2S2O3^2- + I2 ==>2I^- + S4O6^2-

1 mol OCl^- = 1 mol I2 = 2 mol S2O3
Therefore 1/2 mol NaOCl = 1 mol S2O3

We have 0.00175 mol NaOCl. That will use 1/2 that of thiosulfate.
M thiosulfate = mols/L
You know M and mols; solve for L and convert to mL.

posted by DrBob222

## Similar Questions

1. ### Chemistry

A solution of household bleach contains 5.25% sodium hypochlorite, NaOCl, by mass. Assuming that the density of bleach is the same as water, calculate the volume of household bleach that should be diluted with water to make 500.0
2. ### Chemistry

A solution of household bleach contains 5.25% sodium hypochlorite, NaOCl, by mass. Assuming that the density of bleach is the same as water, calculate the volume of household bleach that should be diluted with water to make 500.0
3. ### chemistry

A solution of household bleach contains 5.25% sodium hypochlorite, NaOCl, by mass. Assuming that the density of bleach is the same as water, calculate the volume of household bleach that should be diluted with water to make 500.0

Titration of a Sample of Household bleaches: The oxidizing agent in a household bleach is determined by placing 100 mL of distilled water in a 250 mL Erlenmeyer flask and adding 10 mL of the 10% (w/w) KI solution, swirling the
5. ### CHEMISTRY.

Knowing that bleach contatins 5% aqueous sodium hypocholirte, how much sodium hypochlorite does 700ml of 10% bleach contain? (in grams)
6. ### Chemistry

If you are using 5.25% (mass/mass) bleach solution and you determine that the density of the bleach solution is 1.08 g/mL, how many moles of sodium hypochlorite are present in a 4.00 mL sample?
7. ### Chemistry

If you are using 5.25% (mass/mass) bleach solution and you determine that the density of the bleach solution is 1.08 g/mL, how many moles of sodium hypochlorite are present in a 4.00 mL sample?
8. ### Chemistry

Calculate the mass in grams of the undiluted bleach that was in the sample of bleach titrated. Given: Density of undiluted bleach unkown is 1.042 g/mL. 14.44 mL of .100 M Na2S2O3. .0537 grams of NaClO. Each sample should conain
9. ### Chemistry

Calculate [ClO^-] in a 6% bleach solution. A 6% bleach solution contains 6 grams of NaClO per 100 grams bleach. The density of 6% bleach is 1.07g/mL.
10. ### Chemistry

Calculate [ClO^-] in a 6% bleach solution. A 6% bleach solution contains 6 grams of NaClO per 100 grams bleach. The density of 6% bleach is 1.07g/mL.

More Similar Questions