Question:1 (NOTE: liquid bleach refers to the original sample of liquid bleach.;

Question

Question:1 (NOTE: liquid bleach refers to the original sample of liquid bleach.; bleach solution refers to the diluted sample of liquid bleach) A 10.0 mL sample of liquid bleach is diluted to 100 mL in a volumetric flask. A 25.0 mL sample of this bleach solution is analyzed according the procedure described in the lab. 21.3 mL of a 0.159 M solution of Na2S2O3 is needed to reach the stoichiometric point of the titration. Calculate the number of moles of ClO- that are present in the 25.0 mL sample of bleach solution.

How many grams of Cl2 are equivalent to the number of moles of ClO- calculated above?

How many grams of liquid bleach are actually analyzed? Assume that the density of liquid bleach is 1.084 g/mL.

Calculate the percent "available chlorine" in the liquid bleach.






Question:2
Balance the following redox equation (a reaction that occurs in this week's lab) using the method discussed in Section 19.1 in your textbook. The reaction occurs in basic solution. Show all your work, including the half-reactions that lead to the final balanced equation and the number of electrons that must be used to balance each half reaction.

ClO-(aq) + I-(aq) I2(aq) + Cl-(aq)

Explanation / Answer

I'm gonna answer (for now) question 2. Question 1 post it in another question thread.

ClO- + I- -----> I2 + Cl-

The half reactions:
2I- -------> I2 + 2e-
H2O + ClO- +2e- --------> Cl- + 2OH-

The final balanced reaction would be:
ClO- + 2I- + H2O --------> Cl- + I2 + 2OH-

Hope this helps

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