- #1
Cesium
- 274
- 0
I'm having trouble determining the products of these reactions with bleach. I know for sure that all of these reactions do occur because it's part of a lab in which we find the stoichimetric coefficients for the reactants using calorimetry. Since they don't want us to be able to balance the equation, we are not given the products. Completing the experiment will not tell us what the products are (although it does determine the coefficients which may help figure it out). I've picked these three reactions just because they were the ones given, but I'm open to a larger discussion about the oxidation power of bleach.
I've been using a redox potential list as my guide:
ClO- + H2O + 2e- <-> Cl- + 2OH- 0.81
a) NaClO + KI
I'm pretty sure here that iodine would be oxidized to its elemental form. My guess is...
NaClO + 2KI + H2O --> I2 + NaCl + 2KOH
b) NaClO + Na2S2O3
I've looked online for this one and I only find this reaction which occurs in basic solution. I'm not sure if the thiosulfate ion could be oxidized to the sulfate ion in a neutral solution. Perhaps to S2O6-2?
4ClO- + S2O3-2 + 2OH- --> 2SO4-2 + 4Cl- + H2O
c) NaClO + Na2SO4
This one I have no clue. I would think that no reaction would occur. Oxidation to the peroxydisulfate ion seems difficult:
S2O82- + 2e--> 2SO42- 2.010
I've been using a redox potential list as my guide:
ClO- + H2O + 2e- <-> Cl- + 2OH- 0.81
a) NaClO + KI
I'm pretty sure here that iodine would be oxidized to its elemental form. My guess is...
NaClO + 2KI + H2O --> I2 + NaCl + 2KOH
b) NaClO + Na2S2O3
I've looked online for this one and I only find this reaction which occurs in basic solution. I'm not sure if the thiosulfate ion could be oxidized to the sulfate ion in a neutral solution. Perhaps to S2O6-2?
4ClO- + S2O3-2 + 2OH- --> 2SO4-2 + 4Cl- + H2O
c) NaClO + Na2SO4
This one I have no clue. I would think that no reaction would occur. Oxidation to the peroxydisulfate ion seems difficult:
S2O82- + 2e--> 2SO42- 2.010