A 0.1017-g sample of KBrO3 (MW = 167 g/mole) was dissolved in dilute HCl and treated with an unmeasured excess of KI. The liberated iodine required 39.75 mL of a sodium thiosulfate solution. Calculate the molar concentration of the Na2S2O3. BrO3 - + 6I + 6HCl → Br - + 3I2 + 6KCl + 3H2O I2 + Na2S2O3 → 2NaI + Na2S4O6
A 0.1017-g sample of KBrO3 (MW = 167 g/mole) was dissolved in dilute HCl and treated with an unmeasured excess of KI. The liberated iodine required 39.75 mL of a sodium thiosulfate solution. Calculate the molar concentration of the Na2S2O3.
BrO3 - + 6I + 6HCl → Br - + 3I2 + 6KCl + 3H2O
I2 + Na2S2O3 → 2NaI + Na2S4O6
The type of
a. iodimetry
b. bromination
c. iodometry
d. diazotination
The role of KBrO3 in the titration is ___.
a. reducing agent
b. oxidizing agent
c. source of Br2
d. source of I2
At the endpoint of titration, the equivalence of sodium thiosulfate is equal to the following, EXCEPT ___ .
a. equivalence of KI
b. equivalence of liberated I2
c. equivalence of KBrO3
d. none of the other choices
Step by step
Solved in 2 steps
