1. a. Write the balanced net ionic equation for the formation of iodine when a h

Question

1. a. Write the balanced net ionic equation for the formation of iodine when a hypochlorite containing cleanser reacts with a solution of Kl. b. How many moles of hypachlorous acid can be reduced by 1.2 x 10^-2 moles [? 2. a. Write the balanced net ionic equation for the reaction of iodine with a standardized sodium thiosulfate solution. 3. How many moles of I2 can be reduced with 0.75 mL of 0.15 M Na2S2O3? solution is added near the end of the titration, what color change will be at the end point of the thiosulfate-iodine titration?

Explanation / Answer

1a,ClO- + 2I- + 2 H+ ----->I2 + Cl- + H2O

b. from the above equation no of moles of hypochlorite reduced=1.2x10^-2molx1mol/2mol=6x10^-2mol

2a,2 S2O32- + I2 ------> 2 I- + S4O62-

b.no of moles of thiosulphate=0.15Mx0.075L=0.01125mol

from the above equation no of moles of iodine reduced=0.01125molx1mol/2mol=0.005625mol

3.blue color is appeared due to the formation of iodine-starch complex and it disappears with excess of Na2S2O3

Related Questions

Navigate

• Browse (All)
• Browse 1
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.