Question

LABORATORY REPORT FORM 1. Molarity thiosulfate solution 0.01119 M 25°C 40°C 2. Actual solution temperature 25 40 c 3. Volume of sample withdrawn 20.00 20.00 20.00 20.00 mL 4. Initial buret reading 0.30 0.25 0.05 0.49 mL 5. Final buret reading 22.10 22:40 28.90 26.25mL 6. Volume thiosulfate used 21.80 22.15 28.85 25.76 mL 7. Volume thiosulfate used in liters 0.02 180 0.0.2215 0.02885 0.02574 8. Moles of thiosulfate used 2.44X10-49 48*104 8-234104288xthole 2.439x1074 2.479x104 3.228*10*4 2.882X10-9 9. Moles of 103- in 20.00 mL of sample solution moles 10. [103") equilibrium concentration 11. [Ba2+] equilibrium concentration 12. Calculated value of Ksp 13. Average value of Ksp 14. Ksp value obtained from library Reference used:

Answer 1

9) The moles of IO3- are calculated:

n IO3- = 2,439x10 ^ -4 mol Thio * (1 mol IO3- / 6 mol Thio) = 4,065x10 ^ -5 mol

Trial 2: 4.132x10 ^ -5 mol

Trial 3: 5.38x10 ^ -5 mol

Trial 4: 4.803x10 ^ -5 mol

10) The concentration in 20 mL is calculated:

[IO3-] = n / V = ​​4.065x10 ^ -5 / 0.02 = 2.033x10 ^ -3 M

Trial 2: 2.066x10 ^ -3 M

Trial 3: 2.69x10 ^ -3 M

Trial 4: 2.402x10 ^ -3 M

11) The concentration of Ba + 2 is calculated:

[Ba + 2] = [IO3-] / 2 = 2.033x10 ^ -3 / 2 = 1.017x10 ^ -3 M

Trial 2: 1.033x10 ^ -3 M

Trial 3: 1.345x10 ^ -3 M

Trial 4: 1,201x10 ^ -3 M

12) Ksp is calculated:

Ksp = [Ba + 2] * [IO3 -] ^ 2 = 1.017x10 ^ -3 * (2.033x10 ^ -3) ^ 2 = 4.203x10 ^ -9

Trial 2: 4.409x10 ^ -9

Trial 3: 9.733x10 ^ -9

Trial 4: 6.929x10 ^ -9

13) Average = 6.319x10 ^ -9

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