Experimental Procedure, Part F. A 1.0-mL volume of 0.010 M H_2 SO_3 is added to

Question

Experimental Procedure, Part F. A 1.0-mL volume of 0.010 M H_2 SO_3 is added to a mixture of 6 drops of 0.010 M HlO_3, 14 drops of deionized water, and 1 drop of starch solution. A color change in the reaction mixture occurred after 56 seconds. Assuming 20 drops per milliliter for all solutions, determine the initial molar concentration of HlO_3 after the mixing but before any reaction occurs (at time = 0). The rate of the reaction is measured by the disappearance of HlO_3. For the reaction mixture in this question, what is the reaction rate? Express the reaction rate in units of mol HlO_3/L/sec to the correct number of significant figures. The reactions in the Experimental Procedure, Parts C, E, and F, are timed. Identify the visual signal to stop timing in each reaction. Part C. Part E. Part F.

Explanation / Answer

Qsn. 6 (a)

20 drops of all solutions = 1 ml of solutions

1) 6 drops of HIO3 = 1 x 6 / 20 = 6/20 ml of HIO3

2) 14 drops of Deionized water = 1 x 14 / 20 = 14/20 ml of deionized water

3) 1 drop of starch solution = 1 x 1 /20 = 1/20 ml of starch solution

4) 1 ml of H2SO4

Total Volume of Solution Mixture = 6/20 + 14/20 +1/20 + 1 = 41/20 ml = 2.05 ml

Now use the following equation to calculate the final molar concentration of HIO3:

M1V1 = M2V2

0.01 x 6/20 = M2 x 2.05

0.01 x 0.3 = M2  x 2.05

M2 = 0.003/2.05 = 0.00146 Molar (Mole/Liter) of HIO3

So the initial molar concentration of HIO3 after mixing would be 0.00146 M

Qsn. 6 (b)

Rate of Disappearance of HIO3  =   - [HIO3]/t

= -0.00146 M / 56 sec

= - 0.000026 mole HIO3/L/Sec

So the rate of reaction would be 0.000026 mole HIO3/L/Sec.

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