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Chapter 16

Q. 16.4

Coulometric Titration

A 2.000-mL volume containing 0.611 3 mg of cyclohexene/mL is to be titrated in Figure 16-8. How much time is required for titration at a constant current of 4.825 mA?

FIGURE 16-8

Step-by-Step

Verified Solution

The moles of cyclohexene are

\frac{(200  mL)(0.611  3  mg/mL)}{(82.146  mg/mmol)} = 0.014  88 mmol

2Br^{−} → Br_{2} + 2e^{−}          (16-10)

In Reactions 16-10 and 16-11, each mole of cyclohexene requires 1 mol of Br_{2}, which requires 2 mol of electrons. For 0.014 88 mmol of cyclohexene to react, 0.029 76 mmol of electrons must flow. From Equation 16-3,

Moles  of  e^{−} = \frac{I  ·  t}{F} ⇒ t = \frac{(moles  of  e^{−})F}{I}

t = \frac{(0.029  76 × 10^{−3}  mol)(96  485  C/mol)}{(4.825 × 10^{−3}   C/s)} = 595.1 s

It will require just under 10 min to complete the reaction.

Test Yourself     How much time is required to titrate 1.000 mg of cyclohexene at 4.000 mA? (Answer: 587.3 s)