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10. Acidic MnO,‘ solution reacts with ethanol, CHSCI-IZOH, to produce acetic
acid, (II-ISCOOH. a. Write a balanced equation for the reaction. (5 marks) b. What volume of 0.200 M MnOf solution is needed to titrate 22.5 mL of a
0.350 M solution of ethanol? (5 marks) A concentration cell has a standard Zn2+ cathode (1 M @9103): / Zn
electrode) and a saturated (Zn(OH)2 I Zn electrode) anode. The cell potential
is measured to be 0.169 V. a. Write the two half-reactions, labelling all species with their
corresponding states (g3, s) and electrode (cathode and anode). (2 marks) b. Determine the concentration of [Zn2+] of the anode, and the 553 of
mom; (8 marks) a. Give the cell diagram notation of the electrochemical cell that could be
used to determine experimentally the dissociation constant (Kw) of water. The standard reduction potential for
02 + ZHZO + 4e‘ —I- 40H” is +0.40V For other possible half-reactions, see Table 18.1 of your textbook.
Calculate E° for this cell. (5 marks) b. Use your value from part (a) to calculate the dissociation constant at 298 K. (5 marks) The concentration of potassium ions inside a nerve cell is around 25 times
that outside the cell. Calculate the potential difference between inside and
outside a nerve cell, if it depends only on this ionic imbalance. For simplicity,
pretend that the temperature = 25°C (standard) even though body
temperature is higher than that. (10 marks)

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