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Which of the following is the correct method to calculate the percent ionization of HA in a 0.10 M solution, given that the acid dissociation constant (K_a) is known?
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6. Chemical Quantities & Aqueous Reactions
Calculate Oxidation Numbers
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In the reaction 16H^+ + 2Cr_2O_7^{2-} + C_2H_5OH → 4Cr^{3+} + 11H_2O + 2CO_2, which element is reduced?
A
Hydrogen
B
Oxygen
C
Carbon
D
Chromium
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Identify the oxidation states of the elements involved in the reaction before and after the reaction to determine which element is reduced.
Focus on chromium in the dichromate ion (Cr_2O_7^{2-}). In dichromate, chromium typically has an oxidation state of +6.
Look at the chromium in the product, Cr^{3+}, where chromium has an oxidation state of +3.
Since the oxidation state of chromium decreases from +6 to +3, chromium gains electrons and is therefore reduced.
Confirm that other elements (hydrogen, oxygen, carbon) do not show a decrease in oxidation state, so they are not reduced.
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