Question

QUESTION 1

In the acid-base reactions below, label each reactant as either an "acid" or "base". Also, predict the products that will form for each reaction. (For molecules with subscripts, use the following format: H₃PO₄ = H3PO4 )

HNO3	+	KOH	→		+
CH3COOH	+	NaCN	→		+
Ba(OH)2	+	H2SO4	→		+

8 points   

QUESTION 2

Given the following redox reaction:

3 Cu⁺_(aq)   + Fe_(s)   → Fe³⁺_(aq) + 3 Cu_(s)

Label the reactants that are being oxidized and reduced, and also identify the oxidizing and reducing agents.

(For each label, choose from the letters on the right to match the reactant or product. Letters can be used multiple times, and not all letters necessarily need to be used.)

-       A.       B.       C.       D.	Oxidized
-       A.       B.       C.       D.	Reduced
-       A.       B.       C.       D.	Oxidizing Agent
-       A.       B.       C.       D.	Reducing Agent

A.	Fe(s)
B.	Cu(s)
C.	Fe3+(aq)
D.	Cu+(aq)

Answer 1

Question (1)

HNO₃ + KOH  → KNO₃ + H₂O

CH₃COOH + NaCN → CH₃COONa + HCN

Ba(OH)₂ + H₂SO₄ → BaSO₄ + 2H₂O

Question (2) :

   +1               0             +3                   0

3 Cu⁺_(aq)   + Fe_(s)   → Fe³⁺_(aq) + 3 Cu_(s)

Here the oxidation state of Copper decreases from +1 to 0 so copper is reduced & it acts as oxidizing agent      ( which oxidises others & reduces itself).

The oxidation state of Iron increases from 0 to +3 so iron is oxidized acts as reducing agent ( which reduces others & oxidizes itself)