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# Balanced Molecular Ionic Net Equations

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1. Calculate the concentration of a Pb(NO3)2 in a solution made up of 49.1 mg of solid Pb(NO3)2 (MW=33.22) dissolved in 65.00 mL of water (MW=18.02).

2. Write balanced molecular, ionic, and net equations for the following reactions.

a. KCN(aq) + MgCI2(aq) - KCL (aq) +Mg(CN)2(aq)

b. Zn(NO3)2 (aq) +H3PO4(aq) - Zn3(PO4)2(s)+ HNO2(aq)

3. In the following oxidation-reduction, identify the substance that is oxidized, the substance that is reduced, the oxidizing agent, and the reducing agent. 10 HI(aq) + 2KMnO4(aq) + 3H 2SO4(aq) â?" 5 I2 (s) + 2MnSO4(aq) +K2 SO4(aq) + 8 H2O(l)

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The expert examines balanced molecular ionic net equations.

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chemistry 121
1. Calculate the concentration of a Pb(NO3)2 in a solution made up of 49.1 mg of solid Pb(NO3)2 (MW=33.22) dissolved in 65.00 mL of water (MW=18.02).
SOLUTION:
Note:
The molar mass of Pb(NO3)2 is 331.2 g/mol and not 33.22 g/mol.
Converting mg Pb(NO3)2 to gram:
49 mg Pb(NO3)2 x (1 g/1000 mg) = 0.049 g Pb(NO3)2
Solving for mole Pb(NO3)2:
0.049 g Pb(NO3)2 x (1 mole Pb(NO3)2 / 331.2 g) = 1.479 x 10-4 mole Pb(NO3)2
Solving for volume of solution in liter:
65 mL H2O x (1 L /1000 mL) = 0.065 L
Note: The volume that can be contributed by the solute (Pb(NO3)2) can be considered ...

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