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According to the procedure, 5.00 mL of AgNO3 (0.08 mol/L) will be mixed with 5.00 mL of Na2CO3 (0.45 mol/L). Determine the initial concentration of Ag\(^+\) ions in the initial mixture before any reaction takes place. Submit your answer with 3 decimal places. Do not include units.

Answer :

According to the given procedure, 5.00 mL of AgNO3 with a concentration of 0.08 mol/L will be mixed with 5.00 mL of Na2CO3 with a concentration of 0.45 mol/L. the initial concentration of Ag+ ions in the initial mixture before any reaction takes place is 0.040 mol/L.

To determine the initial concentration of Ag+ ions in the initial mixture before any reaction takes place, we need to calculate the number of moles of AgNO3 in the 5.00 mL solution.

First, let's convert the volume from milliliters to liters:

5.00 mL = 5.00 × 10^-3 L

Now, we can calculate the number of moles of AgNO3 using the formula:

moles = concentration × volume

moles of AgNO3 = 0.08 mol/L × 5.00 × 10^-3 L

moles of AgNO3 = 4.00 × 10^-4 mol

Since AgNO3 dissociates into Ag+ and NO3- ions in solution in a 1:1 ratio, the initial concentration of Ag+ ions in the mixture is equal to the moles of AgNO3 divided by the total volume of the mixture.

Total volume of the mixture = 5.00 mL + 5.00 mL = 10.00 mL = 10.00 × 10^-3 L

The concentration of Ag+ ions = moles of AgNO3 / total volume of the mixture

Concentration of Ag+ ions = (4.00 × 10^-4 mol) / (10.00 × 10^-3 L)

Concentration of Ag+ ions = 0.040 mol/L

Therefore, the initial concentration of Ag+ ions in the initial mixture before any reaction takes place is 0.040 mol/L.

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