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spayn [35]
3 years ago
5

What is the final acetate ion concentration when 69. g Ba(C2H3O2)2 is dissolved in enough water to make 970. mL of solution? The

molar mass of Ba(C2H3O2)2 is 255.415 g/mol.
0.28 M
0.64 M
0.91 M
0.20 M
0.56 M
Chemistry
1 answer:
Alexeev081 [22]3 years ago
8 0

Answer:

<em><u></u></em>

  • <em><u>0.56M</u></em>

Explanation:

<u />

<u>1. Dissociation equation</u>

<u />

Assuming 100% dissociation, the equation is:

  • Ba(C₂H₃O₂)₂    →   Ba²⁺   +   2C₂H₃O₂⁻

                                                          ↑

                                                    acetate ions

<u>2. Molarity</u>

<u />

Calculate the molarity, M, of the solution:

  • M = n / V(in liters)

  • n = mass in grams / molar mass

  • n = 69.g / 255.415g/mol = 0.27015 mol

  • M = 0.27015mol / 0.970liter = 0.27850 mol/liter ≈ 0.28M

<u>3. Acetate ions</u>

From the chemical equation, 1 mol of dissolved Ba(C₂H₃O₂)₂ produces 2 acetate ions in solution.

Thus, 0.28 mol/liter × 2 = 0.56 mol/liter = 0.56M ← answer

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