Suppose of copper(ii) acetate is dissolved in of a aqueous solution of sodium chromate. calculate the final molarity of acetate anion in the solution. you can assume the volume of the solution doesn't change when the copper(ii) acetate is dissolved in it. be sure your answer has the correct number of significant digits.

0.0714 M for the given variables

Explanation:

The question is missing some data, but one of the original questions regarding this problem provides the following data:

Mass of copper(II) acetate:

Volume of the sodium chromate solution:

Molarity of the sodium chromate solution:

Now, when copper(II) acetate reacts with sodium chromate, an insoluble copper(II) chromate is formed:

Find moles of each reactant. or copper(II) acetate, divide its mass by the molar mass:

Moles of the sodium chromate solution would be found by multiplying its volume by molarity:

Find the limiting reactant. Notice that stoichiometry of this reaction is 1 : 1, so we can compare moles directly. Moles of copper(II) acetate are lower than moles of sodium chromate, so copper(II) acetate is our limiting reactant.

Write the net ionic equation for this reaction:

Notice that acetate is the ion spectator. This means it doesn't react, its moles throughout reaction stay the same. We started with:

According to stoichiometry, 1 unit of copper(II) acetate has 2 units of acetate, so moles of acetate are equal to:

The total volume of this solution doesn't change, so dividing moles of acetate by this volume will yield the molarity of acetate:

3 hours because it is a decent distance.

ill try to . no promises tho.

explanation: