Suppose 0.432g of zinc acetate is dissolved in 200.mL of a 16.0mM aqueous solution of ammonium sulfate.
Calculate the final molarity of acetate anion in the solution. You can assume the volume of the solution doesn't change when the zinc acetate is dissolved in it.
To calculate the final molarity of acetate anion in the solution, we need to determine the number of moles of acetate anion present in the solution and then divide it by the final volume of the solution.
First, let's find the number of moles of zinc acetate using its given mass and molar mass.
The molar mass of zinc acetate (Zn(CH3COO)2) is:
Zinc (Zn) = 65.38 g/mol
Carbon (C) = 12.01 g/mol
Hydrogen (H) = 1.01 g/mol
Oxygen (O) = 16.00 g/mol
Summing all the masses gives:
mass of Zn(CH3COO)2 = (65.38 g/mol * 1) + (12.01 g/mol * 4) + (1.01 g/mol * 6) + (16.00 g/mol * 2) = 183.49 g/mol
Now, calculate the moles of zinc acetate:
moles = mass / molar mass = 0.432 g / 183.49 g/mol
Next, we need to find the number of moles of acetate anion present in the zinc acetate.
Since each formula unit of zinc acetate (Zn(CH3COO)2) contains 2 acetate ions (CH3COO-), we can multiply the moles of zinc acetate by 2 to obtain the moles of acetate anion.
moles of acetate anion = moles of zinc acetate * 2
Now, let's calculate the final volume of the solution.
The volume of the solution is given as 200 mL, but we need to convert it to liters for consistency in units.
1 L = 1000 mL
Therefore, the volume of the solution is 200 mL / 1000 = 0.2 L
Finally, we can calculate the final molarity of acetate anion in the solution by dividing the moles of acetate anion by the final volume of the solution.
Molarity of acetate anion = moles of acetate anion / final volume of solution
Note that we already have the moles of acetate anion, which we calculated earlier, and the final volume of the solution is given as 0.2 L.
Simply divide the moles of acetate anion by the final volume to get the final molarity.
To calculate the final molarity of acetate anion in the solution, we need to determine the number of moles of acetate anion present in the solution after dissolving the zinc acetate.
First, let's calculate the number of moles of zinc acetate dissolved in the solution.
Given:
Mass of zinc acetate = 0.432g
Molar mass of zinc acetate (Zn(CH3COO)2) = 183.48 g/mol
Number of moles of zinc acetate = (mass of zinc acetate) / (molar mass of zinc acetate)
= 0.432g / 183.48 g/mol
Next, calculate the number of moles of acetate anion present in the zinc acetate. Since zinc acetate has a 1:2 ratio of zinc to acetate, the number of moles of acetate is twice the number of moles of zinc acetate.
Number of moles of acetate = 2 * (number of moles of zinc acetate)
Now, we need to calculate the final volume of the solution. Given that the volume of the solution is 200mL (0.200L) and it doesn't change when the zinc acetate is dissolved in it.
Finally, we can calculate the final molarity of acetate anion using the formula:
Molarity (M) = (number of moles of solute) / (volume of solution in liters)
Final molarity of acetate anion = (number of moles of acetate) / (volume of solution in liters)
Substitute the values we have and then calculate the final molarity of acetate anion.
Zn(C2H3O2)2 = Zn(Ac)2
0.432 g Zn(Ac)2/mol mass = moles Zn(Ac)2
mols Ac^- = 2 x moles Zn(Ac)2
M Ac^- = mols Ac^-/L soln.