A chemist prepares a solution of zinc nitrate (Zn(NO3)2; MM =189.4 g/mol) by measuring out 0.502 kg of zinc nitrate into a volumetric flask and filling the flask to the 500.0 mL mark with water. Calculate the concentration in M of the chemist's zinc nitrate solution.
To calculate the concentration in Molarity (M) of the zinc nitrate solution, we need to determine the number of moles of zinc nitrate (Zn(NO3)2) and divide it by the volume in liters.
First, calculate the number of moles of zinc nitrate:
Mass of Zn(NO3)2 = 0.502 kg = 502 g
Molar mass of Zn(NO3)2 = 189.4 g/mol
Number of moles = Mass / Molar mass
Number of moles = 502 g / 189.4 g/mol
Number of moles = 2.652 mol
Next, convert the volume from mL to liters:
Volume = 500.0 mL
Volume = 500.0 mL * (1 L / 1000 mL)
Volume = 0.500 L
Now, calculate the concentration in Molarity:
Concentration (M) = Number of moles / Volume
Concentration = 2.652 mol / 0.500 L
Concentration = 5.304 M
Therefore, the concentration of the chemist's zinc nitrate solution is 5.304 M.