An aqueous solution is made by dissolving 15.6 grams of nickel acetate in 373 grams of water.
The molality of nickel acetate in the solution is
I assume that is nickel(II) acetate.
moles Ni(C2H3O2)2 = grams/molar mass.
m = moles/kg soln.
To find the molality of nickel acetate in the solution, we need to first calculate the number of moles of nickel acetate and the mass of water in the solution.
1. Calculate the number of moles of nickel acetate:
To do this, we need to use the molar mass of nickel acetate (Ni(CH3CO2)2).
The molar mass of nickel acetate =
atomic mass of Ni (28.02 g/mol) + 2 * atomic mass of C (12.01 g/mol) +
6 * atomic mass of H (1.01 g/mol) + 2 * atomic mass of O (16.00 g/mol)
= 28.02 + 2 * 12.01 + 6 * 1.01 + 2 * 16.00
= 28.02 + 24.02 + 6.06 + 32.00
= 90.10 g/mol
To calculate the number of moles, we will divide the mass of nickel acetate (15.6 grams) by its molar mass:
Number of moles of nickel acetate = 15.6 g / 90.10 g/mol
2. Calculate the mass of water:
The mass of water is given as 373 grams.
3. Calculate the molality of nickel acetate in the solution:
Molality is defined as the number of moles of solute (nickel acetate) per kilogram of solvent (water). Since we have the mass of water in grams, we need to convert it to kilograms.
Molality = (Number of moles of nickel acetate) / (Mass of water in kilograms)
Molality = (15.6 g / 90.10 g/mol) / (373 g / 1000 g/kg)
Molality = (15.6 g * 1000 g/kg) / (90.10 g/mol * 373 g)
Molality ≈ 0.438 mol/kg
Therefore, the molality of nickel acetate in the solution is approximately 0.438 mol/kg.