what is the molarity of a solution prepared by dissolving 10.60g of Na2CO3 in enough distilled water to obtain 250.0ml of solution
How many mols is 10.6 g ?
mol mass = 2(23) + 12 + 3(16) = 106 g/mol
so we have (1/10) of a mol in 1/4 of a liter
that would be 4/10 of a mol in a liter
To find the molarity of a solution, you need to know the number of moles of the solute (in this case, Na2CO3) and the volume of the solution in liters.
Step 1: Calculate the moles of Na2CO3:
The molar mass of Na2CO3 is:
2(22.99 g/mol) + 12.01 g/mol + 3(16.00 g/mol) = 105.99 g/mol
To find the moles of Na2CO3, divide the given mass (10.60 g) by the molar mass:
moles = mass / molar mass
moles = 10.60 g / 105.99 g/mol
moles ≈ 0.100 moles
Step 2: Convert the volume from milliliters to liters:
Given volume = 250.0 ml = 250.0 cm³
1 liter = 1000 cm³
volume = 250.0 cm³ / 1000 cm³/L = 0.250 L
Step 3: Calculate the molarity (M):
Molarity (M) = moles / volume
Molarity = 0.100 moles / 0.250 L
Molarity = 0.400 M
Therefore, the molarity of the solution is approximately 0.400 M.