what is the molarity of a solution prepared by dissolving 222 g of sodium carbonate in enough water to make a solution volume of 3250 mL's?
moles = 222 g/molar mass Na2CO3.
M = moles/3.250 L.
To find the molarity of a solution, you need to know the amount of solute (in moles) and the volume of the solution (in liters).
First, let's convert the mass of sodium carbonate into moles.
The molar mass of sodium carbonate (Na2CO3) is calculated as the sum of the individual atomic masses:
2(22.99 g/mol) + 12.01 g/mol + 3(16.00 g/mol) = 105.99 g/mol
We can now calculate the number of moles of sodium carbonate:
moles of Na2CO3 = mass / molar mass = 222 g / 105.99 g/mol
Next, we need to convert the volume of the solution from milliliters to liters:
volume of solution = 3250 mL / 1000 mL/L
Now that we have the moles of sodium carbonate and the volume of the solution in liters, we can calculate the molarity.
Molarity (M) is defined as moles of solute divided by liters of solution:
Molarity = moles of Na2CO3 / volume of solution
Now, let's plug in the calculated values:
Molarity = (222 g / 105.99 g/mol) / (3250 mL / 1000 mL/L)
Simplifying the equation, we have:
Molarity = (222 g / 105.99 g/mol) / (3.25 L)
Evaluating this expression, we can find the molarity of the sodium carbonate solution by dividing the moles of sodium carbonate by the volume of the solution:
Molarity ≈ 0.6507 mol/L
So, the molarity of the solution prepared by dissolving 222 g sodium carbonate in enough water to make a solution volume of 3250 mL is approximately 0.6507 mol/L.