calculate the molarity of sodium carbonate in a solution prepared by dissolving 5.3g in enough water to form 250ml of solution
how many moles in 5.3g?
Molarity is moles/liter
Not given
You're not willing to do ANY of this work? I've posted a hint at your duplicate post above. You're right, mols are given BUT you know grams and you can calculate mols.
To calculate the molarity of sodium carbonate in the solution, we need to follow a few steps:
Step 1: Convert the mass of sodium carbonate to moles.
First, we need to convert the mass of sodium carbonate (5.3 g) to moles using its molar mass. The molar mass of sodium carbonate (Na2CO3) is:
Na = 22.99 g/mol
C = 12.01 g/mol
O = 16.00 g/mol
So, 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 convert the mass to moles, divide the mass by the molar mass:
moles of Na2CO3 = (5.3 g) / (105.99 g/mol)
Step 2: Calculate the volume of the solution in liters.
The volume of the solution is given as 250 ml, but for molarity calculations, we need to use liters. So, we convert 250 ml to liters by dividing by 1000:
volume of solution = (250 ml) / (1000 ml/L)
Step 3: Calculate the molarity.
Now that we have the moles of Na2CO3 and the volume of the solution in liters, we can calculate the molarity using the formula:
Molarity (M) = moles / volume in liters
Molarity of sodium carbonate = moles of Na2CO3 / volume of solution
Substituting the values we calculated:
Molarity of sodium carbonate = (moles of Na2CO3) / (volume of solution in liters)
Therefore, to calculate the molarity, you would need to divide the moles of Na2CO3 (calculated in step 1) by the volume of the solution in liters (calculated in step 2).