calculate the molarity of a solution in which 22.6g C6H12O6 is dissolved in 1.08L of solution
moles = grams/molar mass
Solve for moles.
M = mols/L.
Solve for M
Soooo 22.6/ 180.156 + 0.125 moles
than
0.125/1.08L = 0.116 molarity??
=0.125 moles not + that was a typo...
Yes, 0.116 M is correct. And I figured out the + was a typo.
To calculate the molarity of a solution, you need to know the amount of solute (in moles) and the volume of the solution (in liters).
1. Determine the moles of solute:
The molar mass of C6H12O6 (glucose) can be calculated by adding up the atomic masses of its elements:
C (carbon) = 12.01 g/mol x 6 = 72.06 g/mol
H (hydrogen) = 1.01 g/mol x 12 = 12.12 g/mol
O (oxygen) = 16.00 g/mol x 6 = 96.00 g/mol
So, the molar mass of C6H12O6 is 180.18 g/mol.
To find the moles of C6H12O6 in the solution, divide the given mass by the molar mass:
moles = mass / molar mass = 22.6 g / 180.18 g/mol
2. Determine the volume of the solution in liters:
The given volume is 1.08L.
3. Now, calculate the molarity:
Molarity (M) is defined as moles of solute divided by liters of solution:
Molarity = moles / volume of solution
Substituting the values, we have:
Molarity = (22.6 g / 180.18 g/mol) / 1.08 L
Calculate the moles first:
moles = 0.125 mol
Then calculate the molarity:
Molarity = 0.125 mol / 1.08 L
Therefore, the molarity of the solution is approximately 0.116 M.