What mass of sucrose (C12H22O11) is needed to make 0.500 L of a 0.200 M solution?
To find the mass of sucrose needed to make a solution, we need to use the formula:
Mass = molar mass × moles
First, let's calculate the moles of sucrose needed using the formula:
Moles = Molarity × Volume
Molarity is given as 0.200 M, and the volume is given as 0.500 L. So, the moles can be calculated as:
Moles = 0.200 mol/L × 0.500 L
Moles = 0.100 mol
Now, we need to find the molar mass of sucrose (C12H22O11). To do this, we sum up the atomic masses of each element in the molecule:
C (carbon) = 12.01 g/mol
H (hydrogen) = 1.008 g/mol
O (oxygen) = 16.00 g/mol
Molar mass of C12H22O11 = (12.01 g/mol × 12) + (1.008 g/mol × 22) + (16.00 g/mol × 11)
Molar mass of C12H22O11 = 342.30 g/mol
Finally, we can calculate the mass of sucrose needed:
Mass = molar mass × moles
Mass = 342.30 g/mol × 0.100 mol
Mass = 34.23 g
Therefore, you would need approximately 34.23 grams of sucrose to make 0.500 liters of a 0.200 M solution.
This looks, at first glance, a homework dump. You need to show SOME effort and I see none. At least tell us what you don't understand and how we can help. Also, you might include how you think the problem should be approached.
M = mols/L. You know M and L, solve for mols.
mols = grams/molar mass. You kow molar mass and mols, solve for grams.
Post your work if you get stuck.