33. Determine how many moles of solute are dissolved in each of the following solutions.
E) a 250-mL solution of sucrose, C12H22O11(aq), with a concentration of a 0.500 mol/L
H) a 5.00-L solution of potassium sulfate, K2SO4(aq), with a concentration of 0.0250 mol/L
finished all other parts of this question, just two left again
E) a 250-mL solution of sucrose, C12H22O11(aq), with a concentration of a 0.500 mol/L
mols = M x L = 0.500 M x 0.250 L = ?
H is done the same way.
To determine the number of moles of solute dissolved in a solution, you need to use the formula:
moles = concentration (mol/L) x volume (L)
Let's calculate the number of moles of solute for each of the given solutions:
E) a 250-mL solution of sucrose, C12H22O11(aq), with a concentration of 0.500 mol/L
First, convert the volume from mL to L:
250 mL = 250/1000 L = 0.250 L
Using the formula above:
moles = 0.500 mol/L x 0.250 L = 0.125 mol
So, there are 0.125 moles of sucrose dissolved in the 250-mL solution.
H) a 5.00-L solution of potassium sulfate, K2SO4(aq), with a concentration of 0.0250 mol/L
Using the formula:
moles = 0.0250 mol/L x 5.00 L = 0.125 mol
Therefore, there are 0.125 moles of potassium sulfate dissolved in the 5.00-L solution.