1. M = moles solute L vol solution M= 0.75 moles = 3 M 0.25 liters
241 # 4.
Vol = 0.25 L of solution
Moles = 0.75
Molarity (M) = x
NOTE: VOLUME IS IN Liters, solute is in moles…no conversions needed
M = moles solute
L vol solution
M= moles = 3 M
0.25 liters

2. M = moles solute L vol solution M= 1.8 moles = 3 M 0.6 liters
241 # 5.
Vol = 600 mL L of solution
Moles = 1.8 mol
Molarity (M) = x
NOTE: VOLUME IS IN NOT in Liters, must convert.
Volume is given in milliliters, you MUST convert to liters to substitute into molarity equation.,
600mL 1L = 0.6 L
1000mL
M = moles solute
L vol solution
M= moles = 3 M
0.6 liters

3. M = moles solute L vol solution M= 1 moles = 2 M 0.5 liters
241 # 6.
Vol = 500 mL L of solution
Moles = 1.0 mol
Molarity (M) = x
NOTE: VOLUME IS IN NOT in Liters, must convert.
Volume is given in milliliters, you MUST convert to liters to substitute into molarity equation.,
500mL 1L = 0.6 L
1000mL
M = moles solute
L vol solution
M= moles = 2 M
0.5 liters

4. M = moles solute L vol solution moles = MASS GFM N 2 x 14 28 H 8 x 1 C
241 # 12.
Vol = 2000 mL L of solution
Mass = 48 grams (NH4)2CO3
Molarity (M) = x
SKILL: calculating Molarity from grams and milliliters.
NOTE: VOLUME IS IN NOT in Liters, must convert to Liters. Solute is in grams, must convert to moles.
Volume is given in milliliters, you MUST convert to liters to substitute into molarity equation.,
2000mL 1L = 2 L
1000mL
M = moles solute
L vol solution
moles = MASS
GFM
Convert grams of (NH4)2CO3 to moles.
96 g/mol N 2
x 14 28 H 8
x 1 C 1
x 12 12 O 3
x 16 48
M = =
2 L
moles = 48 grams
96 g/mol
moles = 0.5