Here is a question to use an example
50.0mL of 0.20M NaOH and 50.0mL of 0.20M NaOH
50.0mL of 0.20M NaOH and 50.0mL of 0.20M NaOH
-
For this particular question, you are adding together two volumes of the same compound that have the same concentration. So the concentration is the same. Final concentration = 0.20 M
Say you were combining
50.0mL of 1.0 M NaOH and 100.0mL of 0.20M NaOH
first work out how many moles of NaOH are in the stated volume of each solution
moles = molarity x Litres
moles NaOH in 50.0 ml of 1.0 M = 1.0 M x 0.0500 L = 0.050 moles
moles NaOH in 100 ml of 0.20 M = 0.20M x 0.100 L = 0.020 moles
Total moles NaOH = 0.050 mol + 0.020 mol = 0.070 moles
Total volume = 50 ml + 100 ml = 150 ml = 0.150 L
Final concentration = moles / litres
= 0.070 mol / 0.150 L
= 0.47 M NaOH
Say you were combining
50.0mL of 1.0 M NaOH and 100.0mL of 0.20M NaOH
first work out how many moles of NaOH are in the stated volume of each solution
moles = molarity x Litres
moles NaOH in 50.0 ml of 1.0 M = 1.0 M x 0.0500 L = 0.050 moles
moles NaOH in 100 ml of 0.20 M = 0.20M x 0.100 L = 0.020 moles
Total moles NaOH = 0.050 mol + 0.020 mol = 0.070 moles
Total volume = 50 ml + 100 ml = 150 ml = 0.150 L
Final concentration = moles / litres
= 0.070 mol / 0.150 L
= 0.47 M NaOH