Education • All: 4.5: Concentration of Solutions

MOLARITY

$\large Molarity\;=\;M\;=\;\frac{moles\;of\;solute}{1\;L\;solution\;(solute+solvent)}$

Example 1:
What's the molarity of 5.00g C6H12O6 if you were to make 100 mL solution?

$\large 5.00g\;\times (\frac{1\;mole}{180\;g})=0.0278\;mol \\\\\\M\;=\;\frac{moles\;C_{6}H_{12}O_{6}}{1\;L\;solution}\;=\;\frac{0.0278\;mol}{0.100\;L}=0.278\;M$

Example 2:

What's the molarity of K+ in 0.015M of K2CO3?

$\large 0.015M\;K_{2}CO_{3}\;\times\;\frac{2\;mol\;K^{+}}{1\;mol\;K_{2}CO_{3}}=0.030M\;K^{+}$

DILUTING A SOLUTION

Moles of solute concentration = Moles solute diluted

Mc x Vc = Md x Vd

Example:

What is the volume of a concentrated 5.0M of K2Cr2O7 if it has a diluted value of 0.10M and 250mL.

$\large \\(5.0M)\times (XmL)=(0.10M)\times (250mL) \\\\X=5.0mL$

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4.5: Concentration of Solutions

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