Concentration of Solutions (Molarity) Calculations

Key Concepts

Concentration of a solution refers to the amount of solute dissolved in a given volume of solvent.

term

description

example

solute

substance that dissolves

solid sodium chloride, NaCl(s)

solvent

substance that enables solute to dissolve

liquid water, H_{2}O(l)

solution

mixture of solute dissolved in solvent

sodium chloride dissolved in water, NaCl(aq)

Concentration of a solution can be given in moles per litre (mol L^{-1} or mol/L or M).^{1}

solute

solvent

solution

units of measurement

moles mol

litres L

moles per litre mol L^{-1} (mol/L or M)

Molarity is the term used to describe a concentration given in moles per litre.

Molarity has the units mol L^{-1} (or mol/L or M).

Molarity, concentration in mol/L or mol L^{-1}, is given the symbol c (sometimes M).
For a 0.01 mol L^{-1} HCl solution we can write :
[HCl] = 0.01 mol L^{-1} (concentration implied by square brackets around formula)
or
c(HCl) = 0.01 mol L^{-1} (c stands for concentration, formula given in round brackets or parentheses)

Equation (formula or expression) to calculate the molarity of a solution (concentration in mol L^{-1}) is

c = n ÷ V

where

c = concentration of solution in mol L^{-1} (mol/L or M),
n = moles of substance being dissolved (moles of solute),
V = volume of solution in litres (L)

This equation (formula or expression) can be re-arranged to find:

moles of solute given molarity and volume of solution: n = c x V

volume of solution given moles of solute and molarity: V = n ÷ c

Molarity Concepts

Molarity is the term given for concentrations that are given in units of moles per litre (mol L^{-1} or mol/L or M)

Consider the diagram on the right.

The black box represents a 1 litre container.

The white space in the box represents the volume occupied by the solvent.

Each blue X represents 1 mole of sugar molecules.

How many moles of sugar molecules are shown in this container? 1 mole
What is the volume of the container in litres? 1 L

Molarity, concentration in mol L^{-1}, tells us how many moles of solute are in 1 L of solution.

What is the concentration of sugar molecules in the solution?
There is 1 mole of sugar molecules per 1 litre of solution.
That is 1 mole per litre, or 1 mol L^{-1} Concentration of sugar molecules = 1 mol L^{-1}

concentration of sugar solution = moles of sugar ÷ volume of solution (in L)

X

Consider the diagram on the right.

The black box represents a 0.5 litre container.

The white space in the box represents the volume occupied by the solvent.

Each blue X represents 1 mole of sugar molecules.

How many moles of sugar molecules are shown in this container? 1 mole
What is the volume of the container in litres? 0.5 L

What is the concentration of sugar molecules in the solution?
There is 1 mole of sugar molecules per 0.5 litre of solution.

Molarity, concentration in mol L^{-1}, tells us how many many moles of solute are in 1 L of solution.
If we divide both the moles of sugar molecules and the volume by the volume, that is divide by 0.5:
There are (1 ÷ 0.5 = 2) moles of sugar molecules per (0.5 ÷ 0.5 = 1) litres of solution
There are 2 moles of sugar molecules per 1 litre of solution
That is 2 moles per litre, or 2 mol L^{-1} Concentration of sugar molecules = 2 mol L^{-1}

concentration of sugar solution = moles of sugar ÷ volume of solution ( in L)

We can check this equation for our example:
moles sugar = 1 mol
volume = 0.5 L
concentration = moles ÷ volume = 1 ÷ 0.5 = 2 mol L^{-1}

X

Molarity Equation

The molarity of a solution is given by the equation :

c

=

n V

c = concentration in mol L^{-1} n = moles of solute in mol
V = volume of solution in L

If you know the moles of solute in a solution, and, you know the volume of the solution, you can calculate the concentration of the solution in mol L^{-1} using c = n ÷ V

But what if you know the concentration of the solution in mol L^{-1} and the volume of the solution in L, can you calculate how many moles of solute are present in the solution?
Yes! You just need to rearrange the equation by multiplying both sides of the equation by V (the volume of the solution):

c x V

=

n x V V

c x V

=

n

You can even calculate the volume of the solution if you know how many moles of solute are present and its concentration in mol L^{-1}.
Just rearrange the equation above by dividing both sides by c (concentration of solution in mol L^{-1})

c x V c

=

n c

V

=

n c

Examples

1. Calculating Concentration (c = n ÷ V)

Calculate the concentration in mol L^{-1} (molarity) of a sodium chloride solution containing 0.125 moles sodium chloride in 0.50 litres of solution.

What is the question asking you to calculate?
c = molarity (concentration in mol L^{-1}) of solution = ? mol L^{-1}

What information has been given in the question?
Extract the data from the question
n = moles of solute = 0.125 mol
V = volume of solution = 0.50 L

What is the relationship between what you know and what you need to find?
Write the equation:
c = n ÷ V

Substitute in the values and solve:
[NaCl_{(aq)}] = c(NaCl_{(aq)}) = 0.125 ÷ 0.50 = 0.25 mol L^{-1} (or 0.25 mol/L or 0.25 M)

2. Calculating Moles of Solute (n = c x V)

Calculate the moles of copper sulfate in 250.00 mL of 0.020 mol L^{-1} copper sulfate solution.

What is the question asking you to calculate?
n = moles of solute = ? mol

What information has been given in the question?
Extract the data from the question:
c = concentration (molarity) of solution = 0.020 mol L^{-1} V = volume of solution = 250.00 mL = 250.00 ÷ 1000 = 250.00 x 10^{-3} L = 0.25 L (since there are 1000 mL in 1 L)

What is the relationship between what you know and what you need to find?
Write the equation:
n = c x V

Substitute in the values and solve:
n = 0.020 x 0.25 = 0.0050 mol

3. Calculating Volume of Solution (V = n ÷ c)

Calculate the volume of a 0.80 mol L^{-1} potassium bromide solution containing 1.60 moles of potassium bromide.

What is the question asking you to calculate?
V = volume of solution in litres = ? L

What information has been given in the question?
Extract the data from the question:
n = moles of solute = 1.60 mol
c = molarity (concentration in mol L^{-1}) of solution = 0.80 mol L^{-1}

What is the relationship between what you know and what you need to find?
Write the equation:
V = n ÷ c

Substitute in the values and solve:
V = 1.60 ÷ 0.80 = 2.00 L

Problem Solving

The Problem: Chris the Chemist has been given a 250.00 mL volumetric flask and asked to use it to make an aqueous solution of sodium chloride, NaCl, with a concentration of 0.10 mol L^{-1} for a corrosion experiment.
The sodium chloride, NaCl, is available as white crystals.
Determine the mass in grams of sodium chloride that Chris the Chemist will need to weigh out.

What is the question asking you to do?
Determine (calculate) the mass of sodium chloride in grams.
m(NaCl) = mass of sodium chloride = ? g

What chemical principle will you need to apply?
Apply stoichoimetry (chemical calculations)

What information (data) have you been given?

solute is NaCl(s)

solvent is water (we know this because we are told Chris makes an aqueous solution)

V = volume of NaCl(aq) = 250.00 mL

c = concentation (molarity) of NaCl(aq) = 0.10 mol L^{-1}

PAUSE!

Plan.

Step 1: Calculate moles of NaCl in solution solution c = 0.10 mol L^{-1} V = 250.00 L convert volume in mL to volume in L: V(L) = V(mL) ÷ 1000
Assume the temperature of the laboratory is the same as the temperature required by the volumetric flask (eg 25^{o}C). Assume the water used to make up the solution does not contain any NaCl. n(NaCl) = c x V

Step 2: Calculate mass of NaCl(s) to be used Find the molar mass, M, of NaCl:
Use the Periodic Table to find the relative atomic masses for
M_{r}(Na)
M_{r}(Cl)
M(NaCl) = M_{r}(Na) + M_{r}(Cl)
Assume the NaCl(s) that is to be used is 100% pure (no impurities) m(NaCl) = n(NaCl) x M(NaCl)

GO!

Go with the Plan.

Step 1: Calculate moles of NaCl in solution solution c = 0.10 mol L^{-1} V = 250.00 L convert volume in mL to volume in L: V(L) = V(mL) ÷ 1000 = 250.00 ÷ 1000 = 0.25 L Assume the temperature of the laboratory is the same as the temperature required by the volumetric flask (eg 25^{o}C). Assume the water used to make up the solution does not contain any NaCl. n(NaCl) = c x V = 0.10 x 0.25 = 0.025 mol

Step 2: Calculate mass of NaCl(s) to be used Find the molar mass, M, of NaCl:
Use the Periodic Table to find the relative atomic masses for
M_{r}(Na) = 22.99 M_{r}(Cl) = 35.45 M(NaCl) = M_{r}(Na) + M_{r}(Cl) = 22.99 + 35.45 = 58.44 g mol^{-1} Assume the NaCl(s) that is to be used is 100% pure (no impurities) m(NaCl) = n(NaCl) x M(NaCl) = 0.025 x 58.44 = 1.46 g

PAUSE!

Ponder Plausability.

Have you answered the question that was asked?
Yes, we have calculated the mass of NaCl that needs to be used to make the solution.

Is your solution to the question reasonable?
Let's work backwards to see if the mass of NaCl we calculated will give the right concentration:
m(NaCl) = 1.46 g
M(NaCl) = 58.44 g mol^{-1} n(NaCl) = m(NaCl) ÷ M(NaCl) = 1.46 ÷ 58.44 = 0.025 mol
c(NaCl) = n(NaCl) ÷ V(NaCl_{(aq)}) = 0.025 ÷ 0.25 = 0.10 mol L^{-1} 1.46 g of NaCl in a 250.00 mL volume does make a 0.10 mol L^{-1} so we are confident our solution is correct.

STOP!

State the solution.

Chris the Chemist needs to weigh out 1.46 g of NaCl(s).

^{1} There are many other ways to measure concentration of solutions in chemistry. You will find tutorials dealing with these under the heading Solutions on the AUS-e-TUTE homepage.

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