# Concentrations and Dilutions

## Concentrations and Dilutions Revision

**Concentrations and Dilutions**

Understanding changes in **concentrations** is an invaluable tool in chemistry. The vast majority of chemical reactions will take place in the **liquid or aqueous phases** and so it is important that chemists are able to quantify not only the starting concentration of given solution but also the ways in which this concentration changes. Changes in concentrations (specifically a reduction) are called **dilutions**.

**Calculating Concentration of a Solution**

**Concentration** can be calculated using the following equation:

**\text{Concentration}=\dfrac{\text{Number of moles}}{\text{Volume}} **

Concentration: **\text{mol dm}^{-3} \text{or M}**

Number of **moles**:** \text{mol}**

Volume: **\text{dm}^3**

**Example:** Calculate the concentration of a solution made by dissolving 0.0974\text{ moles} of \text{NaCl} in 1.5 \text{ dm}^3 of water.

\begin{aligned}\text{Concentration}&=\dfrac{\text{Number of moles}}{\text{Volume}}\\&=\dfrac{\text{0.0974}}{1.5}\\&=0.065\text{ mol dm}^{-3}\end{aligned}

**Unit Conversions**

Sometimes, you may be given a volume that is not in** \text{dm}^3** and you will need to **convert** between the different **units**.

**Example: **A 0.826\text{ mol dm}^{-3}solution was formed by dissolving \text{CaO} in 430\text{ cm}^3 of water. Calculate the number of moles of\text{CaO} dissolved in water.

\begin{aligned}\text{Volume in dm}^3 &= 430\div 1000 =0.430\text{ dm}^3\\\text{Concentration} &= \dfrac{\text{Number of moles}}{\text{Volume}}\\\text{Number of moles}&= \text{Concentration}\times\text{Volume}\\\text{Number of moles}&=0.823\times0.430\\ &=0.360\text{ mol}\end{aligned}

**Mass Concentration**

Concentrations of solutions can also be measured using **mass** rather than moles so the **units** are **\text{g dm}^{-3}** instead of \text{mol dm}^{-3}.

**Equation 1:**

\text{Mass concentration}=\dfrac{\text{Mass}}{\text{Volume}}

To convert \text{mol dm}^{-3} to \text{g dm}^{-3} we can multiply the concentration in \text{mol dm}^{-3} by the \text{M}_{\text{r}} of the substance.

**Equation 2: **

**\text{Concentration }\left(\text{g dm}^{-3}\right)=\text{Concentration }\left(\text{ mol dm}^{-3}\right)\times\text{M}_{\text{r}}**

**Required Practical**

## Making and diluting a volumetric solution.

**Making a Solution**

**Weigh**the container containing the required**mass of solid**on a balance that measures up to at least 2 decimal places.- Pour the required mass into a beaker and
**reweigh**the container used. Then**calculate the****difference**between the two recorded weights. - Add 100\text{cm}^3 of
**distilled water**to the beaker and use a**glass rod**to stir the solution. If the solute does not dissolve, the beaker may need to be**heated gently**so all the solute can dissolve. - Using a funnel, pour the solution into a
**250 \text{cm}^3 volumetric flask**. **Rinse**the beaker, glass rod and funnel and add any rinsed material to the flask.- With distilled water, fill the flask up to the mark.
- Then
**invert**the flask multiple times to allow the solution to mix well.

**Making a Dilution**

- Using a
**volumetric pipette**, measure out 25.0\text{ cm}^3 of the original solution into a**volumetric flask**of 250\text{ cm}^3. - Fill the rest of the flask (up to the mark) with distilled water. Use a
**dropping pipette**for the last few drops. - Turn the flask
**upside down**several times to allow the solution to mix well.

**Note:** We use volumetric pipettes instead of measuring cylinders because they have a smaller uncertainty which means they are more accurate.

**Dilutions**

Diluting solutions means **increasing the volume** of a solution and** decreasing the concentration** without altering the amount of moles.

Since the amount of **moles** stays the **same** we can use the **concentration** **equation** to create an equation for dilutions:

**\text{C}_1\text{V}_1=\text{C}_2\text{V}_2**

\text{C}_1= **Original Concentration**

\text{V}_1=** Original Volume**

\text{C}_2= **New Concentration**

\text{V}_2= **New Volume**

**Example:** 80\text{ cm}^3 of water is added to 250\text{ cm}^3 of a 0.90\text{ mol dm}^{-3} solution of \text{KOH} . Calculate the concentration of the diluted solution.

\text{C}_1\times\text{V}_1=\text{C}_2\times\text{V}_2

\begin{aligned}\text{C}_2&= \dfrac{\text{C}_1\times\text{V}_1}{\text{V}_2}\\&=\dfrac{0.90\times0.250}{0.330}\\&=0.682 \text{ mol dm}^{-3}\end{aligned}

**Example: Calculating Moles from Volume and Concentration**

A \textcolor{#00bfa8}{1.16 \text{ mol dm}^{-3}} solution was formed by dissolving \text{Na}_2\text{CO}_3 in \textcolor{#f21cc2}{0.98\text{ dm}^3} of water. Calculate the amount of moles of \text{Na}_2\text{CO}_3 dissolved in water.

**[1 mark]**

\text{Concentration}=\dfrac{\text{Number of moles}}{\text{Volume}}

\begin{aligned}\text{Number of Moles}&=\text{Concentration}\times\text{Volume}\\&=\textcolor{#00bfa8}{1.16}\times\textcolor{#f21cc2}{0.98}\\&=\textcolor{#008d65}{1.14\text{ mol}}\end{aligned}

## Concentrations and Dilutions Example Questions

**Question 1: **Calculate the concentration of a solution made by dissolving 13 \text{ grams} of \text{CaCO}_3 in 0.75\text{ dm}^3 of water.

**[3 marks]**

\begin{aligned}\text{Number of Moles}&=\dfrac{\text{Mass}}{\text{M}_{\text{r}}}\\&=\dfrac{13}{100.1}\\&=0.1299\end{aligned}

\begin{aligned}\text{Concentration}&=\dfrac{\text{Number of moles}}{\text{Volume}}\\&=\dfrac{0.1299}{0.75}\\&=0.17 \text{ mol dm}^{-3}\end{aligned}

**Question 2: **Calculate the number of nitrate ions in a 80\text{ cm}^3 solution of \text{KNO}_3 with a concentration of 0.670\text{ mol dm}^{-3}.

**[2 marks]**

\text{Concentration}=\dfrac{\text{Number of moles}}{\text{Volume}}

\begin{aligned}\text{Number of moles}&= \text{Concentration}\times\text{Volume}\\&0.670\times0.080=0.0536\end{aligned}

\text{Number of ions}=\text{Moles}\times\text{Avogadro's constant}

\begin{aligned}\text{Number of atoms}&=0.0536\times6.022\times10^{23}\\&=3.23\times10^{22}\end{aligned}

**Question 3:** Calculate the concentration of a solution made by dissolving 6.6\text{ kg} of \text{HCl} in 0.58 \text{ m}^3 of water.

**[2 marks]**

\begin{aligned}\text{Number of Moles}&=\dfrac{\text{Mass}}{\text{M}_{\text{r}}}\\&=\dfrac{6600}{36.5}\\&=180.822\end{aligned}

\begin{aligned}\text{Concentration}&= \text{Number of moles}\div\text{Volume}\\&=\dfrac{180.822}{0.58\times1000}\\&=0.312\text{ mol dm}^{-3}\end{aligned}

**Question 4:** Calculate the volume of water in \text{cm}^3 that is needed to dilute 10\text{cm}^3 of 1.82\text{ mol dm}^{-3} of \text{NaOH} to make the concentration 1\text{ mol dm}^{-3}.

**[3 marks]**

\begin{aligned}\text{Number of moles}&= \text{Concentration}\times\text{Volume}\\&=1.82\times0.010\\&=0.0182\end{aligned}

\text{Volume}= \text{Number of moles}\div\text{Concentration}

\begin{aligned}\text{C}_1\text{V}_1&=\text{C}_2 \text{V}_2\\\text{V}_2&=\frac{\text{C}_1\text{V}_1}{\text{C}_2}\\\text{ V}_2&=0.0182\div1\\&=0.0182 \text{dm}^3\\&=18.2\text{cm}^3\end{aligned}

\text{Volume of water to be added}= 18.2-10=8.2\text{ cm}^3