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Calculate Concentrations of Solutions (Edexcel IGCSE Chemistry)
Revision Note
Calculate Concentrations of Solutions
- A solute is a solid substance that dissolves into a liquid
- The amount of solute can be expressed in grams (g) or moles (mol)
- A solvent is the liquid that a solute dissolves in
- The amount / volume of a solvent is measured in cm3 or dm3
- Most chemical reactions occur between solutes which are dissolved in solvents, such as water or an organic solvent
- A solution is the mixture formed when a solute dissolves in a solvent
- The amount / volume of a solution measured in cm3 or dm3
- Concentration refers to the amount of solute there is in a specific volume of the solvent
- The greater the amount of solute in a given volume, the greater the concentration
- Concentration is sometimes commonly referred to as strength
- For example, dissolving more coffee in hot water results in a stronger coffee
- Typically, concentration is expressed in terms of the amount of substance per dm3
- Therefore, the units of concentration are:
- g / dm3
- mol / dm3
- Therefore, the units of concentration are:
- It is more useful to a chemist to express concentration in terms of moles per unit volume rather than mass per unit volume
- To calculate concentration in mol / dm3 we use the following equation:
The concentration-moles formula triangle
- Volumes are often expressed in cm3, but dm3 must be used when calculating concentration
- To convert cm3 to dm3, divide by 1000
- To convert dm3 to cm3, multiply by 1000
Converting between cm3 and dm3
Worked example
Calculate the amount of solute, in moles, present in 2.5 dm3 of a solution whose concentration is 0.2 mol / dm3.
Answer:
- Write down the information you are given in the question:
- Concentration of solution: 0.2 mol / dm3
- Volume of solution: 2.5 dm3
- Calculate the number of moles:
- Moles = concentration x volume
- Moles = 0.2 x 2.5 = 0.5 mol
Worked example
Calculate the concentration of a solution of sodium hydroxide, NaOH, in mol / dm3, when 80 g is dissolved in 500 cm3 of water.
Relative atomic masses, Ar: Na = 23; H = 1; O = 16
Answer:
- Calculate the Mr of NaOH:
- 23 + 16 + 1 = 40
- Determine the number of moles of NaOH:
- 40 g = 1 mole
- So, 80 g = 2 moles
- Convert cm3 to dm3:
- = 0.5 dm3
- Calculate the concentration:
- Concentration =
- Concentration = = 4 mol / dm3
Worked example
25.0 cm3 of 0.050 mol / dm3 sodium carbonate was completely neutralised by 20.00 cm3 of dilute hydrochloric acid. Calculate the concentration in mol / dm3 of the hydrochloric acid.
Na2CO3 + 2HCl → 2NaCl + H2O + CO2
Answer:
- Calculate the moles of sodium carbonate:
- Moles of Na2CO3 = concentration x volume
- Remember: The volume needs to be in dm3
- Moles of Na2CO3 = 0.05 x = 0.00125
- Moles of Na2CO3 = concentration x volume
- Calculate the moles of hydrochloric acid:
- The balanced symbol equation shows that 1 mole of Na2CO3 reacts with 2 moles of HCl
- So, 0.00125 moles of Na2CO3 reacts with 0.00250 moles of HCl
- Calculate the concentration of hydrochloric acid:
- Concentration =
- Remember: The volume needs to be in dm3
- 20 cm3 ÷ 1000 = 0.02 dm3
- Concentration = = 0.125 mol / dm3
- Concentration =
Examiner Tip
Don't forget your unit conversions:
To go from cm3 to dm3 : divide by 1000
To go from dm3 to cm3 : multiply by 1000
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