Calculations using moles 2

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Presentation transcript:

Calculations using moles 2 Concentration of solutions

Objectives: To be able to calculate the concentration of a solution To understand why excess of one reactant in a chemical reaction is necessary To be able to explain the term ‘limiting reactant’ To use moles in a calculation of theoretical yield

Many reactants are in the form of solutions, eg hydrochloric acid etc The amount of substance dissolved in the solvent is called the concentration of the solution The concentration of a solution is sometimes given in g/dm3 For example, a concentration of 150g/dm3 means that there are 150g of solute dissolved in every dm3 (litre) of solvent.

Mass of solute (g) Concentration (g/dm3 ) = Volume of solution (dm3 ) 1 dm3 = 1000cm3

Example: A solution has a concentration of 4.2 g/dm3 . Calculate the mass of solute dissolved in 250 cm3 of solution.

Many solutions used in chemical reactions have amount of solute measured in moles. A 1M (molar) solution means that the molar mass of the solute is dissolved in 1dm3 of solvent How many grams of HCl are dissolved in 1dm3 of water to make a 2M solution of HCl?

Number of moles Concentration mol/dm3 = Volume (dm3) The concentration of HCl is 18.25 g/dm3 Work out the concentration in mol/dm3

Limiting reactants When we react magnesium with hydrochloric acid, eventually no more bubbles of hydrogen gas are produced. This is because one of the reactants has been used up. Usually we use excess hydrochloric acid and the magnesium is used up. The reactant that is used up is called the limiting reactant.

Using excess hydrochloric acid means that we know that all the magnesium has been used up and we can calculate how much product we should get.

What mass of zinc chloride would we get if 1g of zinc is reacted with excess hydrochloric acid. Zn + 2HCl ZnCl2 + H2 How many moles of Zinc in 1g? No of moles Zn = 1/65 No of moles Zn : no of moles of ZnCl2 1:1 No of moles of ZnCl2 = 1/65 Mass of zinc chloride produced =

From these sorts of calculations we can compare the mass of product that we actually get when we do the experiment to what we should theoretically get. Why might these masses not be the same?