1.http://getrevising.co.uk/resources/titration_calculations (if asked username:kres0urce12@gmail.com password:dubaimarina)
2.http://www.4shared.com/document/yrX7TshJ/Using_indicators_and_carrying_.html
3.Calculations Involving Titrations
When talking about concentration, we tend to describe it as the amount of the solute (in terms of moles) dissolved in the solution (in one cubic decimetre), so the units are mol/dm³ so if we know the amount of a substance dissolved in a known amount of solution we can calculate the concentration. For example, imagine we were making a sodium hydroxide solution in water by dissolving exactly 40g of sodium hydroxide to make 1dm³ of solution:
2.http://www.4shared.com/document/yrX7TshJ/Using_indicators_and_carrying_.html
3.Calculations Involving Titrations
When talking about concentration, we tend to describe it as the amount of the solute (in terms of moles) dissolved in the solution (in one cubic decimetre), so the units are mol/dm³ so if we know the amount of a substance dissolved in a known amount of solution we can calculate the concentration. For example, imagine we were making a sodium hydroxide solution in water by dissolving exactly 40g of sodium hydroxide to make 1dm³ of solution:
- We know that the mass of one mole of NaOH is the sum of the atomic masses of sodium, oxygen and hydrogen:
23 + 16 + 1 = 40g - Because 40g is in the solution, we know that there is exactly one mole of NaOH in the solution
- And we know that the solution is 1dm³, so the concentration is 1 mol/dm³
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