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Titration Calculations 3
For these problems you are required to write your own balanced equations.
1.Calculate the concentration of a solution of sodium hydroxide given that 25.0cm3 of it required 18.8cm3 of 0.05 moledm-3 of H2SO4. Give your answer to 3 decimal places.
2.Calculate the volume of 0.05moldm-3 KOH that is required to neutralise 25.0cm3 of 0.015moldm-3 HNO3. Give your answer to one decimal place.
3.A 250cm3 solution of NaOH was prepared. 25cm3 of this solution required 28.2cm3 of 0.1moldm-3HCl for neutralisation. Calculate what mass of NaOH was dissolved to make up the original 250cm3solution. Give your answer to 2 decimal places.
4. 1.40g of pure anhydrous sodium carbonate Na2CO3 was dissolved in water and made up to 250cm3 in a standard flask. 25cm3 of this solution required exactly 24.5cm3 of a certain sample of hydrochloric acid solution for complete neutralisation. Calculate the concentration of the acid in a) moldm-3 and b) gmsdm-3. Give your answer to 2 decimal places.
5. 3.0g of a mixture of sodium carbonate and sodium chloride was made up to 250cm3 of solution. 25cm3 of this solution required 21.0cm3 of 0.1moldm-3 of HCl for neutralisation. Calculate the percentage by mass of sodium chloride in the mixture. You may assume that there is no reaction between sodium chloride and hydrochloric acid. Give your answer to one decimal place.
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Using standard solutions tofind Relative Molecular Masses 2
1.3.88g of a monoprotic acid was dissolved in water and the solution made up to 250cm3. 25.0cm3 of this solution was titrated with 0.095M NaOH solution requiring, 46.5cm3. Calculate the relative molecular mass of the acid. Give your anser to three significant figures.
2.A 1.575g sample of ethanedioic acid crystals H2C2O4 nH2O was dissolved in water and made up to 250cm3. One mole of the acid reacts with two moles of NaOH. In a titration 25cm3 of this solution of acid reacted exactly with 15.6cm3 of 0.16moledm-3NaOH. Calculate the value of n.
Extra space for working
3. A solution for a metal carbonate M2CO3, was prepared by dissolving 7.46g of the anhydrous solid in water to give 1dm3 of solution. 25.0cm3 of this solution reacted with 27.0cm3 of 0.1 moldm-3 hydrochloric acid. Calculate the relative formula mass of M2CO3 and hence calculate the relative atomic mass of the metal M
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Back titration 2
There are two questions on this sheet
- An impure sample of barium hydroxide of mass 1.6524g was allowed to react with 100cm3 of 0.2moldm-3 hydrochloric acid. When the excess acid was titrated against sodium hydroxide, 10.9cm3 of sodium hydroxide was required. 25cm3 of the sodium hydroxide required 28.5cm3 of the hydrochloric acid in a separate titration. Calculate the percentage purity of the sample of barium hydroxide.
2.Identify the relative molecular mass of a metal X from the following data. 1.g of the anhydrous X2CO3 was added to 50cm3 of hydrochloric acid of concentration 1.0 moldm-3. The remaining acid after the reaction was complete required 30.0cm3 of 1.0 moldm-3 sodium hydroxide for neutralisation.