acid/base tritation questions

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Acidbase titrations.
1 i) Calculate the number of moles of sulphuric acid of concentration 0.5 moldm3 in the following volumes.
a) 25.0 cm³, b) 55.0 cm³.
ii) Convert the above moles into masses of sulphuric acid present.
2) If the following quantities of sodium hydroxide were dissolved in separate volumes of 1000 cm³ of water
what would be the concentrations of the resulting solutions in moldm3?
a) 40g, b) 10g, c) 25g.
3) What masses of potassium hydroxide would have to be dissolved in 250 cm³ of distilled water to form
solutions with the following concentrations?
a) 0.50 moldm3 b) 0.80 moldm3 c) 1.25 moldm3.
4) If the following mole quantities sulphuric acid were dissolved in 25.0 cm³ of solution what would be the
concentration of the acid, in moldm3?
a) 0.0025, b) 0.0005, c) 0.001.
5) Consider the following balanced equation for the reaction between sodium hydroxide and sulphuric acid.
2NaOH + H2SO4 ==> Na2SO4 + 2H2O
How many moles of acid will react with the following quantities of sodium hydroxide?
a) 4 moles, b) 0.5 moles, c) 40g, d) 10g.
6) In order to neutralise 25.0 cm³ of dilute hydrochloric acid solution, 30.5 cm³ of aqueous sodium hydroxide
of 1.00 moldm3 concentration were required. Determine the concentration of the acid solution.
a) Write a balanced equation for the reaction that takes place between hydrochloric acid and sodium
hydroxide.
b) Calculate the number of moles of sodium hydroxide used in the titration.
c) Using the balanced equation for the reaction and your answer to (b) calculate the number of moles of
hydrochloric acid used.
d) Calculate the concentration of the hydrochloric acid solution.
7) During an acid/base titration 25 cm³ of sulphuric acid were neutralised by 34.6 cm³ of dilute potassium
hydroxide solution of concentration 0.25 moldm3 . Determine the concentration of the acid solution.
a) Write a balanced equation for the reaction that takes place between sulphuric acid and potassium hydroxide.
b) Calculate the number of moles of potassium hydroxide used in the titration.
c) Using the balanced equation for the reaction and your answer to (b) calculate the number of moles of
sulphuric acid used present in 25 cm³ of this solution.
d) Calculate the concentration of the sulphuric acid solution.

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