• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

Acid-Base titration of Sulphuric acid and Sodium Hydroxide

Extracts from this document...


ACID - BASE TITRATION AIM The aim is to perform an experiment involving the titration of an acid and base to find the end-point of the titration in order to determine the molarity of the sulphuric acid. GENERAL BACKGROUND According to Bronsted and Lowry (1923) an acid is defined as a proton (H+) donor, and a base as a proton (H+) acceptor. For example, sulphuric acid, a strong acid, is a good proton donor while sodium hydroxide, a strong alkali (soluble base) contains the hydroxide ion (OH-) which is a strong proton acceptor. The alkali which produces this OH- ion will neutralize acids by the reaction: H+(aq) + OH-(aq) --> H2O(l) This reaction is common to all neutralization reactions between acids and alkalis in aqueous solution. It should be noted that in aqueous solutions the H+ ions exist in their hydrated forms H+(aq). The most accurate method of measurement is to run the acid into the alkali from a burette. This is known as neutralization by titration. Titration is a technique used to find the concentration flask. ...read more.


CONTROLLED VARIABLES * The volume of sodium hydroxide in the conical flask was kept constant at a volume of 25cm3 * The molarity of sodium hydroxide used was kept constant at a value of 0.1mol/dm3. * The number of drops of phenolphthalein indicator that was added in the conical flask was kept constant at 3-4 drops. APPARATUSES AND CHEMICALS USED * 2 beakers of 250ml each * 1 pipette of 25ml with pump * 1 burette of 50ml * 1 metal retort stand * 1 white tile * 1 conical flask of 250ml * 0.1M of Sodium Hydroxide ( NaOH ) * Unknown molarity of Sulphuric acid ( H2SO4 ) * Phenolphthalein indicator METHOD * First, I rinsed out the burette with a little distilled water followed by a little distilled water followed by a little dilute sulphuric acid. Then I filled the burette with dilute sulphuric acid and recorded the initial burette reading in a suitable results table. * Then I rinsed out the pipette with some 0.1M sodium hydroxide and then carefully transferred 25cm3 of the NaOH solution to a conical flask * Then I added 3-4 drops of phenolphthalein solution to the flask. ...read more.


= 0.1 M x 0.025 dm3 = 0.0025 moles No. of moles of Sulphuric acid = 0.5 x No. of moles of NaOH neutralized = 0.5 x 0.0025 = 0.00125 moles Concentration of Sulphuric acid = No. of moles of H2SO4 Volume of H2SO4 (dm3) = 0.00125 0.0239 = 0.052M CONCLUSION After conducting the above the experiment carefully and systematically I conclude that the concentration of sulphuric acid that was used in the experiment is 0.05mol/dm3. I also conclude that from the chemical equation the molar ratio of sulphuric acid to sodium hydroxide is 1: 2. . EVALUATION The sources of error that was present when doing the experiment was parallax error. The measurement of the liquid was supposed to be read from the lower meniscus. The lab should have burettes with a better stopper so as to allow different amount of volumes to pass through. There should be better pumps for sucking the liquid through the pipette. The method used here in order to perform the titration gave me the concentration of sulphuric acid to be 0.05mol/dm3, hence the method used was effective. ?? ?? ?? ?? Arshad Akber IB1 Page 1 ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Aqueous Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related GCSE Aqueous Chemistry essays

  1. A titration to determine the ratio of moles of Sulfamic acid to Sodium Hydroxide ...

    >Using the small pipette fill drop by drop holding the line at eye level until the bottom of the meniscus just touches the line. >Put the stopper in and holding your thumb over the top of it shake until all of the solid dissolves and a clear liquid is formed.

  2. Titration I will neutralize the sulphuric acid with a base, which will be Sodium ...

    (0.005grams X 100) / 2.65grams I divide by 2.65 grams because this is the mass of the sodium carbonate I weighed in the balance. The answer is 0.189% (to 3 decimal places) > A volumetric flask that has a capacity of 250cm3 has an error of 0.2cm3 so the percentage error is...(0.2cm3 X 100)

  1. To carry out a titration between a strong acid and a weak alkali, to ...

    My results are quite reliable because I repeated them many times, and three of the results are within 0.1ml of each other. The concentration of the sodium carbonate solution was accurate because I used distilled water to wash all of the powder from the watch glass into the beaker, and

  2. Titrating Sodium hydroxide with an unknown molarity, against hydrochloric acid to find its' molarity.

    0.05moldm-3 + 0.15moldm-3 = 0.10moldm-3 2 good P11 a and the calculation part is P11b Therefore, I need make up a standard solution of the sodium carbonate solution with a concentration of 0.10moldm-3. I will need to make up this solution with the appropriate concentration of sodium carbonate solution, so

  1. Determine the concentration of sulphuric acid by acid-base titration.

    The solution consists of salt and water. In order to able to recognize the end-point of reaction I need to add a suitable indicator. Different indicators are suitable for different combination of strong acid and weak acids and alkalis as follows: Methyl orange: is used as the indicator for a titration between a strong acid and a weak alkali.

  2. How to find the accurate concentration of the Sulphuric Acid.

    In this case, transport immediately to hospital. -Although, with using between 0.05M and 0.15 of sulphuric acid: -Eye protection should be worn -The room should be adequately ventilated. -Avoid inhalation -Take care pouring solutions; hand protection should be worn if necessary.

  1. Find the accurate concentration of a solution of sulphuric acid acid of which concentration ...

    I will label the flask as "Na2CO3 solution" leaving a space for the concentration to be filled in after I have calculated it. I will set the flask aside for titration. RESULTS AND CALCULATIONS: I will record the data from the experiment in the table below: Molar mass of Na2CO3,

  2. Produce two different metal salts (NaHSO4 and Na2SO4) through an application of specific stoichiometric ...

    V = 0.009349 dm3 ? 0.05 % V2(H2SO4) = 9.349 cm3 ? 0.05 % This is the volume of sulfuric acid required to induce the reaction in (II), producing Na2SO4, it will result in the presence of half the number of mole NaOH in H2SO4.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work