Part of The Student Room Group

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

sulphuric acid is dibasic

Extracts from this document...

Introduction

Demonstrating that sulphuric is dibasic: Aim: The aim of my plan is to demonstrate that sulphuric acid is dibasic. Introduction: Acid is a substance that reacts with a base to form a salt and water similarly a base is a substance that reacts with an acid to form a salt and water. "Lewis (a scientist) states that an acid is a compound that accepts a pair of electrons from a base and a base is a molecule or an ion that donates a pair of electrons to an acid. Acids taste sour and are corrosive and bases are slippery". ? Acid + Base � Salt + Water Acid + Metal � Metal Salt + Hydrogen gas Prediction: I predict that sulphuric acid, H2SO4 is dibasic because it forms two hydrogen (H+) ions in an aqueous solution. It is the molecule of sulphuric acid which changes to sulphate ions (SO42-) and hydrogen ions (H+) when dissolved in water. However, hydrochloric acid is monobasic as it only forms one hydrogen (H+) ion in an aqueous solution. To prove this, I am going to carry out two different experiments that involve a titration and collection of a gas. I assume that it should require me half a volume of sulphuric acid to neutralise sodium hydroxide, NaOH than HCl in titration. ...read more.

Middle

11. If the colour of solution is going lighter, twist the tap so that only drops of acid flow into the conical flask. 12. Keep adding the drops until one last drop changes the colour of the solution to colourless. 13. Close the tap with that last drop and record the reading of the acid that was used in a table. 14. Repeat the same procedure 3 more times and find the average volume of acid used. 15. Carry out exactly the same procedure from step 1 to 13 but using HCl instead of H2SO4. 16. See the figure below for how to set up the apparatus. Pipette Solution Sodium hydroxide (NaOH) 25cm3 moldm-3 Burette Solution Acids (H2SO4/HCl) 25cm3 1.00moldm-3 Indicator phenolphthalein Burette readings Trial 1 2 3 4 Final 25.90 25.80 25.60 25.40 25.40 Initial 0 0 0 0 0 Volume used (titre)/ cm3 25.90 25.80 25.60 25.40 25.40 Mean titre/ cm3 (25.80+25.60+25.40+25.40)/4 =25.60 Since I have got two reading similar, I can stop titration. Titration: Equations H2SO4 (aq) + 2NaOH (aq) �Na2 SO4 (aq) + 2H2O (l) Concentration (H2SO4) =1.00moldm-3 Volume (H2SO4) = 25.60 cm3 no. of moles of (H2SO4) = 1.00 x (25.60/1000) = 0.025mol no. of moles of (NaOH) = 0.025 x 2 = 0.050 mol From this equation we can see that molar ratio of H2SO4: NaOH is 1:2.So, 1 mole of H2SO4 requires two moles of NaOH and produces two moles of water in titration. ...read more.

Conclusion

1/ 24dm3 =4.00x10-3 /x x = 0.096 dm3 x = 96.00cm3 Volume of H2 = 96.00cm3 Mg(S) + 2HCl (aq) � MgCl2 (aq) + H2 (g) Concentration of (HCl) = 1.00moldm-3 Volume of (HCl) = 4.00 cm3 No. of moles of ( HCl) = 1.00 x (4.00/1000) = 4.00x10-3 mole No. of moles of (H2) = 4.00x10-3 /2 = 2.00x10-3mole Since 1 mole of a gas occupies 24dm3 of space. Therefore, 1mole: 24dm3= 4.00x10-3 moles: x dm3 (where x is the volume of hydrogen gas produced.) 1/ 24dm3 =2.00x10-3 /x x = 0.048 dm3 x = 48.00cm3 Volume of H2 = 48.00cm3 1 mole of H2SO4 gives 96.00cm3of H2 gas where as, 1 mole of HCl produces only half a mole of H2 gas (48.00cm3). Consequently, I have proven that H2SO4 is dibasic. Analysis: 1. Titration gives an accurate reading because the apparatus used such as pipette and burette are accurately calibrated and so can measure up to 0.10 cm3 than the collection of gas using a measuring cylinder. 2. Titration is more reliable as it is repeated several times and an average volume of titres is found. 3. Since I am using an indicator in titration, I can determine the end point whereas there isn't an end point for the gas evolved. 4. The results of the gas collection may be inaccurate because some of the gas may have escaped while the metal is added into the acid. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our AS and A Level Inorganic Chemistry section.

Found what you're looking for?

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

or


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 AS and A Level Inorganic Chemistry essays

  1. Peer reviewed

    Determining the concentration of acid in a given solution

    5 star(s)

    even concentration you throughout If the volumetric flask wasn't tipped then the concentration of the sodium carbonate would be higher at the bottom of the flask. When the solution is taken out of the volumetric flask, the pipette usually reaches to the bottom of volumetric flask.

  2. Peer reviewed

    Deducing the quantity of acid in a solution

    5 star(s)

    * Sodium Carbonate We used solution of sodium carbonate both as a solution and as powder. Its concentration is 0.1 M, so it can not be labelled as irritant because only solutions equal to or stronger than 1.8 M are irritant.

  1. effects Concentration and Temperature on the Rate of Reaction

    Alcohol-resistant foam, powder, water spray, carbon dioxide. Explosion Above 79°C explosive vapour/air mixtures may be formed. Above 79°C use a closed system, ventilation. In case of fire: keep drums etc. cool by spraying with water. Inhalation Sore throat. Burning sensation. Cough. Dizziness. Headache. Nausea. Vomiting. Shortness of breath.

  2. Titration Coursework

    I will pour the sulphuric acid using a funnel. I will then burette with sulphuric acid as long as it's on zero or below that. I will then run the burette tap until the sulphuric acid comes to the bottom of the burette. I will then take the initial reading from the burette.

  1. Aim To study the effect of concentration of iodide ion ...

    Preparation of chemical solutions 1. To prepare 1000 cm3 of standard potassium iodide KI 1.0 mol dm-3 solution, 166.000g of KI is needed. However, to prevent wastage, only 83.000g (to 3 d.p) was instead used to produce 500 cm3 of standard potassium iodide KI 1.0 mol dm-3 solution.

  2. Finding Out how much Acid there is in a Solution

    Method - Checking the Indicator Colour Change I need to check the exact colour which the indictor turns my acid and alkali solutions so I can be sure when the titration is finished and the substance is neutralised. I will pour a little of the acid and the sodium carbonate

  1. The Effects of Strong and Weak Acids on the Order of a Reaction.

    Activation energy number becoming positive sure to the negative signs in the equation. Working out the Rate of a Reaction The rate of a reaction can be determined by doing the 'Rate Equation'. This is an equation which has gained by doing experiments and finding out the ratios between the concentrations of the substances.

  2. The Chemistry oh Phosphorous

    Red phosphorus is also used by the military, however because it is less reactive and does not ignite spontaneously, its usage is limited to smoke-screening and less for incendiary weapons. However this is not its main use. Originally matches were made by coating the match head in a mixture containing

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