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

Finding out How much Acid there is in a Solution.

Extracts from this document...

Introduction

Finding out How much Acid there is in a Solution Aim The aim of this investigative experiment is to discover the accurate concentration of sulphuric acid (H2SO4), which is found in a solution. The concentration is thought to be between 0.05 mol dm�3 and 0.15 mol dm�3. I have been given access to anhydrous potassium carbonate (K2CO3) and a range of indicators. Plan In order to obtain the concentration of the acid in the solution I have to titre the known solution of potassium carbonate with the unknown sulphuric acid. The indicator I will be using to indicate when the reaction is fully completed is methyl orange. This is because I am using a strong acid and a weak alkali and methyl orange is the most appropriate indicator for this type of acid-alkali titration. To begin with I will have to prepare a standard solution of potassium carbonate that will be used in the titration with sulphuric acid. The potassium carbonate is of known strength and volume in contrast with the unknown concentration of sulphuric acid. This is the equation for the titration: H2SO4 (aq) ...read more.

Middle

� MAKE SURE YOU HAVE YOUR SAFETY GLASSES ON DURING THE WHOLE EXPERIMENT Potassium carbonate Although the solution I am using is very dilute I should still be aware that contact with eyes, skin and clothing must be avoided. As such I am to be wearing goggles and a lab coat. Also any slippages would cause the area to become slippery and dangerous, if they are not cleaned up quickly. Methyl orange The same precautions apply for this as did with the potassium carbonate. Sulphuric Acid It is very corrosive. If it is swallowed, wash out mouth and give one or two glasses of water. Don't induce vomiting. Seek medical advice as soon as possible. If it is splashed into the eye flood the eye with gently running tap water for 10 minutes. Seek medical advice. If it is spilt on clothes or skin remove the clothes quickly and wipe as much liquid as possible away with a dry clothe before drenching the area with lots of water. If a large area of skin was affected or blistering seek medical advice. If it is spilt in the laboratory, wear eye protection and gloves and cover with mineral absorbent and scoop into a bucket. ...read more.

Conclusion

� The burette and pipette may not have been thoroughly washed out with the solutions used. � The conical flask may not have been thoroughly washed out with distilled water between titres. � The end point may not be accurate if the solution from the burette is not added drop by drop with continuous swirling. � Too much or too little indicator may have been added each time It is not possible to place a value on the effect of human error on the reliability and accuracy of results. However, further repetition of the experiment would limit the effect human error has on results. Improvements to the investigation would be mainly aiming to reduce the human error. This could be done by using equipment that displays values and measurements digitally, or detect the colour change more accurately. Overall I do not believe my results could have been that inaccurate seeing as my titres were the same. I feel that the procedure allowed me to discover the accurate concentration of the acid to a fairly accurate and reliable degree. Sources: � Chemical Ideas - Salters Advanced Chemistry (2nd Edition). � Chemistry - Ann and Patrick Fullick (2nd Edition). � Hazards in the Chemical Laboratory - Edited by G.D Muir (2nd Edition). � Google Images - Keyword: Titration Tahamtan Pishgharavol Chemistry Coursework: Titration 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. Marked by a teacher

    Enthalpy of Neutralisation.

    3 star(s)

    PROCEDURE. * Set up the apparatus by clamping the burette to the clamp stand. * Pour 50cc of Sodium hydroxide into the burette (1 molar). * Pour 25m of Hcl (200cm3 of 1 molar) into the measuring cylinder (making sure it is dried).

  2. In order to find out the exact concentration of sulphuric acid, I will have ...

    Of course not all errors can be accounted as being human, because air pressure, room temperature, etc might have played a minor part on the outcome of the experiment. Results Accurate Rough 1 2 3 4 Final Reading (cm3) 22.01 21.09 21.22 21.12 21.16 Initial Reading (cm3)

  1. Titration with a primary standard.

    Titration Problem Example: If 20 cm3 of a 0.3 M solution of NaOH is required to neutralize 30.0 cm3 of a sulfuric acid solution, what is the molarity of the acid solution?

  2. How much Iron (II) in 100 grams of Spinach Oleracea?

    Ammonium Sulphate (aq) Aim To find out how accurate an Electrochemical Cell is in determining the concentration of an Iron (II) Ammonium Sulphate (aq) Background Theory Electrochemical cells are the basis of electrical batteries (6). In one half of the cell an oxidation reaction occurs and electrons are produced and

  1. Finding out how much acid there is in a solution.

    * Sulphuric acid * Sodium carbonate solution * Distilled water The quantities of the materials to be used: * 1 x watch glass * 1 x digital scales * 1 x spatula * 2 x 250 cm3 beaker * 1 x glass rod * 1 x 250 cm3 volumetric flask

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

    Let out a bit if it is still above the graduation mark, to make sure the bottom of the meniscus is exactly on the graduation mark and transfer it to the conical flask. As the volume of the pipette is greater than the pipette filler, you will have to keep

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

    I will rinse the beaker three times to make sure all the solution goes into the volumetric flask, each time pouring the solution down the stirring rod to rinse it. 7. I will carefully make up the solution to about 1cm of the mark on the neck of the flask using distilled water.

  2. Findingout how much acid

    A suitable indicator would be methyl orange (pH range 3.1 - 4.4) or methyl red (pH range 4.4 - 6.0) Sulphuric acid, is a strong acid and Sodium Carbonate is a weak base therefore it is now clear that a methyl orange indicator will be used to identify the neutralisation of the Sulphuric acid.

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