• Join over 1.2 million students every month
• Accelerate your learning by 29%
• Unlimited access from just £6.99 per month
Page
1. 1
1
2. 2
2
3. 3
3
4. 4
4
5. 5
5
6. 6
6

# 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 During the extraction of a metal from its ore, sulphur dioxide is often produced. It is converted into Sulphuric (VI) acid and sold as a useful by-product. I shall be carrying out a titration between sodium carbonate, a weak alkali, and sulphuric acid, a strong acid, to calculate the concentration of the sulphuric acid. The sodium carbonate sample I shall be using is a solid. Solids cannot be titrated successfully, so I will turn it into a solution by adding distilled water to it. The distilled water has no adverse effects on the sodium carbonate. Na2CO3(aq) + H2SO4(aq) Na2SO4(aq) + H2O(l) + CO2(g) Methyl orange is an acid-base indicator, which changes colour according to the hydrogen ion concentration of the solution to which it is added to. It 'indicates' the end point of the acid-base titration, and tests the acidity or alkalinity of the solution. I shall be using methyl orange as the indicator in my titration because, for a titration between a strong acid and a weak alkali, methyl orange works most effectively. HMe H + Me Red colourless Yellow From this titration, I can expect the solution to turn colourless. ...read more.

Middle

The end point of the titration is when you swirl the solution and it stays colourless. Close the tap. 18. Record the final burette reading. The difference between the first burette reading and the final burette reading is the volume of solution you have run out into the flask. This is your titre reading. 19. Record your results and calculate the average titre: Average titre = Total titre reading (cm�) (cm�) Number of titrations 20. Repeat this experiment as many times as you need until you get 3 results within 0.1 of each other. N.B All the apparatus should be thoroughly cleaned between each titration. Risk Assessment Safety glasses must be worn to protect the eyes from splash-back of any solution or sulphuric acid. In addition, a lab coat should be worn to protect clothes, hair should be tied back, broken skin should be covered with plasters and stools need to be safely tucked under desks. All the apparatus will be placed in the centre of the desk so that nothing is in danger of falling off the desk and breaking. If any equipment does break, it should be placed into the broken glass bin with a dustpan and brush, and the teacher should be notified. ...read more.

Conclusion

So the solution passed its colourless state and turned slightly purple or blue. This may have caused my titres to be larger. Also, the pipette may not have always fully emptied. Overall however, I think my results are relatively accurate and reliable, because I cleaned the equipment after each titration, I took measurements reading from the bottom of the meniscus, I used calibrated equipment, and the same batch of sulphuric acid and Na2CO3 solution every time. To improve my procedure I think I could carry out two rough titrations instead of the one. In this way, it would allow me to expect a value between the two. I would also label a bottle of methyl orange indicator and use that each time so that the concentration of it cannot vary, ensuring the titration results are more accurate. When emptying the contents of the pipette into the conical flask, I would allow the pipette to fully drain until the last drop by touching the side of the flask with the pipette. This ensures the full 25 cm� quantity is used each time. Before a titration I would ensure I shake the volumetric flask thoroughly so that the solution is of even concentration, making my experiment reliable and accurate. Nikki Wadhera 12T AS Chemistry Coursework - 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

# Related GCSE Aqueous Chemistry essays

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

and the Iron (s) strip in the boiling tube that contains Iron (II) Ammonium Sulphate (aq). 8) Take a piece strip of filter paper and soak it in saturated Potassium Nitrate (V) (aq), use this as the salt (ion) bridge to connect the solutions in the two boiling tubes. 9)

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

First of all I noticed that while pouring the alkali solution into the volumetric flask, some residue of sodium carbonate remained behind. This was than washed out with non-ionised water into the flask and once the meniscus line has been reached, no more sodium carbonate could have been poured in, this still leaving some residue in the beaker.

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

Use a pipette filler and pipette to transfer 25cm3 of the sodium carbonate solution from the 250cm3 graduated volumetric flask to the 250cm3 conical flask. Hold the pipette at the top, because if you hold the bulb, it heats it up and may cause the liquid to expand, leading to inaccuracies.

2. ## Investigating the Effects of Increasing Copper Sulphate Solution Concentrations on the Germination of Cress ...

This meant that the wholes were very big, and so evaporation could have occurred. But this should not really have affected the investigation, because all of the pots had cling film pierced with the same size stirring rod, the same number of times.

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

really suitable therefore a ph meter, a conductivity meter or temperature probe has to be used. Hence sulphuric acid is a strong acid and sodium carbonate is a weak alkali, methyl orange is the most suitable indicator for this experiment.

2. ## The Use of Volumetric Flask, Burette and Pipette in Determining the Concentration of NaOH ...

Base The common (Arrhenius) definition of a base is a chemical compound that either donates hydroxide ions or absorbs hydrogen ions when dissolved in water. Bases and acids are referred to as opposites because the effect of an acid is to increase the hydronium ion concentration in water, whereas bases reduce this concentration.

1. ## Chemistry Practical: Finding the water content of Na2 CO3 .xH2O by Titration

Number of moles of sodium carbonate in 25 cm-3=2.89x10-3/2=1.44x10 -3 3. Number of moles of sodium carbonate in 250 cm-3=1.44x10 -2 4. Mass of anhydrous sodium carbonate Na2 CO3 in 250 cm-3=1.44x10 -2 x 106=1.53g 5. Mass of water in the original hydrated crystals=3.99-1.53=2.46g Empirical Formula Na2 CO3 H2O Mass

2. ## Find out how much acid there is in a solution

the glass rod with distilled water above the funnel to wash away any leftover Sodium Carbonate. Furthermore, add more distilled water into the volumetric flask until reaching the graduation mark. Put the plastic or rubber bung on top and make sure its securely fastened to prevent any spillage.

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