• 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

# To find the accurate concentration of sulphuric acid, by making up a standard solution, sodium carbonate, to titrate against the acid. The titration is therefore an acid-base reaction.

Extracts from this document...

Introduction

Finding the Accurate Concentration of Acid in a Solution. Aim: To find the accurate concentration of sulphuric acid, by making up a standard solution, sodium carbonate, to titrate against the acid. The titration is therefore an acid-base reaction. Na2CO3 + H2SO4 --> H20 + CO2 + Na2SO4 Apparatus: 250cm3 volumetric flask and its stopper Funnel Glass rod 1 Bottle of distilled water Weighing bottle 100cm3 beaker Spatula Top pan balance Analytical Balance Making a Standard Solution As I am only provided with anhydrous sodium carbonate, my idea is to find how much of this solid is needed to make up the standard solution for the titration. To do this I must determine the approximate number of moles of the alkaline I want. As the concentration of acid is approximately between, 0.05-0.15 mol/dm3, it is best if the concentration of the alkaline is approximately the same, as the ratio of sulphuric acid to sodium carbonate is 1:1. This allows equal volumes to be used. I have decided to take the mean value of 0.05-0.15 for the number of moles for the alkaline I want. Therefore: (0.05+0.15) / 2 = 0.1mol/dm3 Now that I know the number of moles, I can substitute the known into a formula and find the mass of anhydrous sodium carbonate needed to make up s standard solution. ...read more.

Middle

Make sure to run the solution and distilled water though the jet too. 2 Set up a clamp stand and place a white tile firmly by the leg 3 Close the tap on the burette and pour the acid through carefully. Fill the burette up to zero. Place a small, clean beaker under the burette and run the acid though into the beaker. This fills the jet and check to see if there are any air bubbles present. (The acid in the beaker can be poured into the burette again) 4 Connect burette to the clamp stand and read value off to 2 d. p using a magnifying glass. This is you initial reading. 5 Rinse a pipette with distilled water and the solution to be pipette. Connect the pipette to its pipette fuller by holding the ends together and pushing firmly. Then pipette out 25cm3(up to the mark present on the pipette itself) of standard solution (the alkaline) and bring the conical flask to the pipette and fill by pressing on the lever. 6 Wash out the sides of the conical flask by using distilled water, so all content are being titrated. Do this periodically for more accurate results. ...read more.

Conclusion

VOLUMETRIC FLASK- the best equipment for best dilution. WHITE TILE-ensures the reliability as you can see if any drop are present on it, informing toy that the experiment has lost some atoms and ions and therefore not accurate as it could be. Also when titration begins the colour can be easily contrasted against the white tile, indicating when to stop titrating. This eliminates the possibility of over titrating. SUFFIENT INDICATOR-too much indicator could mean the titration process needs to titrate the indicator as well as the acid. MENISCUS: a meniscus is the shape that the solution makes and is quite thick. Always be consistent and read from the bottom of the meniscus to the mark, as represented on the diagram below. REPEATS- all experiments are independent to each other so neither experiment has an influence the tire. Repeating the experiment till the titres are consistent increases reliability as the answer is evidently within range. A ROUGH TITRATION-the rough allows over titration to be made a, eliminating the possibility of over titration at the later stage. RISK ASSESMENT Sulphuric acid (H2SO4) - Between the moles 0.5-1.5, it is known irritant to the eyes and the skin. Wear goggles and gloves when handling. (ii) Anhydrous Sodium Carbonate (Na2S04) - Irritant to eyes. Wear goggles when handling. (iii) As several glass equipment is going to be used carefully handle them. Clear any spills. ...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. ## Titration To Determine the Concentration of a Solution of Sulphuric Acid.

The ph of the indicators changes over 2 units. Or using a different concentration of sodium hydroxide. Discussion The end point might be different due to human error, they might have added a couple of extra drops or they might not have added enough drops.

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

I can use the equation below to work out the mass of Iron (II) present in the 100 grams of Spinach Oleracea. Mass = Moles X Ar The Ar of Iron (II) is 55.9 and therefore: Mass = 0.012127766 mol dm-3 X 55.9 Mass = 0.677942119 mg This answer tells me that there are 0.678 mg's of Iron (II)

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

Significant attention is paid to the proper technique for reading a meniscus While reading the level of burette, the viewer's eyes must be at the level of the graduation to prevent parallax error level Remember to wash the reaction beaker, pipette with distilled water before each titration.

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

Titration Curves I think that a titration curve for this reaction: H2SO4(aq) + Na2CO3(aq) � Na2SO4 (aq) + H2O(l) + CO2(g) is going to resemble letter S turned 900 anti-clockwise. The first part of the curve is going to be sloping downwards, because there will be a weak acid present in the solution.

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

bottle with distilled water and transfer the washings each time to the 100cm3. Make sure all of the solid goes into the beaker because if it doesn't it will affect the accuracy of the experiment. > Pour a further 25cm3 of distilled water into the beaker > Stir the distilled

2. ## Experiment to determine the concentration of sulphuric acid

Safety Safety goggles will be worn to protect eyes from any splashes of irritants. Gloves will be used to protect hands from any contact with corrosive, irritant or toxic substances. Equipment 1g Magnesium carbonate Sulphuric acid ( 10 mol dm-� sulphuric acid.) Distilled water Divided flask Rubber delivery tube Pipette.

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

The temperature will also be kept the same as the titrations will be carried out on the same day. If the temperature is increased, the liquid will expand and it will make the test inaccurate. Method: - 1. Wash out the watch glass, graduated volumetric flask and the 250cm3 beaker with distilled water to get rid of any contamination.

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

This is an acid-base titration therefore the chemical reaction I am expecting sulphuric acid to donate H, which will be accepted by the sodium carbonate. The end-point of this particular titration is when all the alkali has been neutralized and neither excess acid nor excess alkali is present in the solution.

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