• 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

# Report on Preparing a sample of fertiliser, in titration

Extracts from this document...

Introduction

﻿Preparing a sample of fertiliser The Equipment used in this experiment was: 1. Eye Protection. - 25ml Graduated pipette and filler. 2. Burette and Stand. - Litmus indicator. 3. Evaporating Basin. - Tripod. 4. Balance (to 0.0g). - Ammonium Hydroxide. 5. 250ml Conical Flask. - Sulphuric Acid. 6. Clay pipe triangle. - Bunsen Burner. 7. White tile. Before starting this experiment I weighed the Dish, this came to 45.9g. Rough 1 2 3 Average Final Burette Reading (cm3) 22.65 22.15 22.2 22.15 22.16 Initial Burette Reading (cm3) 0 0 0 0 0 Titre (cm3) 22.65 22.15 22.2 22.15 22.16 The calculation to find the average was Final Burette Reading 1 + Final Burette Reading 2 + Final Burette Reading 3 = Average 3 22.5 +22.2 + 22.15 = 22.16 3 Carefully we drew 25ml of Ammonium Hydroxide using a glass pipette. ...read more.

Middle

Turning the nozzle slowly on the burette so it was horizontal we allowed the acid to empty into the conical flask with the Ammonia in it, one drop at a time, until the Ammonia solution and Acid, mixed and turned an almost pinkish colour. Recording how much of the Sulphuric Acid was used, we then repeated this 3 times till they were all 0.1cm3 difference between them, we the calculated the average. We repeated the procedure again, this time without the litmus indicator, adding the average volume of acid, as accurately as possible. The reason we did this, was so that there wasn?t any other chemicals mixed into the solution, when we heated the ammonium sulphate later. Pouring the solution, into the pre-weighed evaporating basin. ...read more.

Conclusion

2.85 Solutions mass 22.16 Mass lost 19.31 After several days, we checked our solution, and found that all the liquid had been evaporated, and crystals, were what remained. We measured the crystals, and recorded all the information in the table above. The reaction that had taken place was: Ammonium Hydroxide + Sulphuric Acid Ammonium Sulphate 2NH4OH + H2SO4 (NH4)2SO4 + 2H2O H2SO4 NH4OH (NH4)2SO4 Volume (in dm3) 0.02216 0.025 Concentration 1M 2M Moles = 1 X 0.02216 = 0.02216 mol = 2 X 0.025 = 0.05 mol Ratio (from balanced equation) 1 2 1 Moles = Mass of Crystals Mr (NH4)2 SO4 N X 2 = 14 X 2 = 28 H X 8 = 1 X 8 = 8 S X 1 =32.1 X 1 = 32.1 O X 4 = 16 X 4 = 64 132.1 Moles = 2.85 = 0.02157456 132.1 ...read more.

The above preview is unformatted text

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

1. ## Determination of the formula of Hydrated Iron (II) Sulphate crystals

Again, this would mean that the weight calculated for the loss of water was not completely accurate as not all the water was driven off, making the calculated mass of water lower than it really was. Following this procedural error, there is the issue around the shape of the crucible as it was quite deep.

2. ## The aim of this experiment is to produce Aspirin. This is an estrification in ...

Burette (class B) All burettes read to 2 decimal places in which the second figure is either 0 or 5. One drop from a burette has a volume approximately 0.05 cm3. Therefore the precision error is 0.05. Pipette (class B)

1. ## investigating the amount of ascorbic acid present in fruit

= 2.80 x 10-3 moles 1000 To work out the number of moles of NBS solution used on the lime sample I multiplied 0.1 (concentration of NBS solution that was used) by the average titration for the lime sample which was 28.03cm3.

2. ## Comprehensive and Detailed Chemistry notes

-- Differences in bonding affect the behaviour of each oxide with water define Le Chatelier's principle identify factors which can affect the equilibrium in a reversible reaction TEMPERATURE: -- In enothermic equlibria, an increase in temperature will trigger equilibrium to shift to the right to favor the products -- In

1. ## hydrated copper sulphate

This adds onto the mass and therefore the reliability of the experiment is hindered. This is therefore an error in both measurement and procedure. > The conical flask was constantly being swirled whilst being titrated so that the reaction could happen quicker.

2. ## Finding the concentration of an acid sample

So the indicator I need will have to be near the equivalence point. As we can see above5 the indicator of choice is Methyl Orange6. And as from the above theory the equivalence point is near the endpoint of the indicator.

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