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

test for anions present in various salts.

Extracts from this document...

Introduction

CHEMICAL TESTING FOR ANIONS INTRODUCTION; In this investigation we are going to test for anions present in various salts. Such as we have known, the charged particles are called ions. Positive ions are called cations because they travel towards the cathode, such as: aluminum, ammonium, calcium, copper, iron (II), iron (III); Negative ions are called anions because they travel towards the anode, such as: carbonate, chloride, iodide, nitrate, sulphate. Anions - the Negative ions are called anions because they travel towards the anode. Sulphate ions and nitrate ions are very difficult to discharge. When solutions of sulphates and nitrates are electrolyzed, hydroxide ions are discharged instead, and oxygen is evolved.Cations are the charged particles that contain positive ions and anion are the charged particles that contain negative ions. In this experiment, we are going to use the tests of anions of various metals slats Potassium chloride, Iron chloride, Sodium sulphate Calcium carbonate and Lead carbonate. AIM - To identify anions present in various salts by chemical testing. APPARATUS: * Spatula * Test tubes * Test tube racks * Distilled water * Pipette * Hydrochloric acid * Barium chloride * Silver nitrate solution * Calcium carbonate * Lead carbonate * Potassium chloride * ...read more.

Middle

A precipitate is formed no Dissolved with the solution Iron chloride FeCL It dissolved did not fizz White precipitate No No reaction Sodium sulphate no no Bubbles formed. It Dissolved White precipitate formed Calcium carbonate Cloudy white precipitate White precipitate Bubbles, white precipitate White precipitate Lead carbonate Fizzed White precipitate fizz White precipitate Tap water No fizz White precipitate No fizz No reaction CONCLUSION From the result I can inform that - The salts that gave white precipitate when the acids were inserted (silver nitrate and nitric acid) there were the metal chlorides and carbonates. The sodium sulphate reacting with hydrochloric acid and barium chloride produced a white precipitate, informing us that there are negative ions present in this salt. The lead carbonate reacted with nitric acid and hydrochloric acid producing bubbles which indicates that a gas was given off. When the salts were added to silver nitrate they all generally produced precipitates informing that they were insoluble suspensions. * From my results I discovered that when the chlorides, both metals potassium chloride and iron chloride were inserted in the solution of nitric acid followed by a few drops of silver nitrate a precipitate was formed. ...read more.

Conclusion

further more if any salt or test was carried out to identify the anions present , if hydrochloric acid or nitric acid were inserted into it and the solution formed bubbles/fizzed, then the negative ion present here will be carbonate. Thus the salt will then have a carbonate anion present in it. When carrying out experiments to see which negative ion is present, if the mixture fizzes when nitric acid or hydrochloric acid is inserted then you can automatically identify it has a carbonate ion present. EVALUATION In this experiment I have achieved my aim in identifying anions present in several salts. My experiment could have improved if I had followed the procedure much better. I had difficulty in this experiment in realising the reactions taking place in the test tubes I overcame this problem by focusing carefully and consulting with my partner in the reactions occurring. I have learnt that when an atom absorbs light or when an atom bonds an electron can be gained or lost and what is left is an ion. If the ion gains an electron it has become a negative ion and if it looses an ion it becomes a positive ion. This is because the balance of the electrons protons is distributed. ...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. To find out the 5 solutions by testing out the cations and anions.

    * HNO3 is a kind of strong acid, though it has been diluted, but we still have to be careful when we are using it. *Always clean up the lab and all apparatus after use, and dispose of substances according to proper disposal methods.

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

    Anomalies and Improvements In the raw data, some of the results stand out. These were in the 6mg/l, 0.6 mg/l, and 0mg/l copper sulphate concentrations, and one test had other problems: Mass of copper sulphate solution (mg/l) Sample Number Result Average number seeds germinated for this concentration 6 6 2

  1. Production of Epsom salts

    It weighed 0.539g. 3. I added the magnesium to the acid and waited for it to react. There was some magnesium left at the end of the experiment. 4. I poured the liquid into an evaporating basin 5. I then heated the evaporating basin containing the solution to remove half

  2. AIMIdentify anions present in various salts by chemicals testing

    Danger of cumulative effects. Tap water Don't spill it on chemicals. Important = If you spill any chemicals on your skin and eyes quickly wash it for it for 10 min and if you can still feel it keep it like that until you don't feel anything.

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

    Three values within 0.1 cm3 of each other need to recorded in this experiment, as an average titre needs to be obtained. If points within 0.1 cm3 of each other are used the average results will be more accurate. This will also ensure that any random results are noted and

  2. Comparing the solubility's of copper sulphate, sodium chloride and potassium nitrate.

    Branching - This factor only applies to organic compounds. The amount of carbon branching will increase solubility because more branching will reduce the size of the molecule, making it easier to solvate. Chemicals The chemicals I will be using will be: 1.

  1. Investigating for Cations and Anions.

    * I added some Artificial Silver Nitrate solution. * A white precipitate appeared that indicated that there was Cl present. * For the last test-tube, I put some Copper Sulphate solution into the test-tube. * I then added Artificial Barium Chloride solution.

  2. Precipitation of Salts & Identification of Unknown Solutions

    However, according to the solubility rules, seventeen of these twenty four combinations were meant to produce precipitates. All salts containing chloride anions are soluble in an aqueous solution with the exception of Ag+, Hg+ and Pb2+.

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