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

Testing Nickel (II) Sulphate, Iron (III) Chloride, Potassium Sulphate

Extracts from this document...

Introduction

1. Nickel (II) Sulphate (NiSO4) Iron (III) Chloride (FeCl3) Potassium Sulphate (K2SO4) 1. Describe the bonding present in the molecule. The bonding present in all three molecules is ?Ionic bonding?. This type of bonding occurs when a positively charged (cation) and a negatively charged (anion) ion are attracted. It typically occurs between a metal and a non-metal. The bond?s structure is strong and rigid. Nickel (II) Sulphate: Nickel (II) (Ni+2) is the cation, whereas Sulphate (SO4-2) is the polyatomic anion. Iron (III) Chloride: Iron (III) (Fe+3) is the cation, whereas Chloride (Cl-1) is the anion. Potassium Sulphate: Potassium (K+), whereas Sulphate (SO4-2) is the polyatomic anion. 1. Explain how the cation tests work, use equations. -Appearance: The elements of group 1, 2 and 3 appear to be white whereas, transition metals appear coloured. Potassium is a group 1 element; therefore, its colour is white. ...read more.

Middle

Iron (III) gave the flame colour bright yellow; this could be due to contamination, normally no specific colour is observed when a flame test is done for Iron (III). Its electron configuration is: 1s2 2s2 2p6 3s2 3p6 4s1 3d5; as it is seen, the 4s and 3d orbitals aren?t fully filled. This effects the movement of the electrons when it gains energy and no specific colour is observed. Nickel (II) gave the flame colour blue green. Normally it does not give a specific flame colour. Its electron configuration is: 1s2 2s2 2p6 3s2 3p6 4s1 3d8; as it is seen, the 4s and 3d orbitals aren?t fully filled. This effects the movement of the electrons when it gains energy and no specific colour is observed. -Precipitation Tests: The precipitation tests which take place could either be single replacement reactions or double placement reactions. ...read more.

Conclusion

In the Sodium carbonate test; Nickel (II) Sulphate formed blue precipitation with Sodium carbonate, normally Nickel forms green precipitation: Iron (III) Chloride formed green precipitation with Sodium carbonate, normally Iron (III) forms brown precipitation: Potassium formed white precipitation with sodium carbonate. 1. Explain how the anion tests work. In the Barium Chloride test; When barium chloride was added to Nickel (II) sulphate white precipitation was formed and when hydrochloric acid was added the precipitation became insoluble: When barium chloride was added to Iron (III) sulphate no precipitation was observed, the solution was colourless and when hydrochloric acid was added there was still no difference, the solution was still colourless; this indicates that the reaction was unsuccessful. Potassium Sulphate formed white precipitation and when hydrochloric acid was added the precipitation became insoluble: In the Silver nitrate test; Iron (III) chloride formed white precipitation when silver nitrate was added: Both the solutions Nickel (II) Sulphate and Potassium Sulphate formed colourless solutions, this indicates that the reaction was unsuccessful. ...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 Inorganic 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 AS and A Level Inorganic Chemistry essays

  1. Peer reviewed

    Determining the concentration of acid in a given solution

    5 star(s)

    but the percentage error can be reduced by increasing the volume used in the burette. The burette has to be read before and after titrating the solution so that the titre can be calculated. I made sure that I filled up by burette after each titre so that I wouldn't

  2. Peer reviewed

    Deducing the quantity of acid in a solution

    5 star(s)

    Sometimes the indicator changes colour when the H2SO4 hits the solution in the flask, but then the colour change disappears upon when swirling, so swirling the flask constantly will ensure us that the reaction has occurred. That is why swirling the flask all the time is a very important step.

  1. Determination of the formula of hydrated Iron (II) Sulphate crystals (FeSO4xH2O)

    Empirical formula Mr of FeSO4xH2O: Mr = mass Mr = 3.02 = 277 number of moles 1.09 x 10-2 Mr of FeSO4 = 56 + 32 + (16 x 4) = 152 Mr of H2O = (1 x 2) + 16 = 18 Value of x 277 - 152 =

  2. determination of the percentage of oxalate in iron (II) oxalate by redox titration

    Therefore redox indicator which gives a sharp end-point to the titration is unnecessary in this titration. 2) In this titration, no brown precipitate should appear in the conical flask. If it does, what would you do? Explain why you should do so.

  1. The preparation, analysis, and reactions of an ethanedioate complex of iron

    Then few more drops of tin(II) chloride were added . Once the solution was cooled to room temperature, one portion 10cm3 of mercury(II) chloride solution was added quickly. 10cm3 of 40% phosphoric acid and 10 drops of barium diphenylamine sulphonate indicator solution were added to the reduced solution.

  2. Aim To study the effect of concentration of iodide ion ...

    A graph of rate of reaction against concentration was plotted after an error analysis was conducted. A best fit line was drawn to connect the plots. Data Collection OBSERVATION All solutions in test tube A (KI 1.0 mol dm-3), B (Na2S2O8 0.04 mol dm-3), and C (Na2S2O3 0.05 mol dm-3)

  1. The Effects of Strong and Weak Acids on the Order of a Reaction.

    y = mx + c This is where, y = ln (rate), m (the gradient) = -EA/R, x = 1/T and c = ln (A) Once the gradient of the graph has been determined, one can then begin to substitute the numbers into the equation: -Ea = -gradient/8.31; the overall

  2. Anion Test- Testing for negative ions in solutions.. Applied science unit 3 (AQA)

    Any contact to the eyes can cause serious long term damage such as low eyesight. To protect your eyes you should first keep your goggles on at all times, also you should handle the acid with care so that you don?t spill on your skin or anyone else.

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