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

Finding the percentage of Nickel in an unknown compound.

Extracts from this document...


Finding the percentage of Nickel in an unknown compound. LAB 3 I. Purpose: Finding the percentage of Nickel in an unknown compound. II. Objectives: To separate and weigh nickel from a sample that contains an unknown amount of nickel and to use the mole method to determine the amount of nickel in the unknown sample. III. Background: Analytical chemistry can be simply divided into two areas. Qualitative analysis and quantitative analysis. The two words "qualitative", means to find out if a specific substance is present in a soil sample, and "quantitative" means to determine how much of that substance is in the sample. The analytical chemist has many tools at his disposal, for this quantitative experiment we will be performing a gravimetric analysis to find our how much nickel is in an unknown sample. Gravimetric analysis means to separate the nickel from the sample, and then weigh it. Your instructor will give you a test tube that contains approximately one gram of a compound that contains an unknown amount of nickel compound. You will dissolve a portion of this sample in water. ...read more.


Avoid direct contact with nickel compounds by using plastic gloves. VI. Experimental Procedures: 1. Find the mass of the unknown sample. Prepare your sample. Carefully weigh about 2.0 grams of your unknown nickel compound into a small beaker. Be precise. 2. Dissolve your sample in distilled water. Dissolve the sample in 20-30 mL of distilled water. You may need to heat your beaker slightly in order to dissolve the entire sample. Be careful not to spill any of your samples. 3. Use a clean beaker to get about 25 mL of DMG solution. 4. Add NH4OH and DMG. The nickel/DMG reaction proceeds more quickly and completely if you add a small amount of NH4OH (4-5 drops) to your dissolve nickel solution before you add the DMG. Bring your beaker of dissolved nickel to the lab fume hood and add the NH4OH. The NH4OH is very concentrated so do not spill any on yourself and do not inhale any vapors. 5. Bring the beaker containing the nickel solution and NH4OH back to your lab bench and carefully add the DMG solution a few drops at a time. ...read more.


Add DMG to the liquid in your vacuum flask to see if more NiDMG precipitates out. Re-filter if necessary. 8. Dry with acetone. By now you should have a wet mass of NiDMG sitting on your filter paper. In order to obtain an accurate mass measurement, you must completely dry the NiDMG. Acetone will remove water from the NiDMG, but will not dissolve the NiDMG. Acetone also evaporates very quickly. Turn the vacuum aspirator on and use an eye dropper to add about 25 mL of acetone to the NiDMG on your filter paper; then let the NiDMG dry for five to ten minutes with the aspirator on. The precipitate will turn light pink as it dries. 9. Determine the mass of the precipitate on your filter paper. Weigh your filter, funnel, and precipitate. Subtract the weight of the top of the funnel and filter, and you willl have the weight of the NiDMG you have recovered. 10. Repeat the entire experiment two more times to show that yur results are reproducible. Clean up. By the time you perform this experiment 3 times, you will have flasks and beakers encrusted with sticky, pink, solid NiDMG. Take time to completely clean your glassware and filtering apparatus before you leave the lab. ...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 Classifying Materials 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 Classifying Materials essays

  1. Marked by a teacher

    Identifying an Ionic Compound. Objectives: To learn and test for metal ions ...

    5 star(s)

    if I was testing for Na+, K+, Ca2+, Cu2+ using a nichrome wire with HCL over a Bunsen burner, then colored flames would be produced. To my amazement, many colored flames were produced and sodium had an orange flame, potassium a lilac flame, calcium a brick red flame and copper (II)

  2. Marked by a teacher

    In this CDA I will write about how plastic bags are made, why plastic ...

    Many people do not throw them away, but use them to carry food and items around the house or out. Moreover, there are several people working in the factories that produce these plastic bags, and banning the use of them or reducing them will increase job loss.

  1. Our experiment consisted of two samples of water containing unknown substances, and our objective ...

    Temporary hardness removal: Permanent hardness removal: In each case magnesium or calcium is precipitated and this removes the hardness of the water. Soft water doesn't contain as many minerals as hard water. Also, unlike hard water, soft water doesn't cause limescale to build up in appliances since it doesn't have calcium carbonate dissolved into it.

  2. The role of mass customization and postponement in global logistics

    The major assumption being that markets were homogeneous - everybody had basically the same wants and needs that could be satisfied by a few standard products. Over the past 40 years significant changes have occurred in the business environment - increased pace of technological change, more fashion consciousness, globalisation of

  1. Particulate Nature of Matter

    Gases are random groups of atoms. There are solids where atoms and molecules are really compact. Liquids have them a little more spread out. But gases are really spread out and the atoms and molecules are full of energy, bouncing around constantly.

  2. Specific Heat Lab

    cmetal= (mh2o*(Ti-Te)h2o)/(mmetal*(Ti-Te)metal) - We ignore the specific heat of H2O because no error is present. cmetal= (0 .005* 0.10)/( 0.005*0.10) - Our Error Values 861.91= (.401*2.20)/(.05348*80.00) - Our Results Uncertainty = (0.005/.401. + 0.10/2.20 + 0.005/.05348 + 0.10/80.00)861.91 Uncertainty = 131.5846 The result is 861.91� 100 Hence our range is

  1. Antimatter and matter

    Although Dirac may not have been the most sociable person, the consequences of his physics can certainly be mind-boggling. Here are ten Dirac facts that you might not have known... Ten Dirac facts 1. Antimatter is the most expensive stuff on earth at $62.5 trillion a gram.


    When carbon dioxide gas is bubbled limewater, it turns is milky and this is a useful test to show the presence of a carboxylic group. e.g. CH COOH + CaCO3 (CH3COO)2Ca + CO2 + H2O 4. Sodium metal- on observation we see an effervescence and gas Conclusion - All acids

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