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

Solubility of potassium chlorate

Extracts from this document...


SOLUBILITY OF POTASSIUM CHLORATE By Yutao (Anya) Liang Solubility is the maximum amount of solid that will dissolve in 100g of solvent. The solubility of a substance depends on the type of ionic particles in it. So the solubility of each substance is different. The formula of solubility is: SOLUBILITY (g/100g) = (SOLUTE / SOLVENT) * 100 I did an experiment to prove this and find the solubility of potassium chlorate, an ionic solid. Apparatus: 2g potassium chlorates, some distilled water, a stand, a clamp, two beakers, a thermometer, a test tube, and a measuring cylinder. Method: 1. Put the potassium chlorate into the test tube, and then put 4g distilled water. 2. Then the solute (which is the salt) dissolves in water (the solvent) by heating. A solution is made, this is the dissolved solute in solvent. The solution is left to cool down, and the temperature at which the solute crystallizes is recorded. ...read more.


Temperature will affect solubility. If the solution process absorbs energy then the solubility will be increased as the temperature is increased. If the solution process releases energy then the solubility will decrease with increasing temperature. The solution may be saturated, but it likely is less than saturated. Only when some solid remains undissolved are you sure it is saturated. The presence of undissolved solid suggests that the solution is saturated. From the graph, 25 g KClO3 dissolve at 70 �C, and 50 g KClO3 dissolve at 96 �C. The graph shows me that I can get different kinds of information about solubility of this solid in water. 1. I can get the solubility of KClO3 at any temperature. For example.....(use graph) This means I can get the solubility of KClO3 at any temperature. 2. The solubility at 20oC is ... if I double this temperature to 40oC the solubility value is. This has not doubled in value. This shows that solubility is not proportional to rise in temperature. The solubility vs. temperature is a curve. 3. ...read more.


If time had allowed I could have repeated the work and obtained at least 3 sets of results and used the average. The results would have been more reliable. However, the solubility line I got gave me enough information to explain the solubility of solid in solvent. 8. If I had obtained the solubility of other salts I could also compare their saturation temperature and solubility with potassium chlorate. Scientific explanation of solubility Ionic compounds exist as giant ionic structures. There is a strong force of attraction between the opposite charged ions. A lot of energy is needed to break up this strong force .....(explain how water breaks up the crystal structure and surrounds the ions and how the amount of solid in water affects its solubility. Use the ionic model from your notes..) (Anya: you must try to interpret your graph. Explain the line and give information form the graph. I have tried to show you this by giving you all the points necessary. Please try to understand these points and write them in your own style, using your own words. Do not use my words but only be guided by them.) Anya ...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. Determine Solubility of KClO3 Salt.

    Solubility in water in the presence of DOM is explained by the equation below: Csat,DOM = Csat (1 + [DOM]KDOM) [DOM] = concentration of DOM in water, kg/L KDOM = DOM/water partition coefficient. And for co-solvent factor, its presence increases the solubility of hydrophobic organic chemicals.

  2. Investigate how the solubility of Potassium Nitrate is affected by Temperature.

    4.48 3.28 3.20 4.8 Analysis My Graph and table shows that the temperature of water does affect the solubility of potassium nitrate, as I said in my prediction, which was higher, the temperature, the more potassium nitrate will be dissolved.

  1. How the solubility of potassium chlorate (KClO3) changes as the temperature changes

    *100 Mass of water (g) 2*100=50 4 2*100=25 8 2*100=16.67 12 2*100=12.5 16 2 *100=10 Average temp = (temp1 + temp2) 20 2 Results: Mass of KclO3 (g) Volume Of Water (cm3) Solubility g/100cm3 Water Temperature (oC) at which Crystals reappear Temperature (oC) at which Crystals reappear Average Temperature (oC)

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

    present in 100 cm3 of spinach extract solution. To do this the moles present in 10 cm3 will have to be multiplied by 10. 0.000363833 mol dm-3 X 10 = 0.003161666 mol dm-3 Only 15 grams of Spinach Oleracea were used to make up the 100cm3 spinach extract solution, so in order to work out the moles of Iron (II)

  1. Find the solubility of potassium nitrate in water at different temperatures and to estimate ...

    of the saturated solution Reciprocal of Kelvin temperature (1/T)/K-1 Solubility of potassium nitrate/mol dm-3 of water ? Log 10 ? Celsius T/�C Kelvin T/K 10.1 8.0 67� 340 1/340 12.5 1.09 10.1 10.0 57� 330 1/330 10 1 10.1 12.0 48� 321 1/321 8.33 0.92 10.1 14.0 42� 315 1/315

  2. My plan is to find the determination of solubility curve of potassium chlorate.

    as shown on the diagram sheet. * Put 2 grams of potassium chlorate into a boiling tube. * Add 4ccm of distilled water from the burette. ( the burette is more accurate to use) * Place the boiling tube in boiling water and allow the solid to dissolve.

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