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

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Introduction

Experiment - The Solubility of Potassium Nitrate Aim To investigate how the solubility of Potassium Nitrate is affected by Temperature. Background Knowledge Potassium Nitrate (KNO3) is an ionic compound. The strong ionic bonds hold the compound in an ionic lattice which gives KNO3 its crystalline structure. These ionic bonds also have other properties which will affect my investigation, I must be aware of these properties for greater accuracy in my method. The ionic bonds give KNO3 high melting and boiling temperatures. In the case of KNO3, ionic bonds are present, which are strong and hard to break under room temperature; I believe that this may have an impact on the solubility of KNO3 at low temperatures, where there is very little energy present to break these bonds. Particles move faster and collide with a greater energy output. A greater proportion of these particles now have enough energy to react. Therefore there is a greater chance of a collision between KNO3 and water molecules resulting in a successful reaction. Hypothesis My hypothesis is that the temperature of the water affects the solubility of Potassium Nitrate. ...read more.

Middle

Apparatus * Test tube rack * Five test tubes * Five Plunges * Potassium Nitrate * Spatula * Thermometer * Stop Watch * Scale (Electric) * Water Bath (at 40 oC, 60 oC and 80 oC) * Ice (for 4 oC) * Room at 20 oC * Water Method 1. Collect all the required Apparatus. 2. Fill up the five test tubes with 10ml of water, which are at five different temperatures. 3. Weigh the Potassium Nitrate without the containers lid on. 4. Add one spoonful of potassium nitrate to the fist test tube, which has the lowest water temperature (4oC). 5. Place a plunge on the test tube and shake for 1 minute. 6. Check if the solution has become saturated this is where no more salt can be dissolved in the water and crystals form at the bottom of the test tube. If no crystals appear repeat steps 4 to 5until the solution becomes solute. 7. Once the solution is saturated, re-weigh the potassium nitrate and work out the difference. By working out the difference this shows how much potassium nitrate was dissolved (Starting weight take away end weight equals difference). ...read more.

Conclusion

then converted into kinetic energy so if the energy is strong enough allows the reaction to take place causing the KNO3 to dissolve. I think I should have repeated this experiment at least three times making sure that the results I gather are accurate or I could have worked out an average, or I could have repeated the experiment the results which were anomalous. I think I did get a suitable range because these are the results I predicted and to prove this I could plot them on my scatter diagram and they would fit in with the correlation of the points. There is a particular pattern in my graph because as I increase the water temperature the more potassium nitrate is being dissolved, so the line of best fit in my graph is a curve. There is only one of a possible many variables of the original question that I could investigate, if given time I would do the experiment the other way round, not testing the solubility of potassium nitrate in water, but how water evaporates in a solution of potassium nitrate and water. ?? ?? ?? ?? Ricky Patel 10/05/2007 5:21 AM C:\Documents and Settings\Patel\My Documents\My Files\Coursework\Completed Coursework\Science\CourseWorkchemsolubilyofpattasiumnitrate.doc ...read more.

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