Project on Saturated Solutions: Measuring Solubility iC BS E.c om Index 1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. 12. Certificate Acknowledgement Objective Introduction Basic concepts Materials and Equipment Experimental Procedure Observation Conclusion Result Precautions Bibliography iC BS E .co m CERTIFICATE This is to certify that the Project titled ’Saturated solutions: Measuring Solubility ’ was completed under my guidance and supervision by Roll No. ________
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constituent in the original sample can be calculated. Precipitation is effected by inorganic or organic precipitating agents. Two common inorganic precipitating agents are silver nitrate‚ which is used to precipitate halide ions such as chloride‚ and barium chloride‚ which is used to precipitate sulfate ion. In all of these precipitation reactions‚ the product is a salt because it is formed by reactions between cations and anions.Thus the bonding is ionic or electrovalent. The three major requirements
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Results Calculation a) 50ml of suspensions containing 5% w/v of sulpharmerazine which containing 10-2‚ 5 x 10-3‚ 10-3‚ 5 x 10-4‚ 10-4‚ 5x 10-5‚ and 10-5 molar concentrations of Calcium Chloride. ( 10-2 are provided ). By using this formula‚ we can get the amount of calcium chloride to be added in making 50 ml suspensions containing 5% w/v of sulpharmerazine. M1V1 = M2V2 M2 = 5 x 10-3‚ 10-3‚ 5 x 10-4‚ 10-4‚ 5x 10-5‚ and 10-5 M ‚ V2 = 50ml M1 = 0.01M Thus‚ V1 = ( M2 . V2 )
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Sealable‚ zipper-lock plastic bags‚ quart size‚ 6 Measuring spoons‚ teaspoon and half-teaspoon‚ 1 each Water‚ distilled‚ or deionized Phenol red‚ 0.02% aqueous solution 30mL Sodium Bicarbonate (solid)‚ 3 tsp. Calcium Chloride (solid)‚ 6 tsp. Safety Precautions: Calcium chloride is slightly toxic by ingestion. Phenol red is a dye solution and will stain skin and clothing. Avoid contact of all chemicals with skin and eyes. Be careful to mix the chemicals in the amounts called for in the procedure
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Claim Evidence Reasoning What is your CLAIM? Sodium Bicarbonate and water make the bag cold. EVIDENCE to support your claim Sodium Bicarbonate and water make the bag noticeably cold. When you take calcium chloride‚ phenol red‚ and water the bag becomes hot. If you add Calcium chloride and sodium bicarbonate there will be no reaction. If you add Sodium Bicarbonate and Phenol red the bag will become cold. When you take Sodium Bicarbonate‚ Phenol red‚ and water the bag will become cold. Using
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It is clear that salt‚ also known as sodium chloride‚ should no longer be used on our roads in the winter months. The first two reasons why salt needs to stop being used are because salt negatively affects aquatic ecosystems and causes damage to vegetation. The third reason is because thankfully‚ there are alternatives that we can use‚ that would be benefiting us which we should use instead of sodium chloride. To begin with‚ sodium chloride is detrimental to our aquatic ecosystems when it is
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Introduction The experiment is testing for the formation of precipitates caused by different limiting reactants. A precipitate results in a solid formed by an ionic compound. Calcium nitrate and copper sulfate will be added to separate beakers with approximately half of the solutions from the Büchner funnel system of each trial to test for the formation of precipitates. The limiting reactant is the reactant that will run out first in the chemical reaction. It is important to recognize which chemical
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orange‚ coming in with the second lowest energy. Iron chloride had a “sparky” appearance that lasted for approximately six seconds and it was concluded that it had a high energy. Lithium chloride burned a pinkish color. Potassium chloride had a high energy and produced a purple flame. Strontium chloride had the lowest energy which was determined by red color of its flame. Unknown 1 was strontium chloride and unknown 2 was calcium chloride. The unknowns were found by comparing their flame colors
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An example of this process is when calcium chloride dissolved in water. The polar water molecules attracted the oppositely charged Ca2+ and Cl- ions as calcium chloride is a polar molecule as well. The ions brake apart as the water attraction is greater than the ionic bond within the calcium chloride molecule. Solubility is also important for conductivity as some elements such as calcium chloride do not conduct in a solid state. This explains why calcium chloride conducted when dissolved in water
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lab: * 6 Watch Glasses * 2 g Calcium Chloride per parts A‚ B‚ C * 2 g Citric Acid per parts A‚ B‚ C * 2 g Phenyl Salicylate per parts A‚ B‚ C * 2 g Potassium Iodide per parts A‚ B‚ C * 2 g Sodium Chloride per parts A‚ B‚ C * 2 g Sucrose per parts A‚ B‚ C * 6 Bunsen Burners * 6 Test Tubes with 25 ml Ethanol each * 6 Test Tubes with 25 ml Water each * 6 100 ml beakers with 50 ml Water each * 10 g Calcium Chloride per parts D * 10 g Citric Acid per
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