Does Salt Affect Water Boiling Point?

Using a scoopula, add 5-6 grams of the hydrate into the dish and measure the mass of the hydrate and the dish

Procedure: I used a ruler, thermometer, and scale to take measurements. I used a graduated cylinder, short step pipet, scale, and ruler to determine volume and density. I used a volumetric flask, graduated pipet, pipet bulb, scale, and glass beaker to determine concentrations and densities of various dilutions.

Next, I poured distilled water just below the 250ml mark on the neck of the volumetric flask.

First, we were to measure and record the mass of a beaker, then transfer about 1 gram of the salt mixture into the beaker, measure, and record the combined mass. Then, we had to fill a 400-ml beaker with deionized water and test it to make sure that the ph was just basic. We then combined the deionized water and salt by adding about 150ml of the deionized

Then 8.0g of copper sulfate crystals were placed inside the beaker and the mass was recorded for the actual crystals. 50 mL of water was added to the beaker with the crystals. The ring stand was set up with the wire mesh on it and one partner should place the mixture in the beaker on it should be heated without letting the mixture boil. Stir the mixture and heat until the crystals are dissolved. While one partner does this, the other should obtain 1.5g of iron filings in a measuring cup and records the mass. Then the iron filings should be added small amounts at a time to the heated solution. Stir continuously until all the mixture is added to the beaker. Then it sat for 10 minutes and observations were recorded. Record the mass of a filter paper and set up a filtration apparatus with the filter paper in a funnel over an Erlenmeyer flask. Decant the liquid through the paper slowly trying not to allow any solid to get on the filter paper. Then with de-ionized water, rinse your solid in the beaker and let the solid settle then decant the liquid. Repeat the washing twice more and in the last time guide all the solid into the filter paper. Then place the filter paper on a watch glass and then into a warm oven to dry. After it is cool, record the mass of the watch glass, filter paper and solid. If there is not enough time to cool, you may have to do it the next

9) Trial E: Remove the syringe and empty the beaker. Add a Thermometer to the beaker. Add 200 mL of Room Temperature water to the beaker and heat with a Bunsen Burner until it reaches 100° C. Remove the Bunsen Burner. Repeat Steps 5 & 6.

Because salt dissolves in water, we added water to the salt and sand mixture. Sand is insoluble in water making the sand not dissolve. The mixture containing of sand and salt water was then filtered with filter paper. The filter paper allowed the salt water to pass through because it is a liquid while not allowing sand to pass through because it is a solid. The salt water was then collected in a pre-weighed 250-mL (67.88 gram) beaker while the sand and filter paper was put in a pre-weighed (52.02 gram) 100-mL beaker. The water was then evaporated because we left both beakers to dry overnight.

Then in the last test tube fill it up with 5ml of sodium sulphate. Then after that carefully pour the sodium carbonate solution into the test tube labelled copper chloride solution examining the result and recording appropriately.

B. While heating two different samples of water at sea level, one boils at 102°C and one boils at

The goal for this lab is to be able to get the boiling water's temperature to increase by adding table salt. The problem it is trying to explain is, how does table salt affect the boiling temperature of water? does it increase or decrease? or does it stay the same?

Cut the potatoes using a cork borer approximately 5cm in length and 1cm in diameter. Using the appropriate tool cut the potatoes into cylinder form measuring the cylinders with a ruler.

Distillation. Transfer the clear liquid to a dry 25-mL round-bottom flask using a Pasteur pipet. Add a boiling stone and distill the crude t-pentyl chloride in a dry apparatus. Collect the pure t-pentyl chloride in a receiver cooled in ice. Collect the material that boils between 78°C and 84°C. Weigh the product and calculate the percentage yield.

The boiling points of the ionic and covalent compounds do not show any clear sign of differentiation. Because ionic compounds have high boiling points, the expected results were that unknown 1 and 2 were going to boil last. According to the results, it was mostly it was mostly the results of unknown 1 that was incorrect. Because the beakers with the 4 different unknowns in each of them were right beside each other, the heat of the surrounding beakers may have transferred to the beaker beside each other. Furthermore, all the beakers on the hot plate might have made the process of boiling take longer. Because the center of the hot plate might have had the most heat, heating each beaker individually might have resulted in more accurate results. Also, when instructed to fill up the beaker halfway, it was not clearly implied that the intended amount of water was supposed to be 25mL, not 35mL. The ratio between the amount of distilled water and the unknown substance may have also hindered the results. The actual boiling point for sodium chloride

Solute – A solute is the material (solid, liquid or gas) that is dissolved in the solvent to create the solution.

8. In order confidently determine what substance my “G9R” was I would have to do over the boiling point experiment a couple of more times. I would turn the gas off and take the Bunsen burner away from the apparatus when the stream of bubbles started coming out from the mouth of the capillary tube. This would allow me to correctly determine when the atmospheric pressure was equal to the vapour pressure.