After that, dissolve the sample in 2 mL of deionized water and shake the test tube for 1 to 1 ½ minutes to dissolve the solid. Place another dry test tube in a 50mL beaker and weigh it. Find a bottle of barium iodide and record the name and molar mass. Then, weight out either anhydrous barium iodide or barium iodide dehydrate into this test tube and dissolve is it in 2 mL of deionized water. Pour the contents of one of the test tubes into the other and a reaction should occur and you should see a white precipitate of barium sulfate form.
Begin by adding 1 mL of rubbing alcohol to test tube and attach a thermometer to it. b. Place assembly in water bath and begin to heat beaker c. As isopropyl alcohol begins to boil, bubbles begin flowing from the capillary tube d. While temperature is decreasing, record the temp. when the last air bubble comes out of the capillary tube. e. Let assembly cool down and repeat process two more times.
Care must be taken when squeezing the pipet bulb on the filter pipet. Too much pressure might cause the filter to leak or fall off. Add about 2 mL of fresh tert-butyl methyl ether to the solid in the RB flask, warm briefly, let the solids settle for a minute, and pipet the liquid to the centrifuge tube as before. Again allow the solids to settle briefly in the centrifuge tube, then filter the liquid through the pressure filtration apparatus, into the same 25 mL Erlenmeyer flask. Doing a rinse such as this helps to ensure that any trimyristin that was left behind in the RB flask and centrifuge tube is not lost, thereby helping to ensure that
This energy is indestructible and is converted to light and heat. c. If you accidentally spill sodium chloride into a stove while cooking, it does not melt It is an ionic compound and the forces attract between the positive and negative ions, I ionic compounds they have a strong ionic bond and it takes a lot of energy to break. A high can only melt the table salt. 6) a. Which pairs will react from an ionic compound?
While conducting this laboratory experiment, be sure to use minimal amounts of each substance in order to create the habit of using only the amount necessary. This is a good habit to form so that product is not wasted and reduces the amount of product to dispose. Follow the steps below: 1. Pour 50 to 75 mL of water into a glass beaker and allow it to come to room temperature. 2.
Measure approximately 1 g of Copper(II) Sulfate Hydrate into the crucible and crucible and lid. 4. Heat the crucible gently. 5. Stirring carefully and observe the color of the hydrate until it changes to a consistent white color, then the Copper(II) Sulfate is dehydrated.
Name: ___________________________________ Date: ______________ Practice Test #3 ____ 1. When a precipitation reaction occurs, the ions that do not form the precipitate A) evaporate B) are cations only C) form a second insoluble compound in the solution D) are left dissolved in the solution E) none of these 2. An aqueous solution of potassium chloride is mixed with an aqueous solution of sodium nitrate. The complete ionic equation contains which of the following species (when balanced in standard form)? A) B) C) D) E) ____ 3.
Obtain a clean-dry test tube. Place 0.3g of the unknown substance in the test tube. Next, add 10mL of distilled water to the test tube. Mix with a stirring rod until unknown is dissolved. 2.
Objective: To observe the physical properties of solids containing: ionic, polar covalent, nonpolar covalent, network covalent, and metallic bonds. Thus, being able to classify unknown solids into the appropriate bonding categories based on their physical properties. Materials: - Test tubes - Test tube clamp - Bunsen burner - Distilled water - Conductivity probe - A spatula - One compound from each category (ionic, polar covalent, nonpolar covalent, network, and metallic) - Acetone/hexane mixture - Parafilm Methods: One compound from the following compounds was obtained from the professor: ionic, polar covalent, nonpolar covalent, network, and metallic. The following tests were carried out on each sample and the observations were recorded. For the metal sample, only steps one and five were conducted.
4) Ignoring step 3, after step 2, you can take the solution that you have created and pour it into a 100 mL beaker. Once the solution is in the beaker, turn on the conductivity tester and gently place it in the solution (try not to touch the bottom of the beaker). Record the results. 5) Now, take the beaker with the solution already inside and place it on a hot plate. Turn on the hot plate to a medium heat.