2. All anhydrous sodium carbonate was dissolved in a beaker with a suitable amount of deionized water and the mixture was stirred. 3. Sodium carbonate solution was poured into a 250.0 cm3 volumetric flask and it was made up to the graduated mark using deionized water. 4.
Next, 2 drops of Copper (II) Nitrate, Cu(No3)2?3H2O solution were placed within the first seven B wells. Next, 2 drops of Iron (III) Nitrate, Fe(No3)3?9H2O were placed within the first seven C wells. Next, 2 drops of Barium Nitrate, Ba(NO3)2 were placed into the first seven D wells. Lastly, 2 drops of Nickel (II) Nitrate, Ni(NO3)2?6H2O were placed into the first seven E wells. The following steps were performed to create the ionic reaction.
A melting point will be ran on the aspirin when completely dry. A capillary tube containing the dry aspirin will be placed into the melting-point apparatus. This process is to determine the melting point range of aspirin. First, a hot water bath was created with a 400. mL beaker on a hot plate. The temperature was raised to 70 degrees Celsius and 4.419 g of salicylic acid was measured out on a balance and transferred into a 125. mL Erlenmeyer flask.
Controlled The controlled variables of the experiment were: A. The volume and concentration of the Hydrochloric acid. B. The concentration of the Sodium Hydroxide. Equipment List * Boiling Tube * 10 cm3 1mol dm-3 Hydrochloric Acid (HCL) * 15 cm3 1mol dm-3 Sodium Hydroxide (NaOH) * pH and Temperature Probes * Data Logger * Measuring Cylinder ‘ * Boiling Tube * Teat Pipette Method * Add 10ml of Hydrochloric acid, measured in a measuring cylinder, into a boiling tube.
25 ml of diluted unknown acid solution to 100ml beaker by using 25 volumetric pipet. 10ml of deionized water and 3 drops of phenlpthalin indicator the beaker labeled as 3. Potentiometric titration acid solutions 125 ml of NaOH was obtaining in a beaker and 50 ml of NaOH transfer to buret the tip and the meniscus is at below 0 ml. one magnetic stirring bar placed in a beaker contain one of the known solution on a stir. The pH recorded by using pH electrode before adding NaOH.
Mix either chlorine solution, bromine solution or iodine solution with either potassium chloride solution, potassium bromide solution or potassium iodide solution. 2. For every possible mix of the nine total mixes, record the appearance of the solution formed. 3. For every mix, add cyclohexane, record the appearance of the solution.
Specific Heat of a Metal Michael Diaz Ms. Zhort Performed: October 3, 2013 Due: October 24, 2013 Period: 1 Lab Partner: Rocco & Asha Objective: This lab was meant to teach us how to find the specific heat of a metal sample. Materials: * Specific heat set * Balance * Thermometer * Tap Water * Hot plate * Polystyrene cup and a lid * Stirring rod * 250 mL beaker * String (about 15 cm) Procedure: 1. Fill a 250 mL beaker approximately half full of water. Place the beaker of water on a hot plate. Begin heating the water to the boiling point.
Define also the overall order of a reaction and describe how it’s found. Explain how the iodine clock reaction works and the method it employs to find the order of a reaction with respect to a particular reactant. Experimental: Apparatus: 3 -100 cm3 beakers, 1 thermometer, 0-100 0C, 8 burettes with beakers and funnel for filling, clamps and stands, stop clock or watch. Reagents: Potassium peroxodisulphate (VI) solution [0.100 mol dm-3 and 0.050 mol dm-3 K2S2 O8], Potassium iodide solution, [0.500, mol dm-3 and 0.250 moldm-3, KI], Sodium thiosulphate solution, [0.010 mol dm-3 Na2S2O3], Starch solution, 0.2% Procedure: 1. Using a burette, run 5.0 cm3 of 0.100 mol dm-3 peroxodisulphate solution into a 100 cm3 beaker.
Bunsen burner 5. 100 mL Erlenmeyer flask 6. 250 mL graduated cylinder 7. Tripod stand 8. Wire gauze 9.
The next one was sodium bicarbonate solution I placed 2 drops into 5 vertical rows. The next was carbonate solution I placed 2 drops into 5 vertical rows. The next was hydroxide solution I placed 2 drops into 5 vertical rows. The sodium iodine solution reacted with the cobalt (II) nitrate, it turned a mirky white, the sodium iodine solution also reacted with the copper (II) nitrate, this one turned orange. Sodium phosphate solution reacted with the cobalt (II) nitrate turning lavender, the copper (II) nitrate turning red, the iron (III) nitrate turning a yellow-orange, the