Measure the solution by right clicking on the beaker and choose pH meter *Then I had to measure the pH of 0.1 M sodium hydroxide Get a 100 mL beaker from the equipment menu Right click on the beaker, select chemicals, and add 50 mL of 0.1 M sodium hydroxide. Measure the solution by right clicking on the beaker and choose pH meter Part 2: *First add 35 ml of unknown acid a to 100 mL beaker. Select all chemicals from the toolbar in the chemicals section, choose unknown acid a. Put the volume at 35 mL in a new 100 mL beaker. *Then add two drops of phenolphthalein indicator to the beaker by right clicking, choosing indications, and adding 2 drops of phenolphthalein.
The two unknown solids are weighed to a mass of 0.15g each. The unknown solids are dropped carefully into the corresponding Erlenmeyer flask wit 50mL of distilled water. The solid in the water must be dissolved and afterwards add 10 drops of Bromecresol green to indicate the change of color when the solution has been titrated. The flask should start with a blue tint. HCl is carefully dropped into the Erlenmeyer flasks with the primed pipette until the solution turn to a green tint.
Part C: Density of Sodium Chloride (NaCl) Solution, a sample of NaCl was obtained and measured using a 100mL beaker and a 10mL pipet to determine the concentration of the solution. In order to obtain the appropriate result, a calibration graph and density measurement was used to determine the concentration of the sodium chloride solution. In conclusion, based on the water temperature of 21.8°C in part A’s graduated cylinder experiment obtained, it was determined that the average density was .0973g/mL with a percentage error of 2.5%. When graphed the measurement was equal to Y=0.988x. Part B: The graduated pipet’s average density at 22.3 °C was determined to be 0.9785g/mL with a percentage error of 1.89% shows the graduated pipet to be more accurate and precise.
Nathan Bahn Beer’s Law Study Lab Introduction: In this lab, we used a spectrometer to observe the transmittance of light at a certain wave length. We experimented to see if the molarity of a solution changes the transmittance of light and the absorbance of that light by the solution. By observing the percent transmittance and the amount of light absorbed, we can calculate the amount of color absorbing components in the solution. Through this process is how we are able to discover the amount of copper in the solution. Experimental Procedure: 250 mL of the copper solution was made by creating 100 mL of the solution, reacting CuO with HNO3, and then diluting to the mark of 250 mL.
We need to be able to find the limiting reagent and be able to go through the process of gravimetric stoichiometry. Hypothesis: The limiting reagent will be the strontium chloride due to the calculations and the copper (II) sulphate pentahydrate. My calculations also conclude that we should get 1.378 g of the precipitate of Strontium Sulphate. SrCl2 * 6H2O + CuSO4 *5H2O SrSO4 + CuCl2+ 11H2O I Mole 1 Mole 1 Mole 1 Mole 11 Mole 2g 2g ? Materials: • 2 Graduated Cylinders • Distilled Water • Stirring Rod • Balance • One 250ml Beaker • One Erlenmeyer Flask • Filter Paper • Copper (II) Sulphate Pentahydrate • Strontium Chloride Hexahydrate Procedure 1.
Part II: Colorimetry of FD & C Blue # 1 Dye (Brilliant Blue FCF) Discussion and Review: In this part of the experiment, we will use a color standard calibration system to determine the concentration of an unknown solution. FD&C dyes refer to specific commercial dyes approved for human consumption under the US government’s Food, Drugs, and Cosmetics Act. We will start with FD&C Blue #1, a commercial food dye of known concentration. Through serial dilutions we will end up with a color “standard”, a set of diluted
In the chart provided record if each compound is solubility in water. Part D - Conductivity 1. Obtain six 100ml beakers and add 50ml of water to each. 2. Place a 10g sample of each of the above compounds in a separate beaker.
After 10 seconds, the colorless mixture suddenly turns blue. Concept: Demonstrates a typical clock reaction; shows the effect of the interaction between chemical reactions that have different rates. Materials: • Solution A o 0.6 grams Starch o 30 mLs of Acetic Acid o 4.1 grams of Sodium Acetate o 50 grams of Potassium Iodide o 4.7 grams of Sodium Thiosulfate ▪ Allow mixture to cool and dilute to 1 liter with distilled water o 1 liter flask • Solution B o 500 mLs of 3% Hydrogen Peroxide o 500 mLs of distilled water o 1 liter flask o Safety: Hydrogen Peroxide can be irritating to skin and eyes. Wear safety goggles and gloves. Procedure: Mix the two solutions together.
After adding three drops of brymothymol blue indicator, the solution was now a clear blue colour. In the first and fourth trial, the bromothymol blue indicator caused the solution in the Erlenmeyer flask to turn a pale yellow colour from the blue colour that the solution already was after the 10.00mL of acid was added. This indicates that the solution was now acidic. In the second, third and fifth trial, the bromothymol blue indicator caused the solution in the Erlenmeyer flask to turn a pale green colour from the blue colour that the solution already was after the respective amounts of acid was added to the solution. This indicates that the solution was now neutral, or close to a pH of 7.
The extraction process is when a solvent, dichloromethane (15mL) is added to the filtrate in a separatory funnel; the mixture is gently swirled together 3 times, and stopcock is released in between to vent the funnel. Dichloromethane (including the emulsion) is then drained from the bottom into a 50mL Erlenmeyer flask. Same extraction process is repeated on the same filtrate and the dichloromethane is, once again, let out to the same 50mL Erlenmeyer flask as before. The combined dichloromethane solution and water (20mL) is poured into a rinsed separatory funnel. Mixture is gently swirled and drained out into an Erlenmeyer flask.