Add 1.0M copper (II) nitrate to the first mark on the test tube. 4. Add 1.5M sodium hydroxide to the second mark on the test tube. Mix with the stirring rod. Touch the bottom of the outside of the test tube to see if heat has been released.
To the second, add 10% NaOH dropwise until the pH is 14. (To do this, add a couple of drops of NaOH to the tube; stir thoroughly with a stirring rod; then touch the stirring rod to a piece of pH paper to check your pH.) To the third, add 0.5% sodium bicarbonate solution to pH 9, and to the fourth, add 2% HCl to pH 2. Record your observations on the data sheet. Repeat the above tests using 2% casein solution.
Chemistry: Molarity and Stoichiometry Directions: Using the definition of molarity, the given balanced equations, and stoichiometry, solve the following problems. Please submit your work via the link provided. 1. Calcium hydroxide (“slaked lime”) and sulfuric acid react to produce calcium sulfate and water according to the following balanced equation: Ca(OH)2(aq) + H2SO4(aq) ⋄ CaSO4(s) + 2 H2O(l) a. How many liters of 0.2 M calcium hydroxide do you need in order to have 6.0 moles of calcium hydroxide?
Purpose: The purpose of this lab is to investigate whether mass is gained or lost during a chemical reaction. Hypothesis: It will be found out that the mass is neither gained nor lost during a chemical reaction but transferred. Materials: * Safety goggles * Erlenmeyer flask * Balance * Graduated Cylinder * Beaker * Iron (III) chloride solution * Copper (II) sulphate solution * Sodium bicarbonate * Test tubes (small, and large) * Rubber Stopper * Tweezers * Paper towel * Scoopula * Sodium hydroxide solution * Hydrochloric acid Procedure: 1. 5ml of iron (III) chloride was measured and placed in the Erlenmeyer flask. 2.
Aim To compare the reactivity of various metals by observing their reaction with hydrochloric acid Hypothesis That the all the metals will produce foam and a pop. Variables Independent – Magnesium, Aluminium, Zinc, Copper Dependent – Detergent, Hydrochloric Acid Controlled – Size of the metals, amount of detergent and hydrochloric acid Materials 2 M hydrochloric acid Detergent 10 x test tubes and test tube rack and 5 rubber stoppers 0.5 cm pieces of magnesium, aluminium, zinc and copper 2 cm pieces of magnesium, aluminium, zinc and copper Steel wool Ruler Timer Bench mat Matches and birthday candle Marking pen Safety Remember to wear safety glasses and protective gloves when you do this experiment. 2 M HCl is corrosive. Wash with plenty of water should you get any on your skin or in your eyes. Method Part 1 1 Clean the surface of the 0.5cm piece of magnesium with a piece of steel wool 2 Place the magnesium into a test tube 3 Add three drops of detergent to the test tube 4 Add 2 cm of hydrochloric acid to the test tube.
Riya Singh Banita Sathpathy Period 1 Analysis of a Commercial Bleach Purpose The purpose of this experiment is to determine the amount of sodium hypochlorite in commercial bleach by reacting the bleach with sodium thiosulfate. Procedure In this experiment a solution of sodium thiosulfate of known concentration will be added to the bleach using a buret in a titration procedure. The disappearance of the dark blue color of the starch- iodine complex will signal the end point. Data Trial 1 Trial 2 Trial 3 Initial Reading (ml) 0 0 0 Final Reading (ml) 35.7 36.0 36.6 Volume of Na2S2O3 35.7 ml 36.0 ml 36.6 ml Calculations and Analysis 2 S2O3-2 = I3- = I2 = ClO- Therefore looking at the equation above, we can conclude that for every mole of sodium thiosulfate we need half a mole of sodium hypochlorite. (35.7+36+36.6)/3=36.1 ml is the average volume of the Na2S2O3.
Describe the precipitate formed. NaOH (sodium hydroxide - a base) and phenolphthalein. Phenolphthalein is
One method for preparing baking soda is through reacting crystalline ammonium hydrogen carbonate with brine according to the following equation: NH4HCO3(s) + NaCl (aq) --> NaHCO3(aq) +NH4Cl(aq) Eq. 1 Brine contains sodium chloride, the compound needed to make baking soda, as well as potassium chloride, lithium chloride, and calcium chloride. Once the reaction has been completed, the solid baking soda is filtered off, but some contaminants may be present in the solid. The first step in determining the purity of the sample is to perform thermal gravimetric analysis (Experiment 7) on the baking soda sample to determine the percent composition of sodium bicarbonate in the sample. A sample of the baking soda will be heated until it decomposes to leave solid sodium carbonate according to the following equation: 2NaHCO3(s) --> Na2CO3(s) + CO2(g) + H2O(g) Eq.
Equipment/Materials: sample of unknown copper compound distilled water electronic balance 250 mL beaker magnesium metal 6 M HCl filter paper ethanol acetone funnel stirring rod watch glasses Safety: • Always wear an apron and goggles in the laboratory. Procedure: 1. Obtain a vial of an unknown copper compound. Record the
INTRODUCTION: This experiment aims to demonstrate liquid-liquid extraction. Chemicals used were 18.0 M Acetic Acid, Toluene, Phenolphthalein and 0.1M Sodium Hydroxide. In this experiment, the process of titration was used in order to determine the amount of acetic acid, which was done in three different procedures (1 trial each). The calculations took place right after accomplishing all