| A colorless solution was formed after the addition of concentrated HNO3. | Concentrated HNO3 | - | 4 Mn2+ | Centrifuge the solution. | Deep purple solution was formed. | A slight excess of solid NaBiO3 | 2Mn2+ + 5BiO3- + 14H+→ 2MnO4- + 5Bi3+ + 7H2O | 5 Fe3+(2+) | Centrifuge the solution. | A light red precipitate was formed.
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.
The universal indicator is made from magnesium hydroxide with a pH value of 4. A universal indicator is typically composed of water, propan-1-ol, phenolphthalein sodium salt, sodium hydroxide, methyl red, bromothymol blue monosodium salt, and thymol blue monosodium salt. The colours that indicate the pH of a solution, after adding a universal indicator are: pH range Description Color 0-3 Strong acid Red 3-6 Acid Orange/Yellow 7 Neutral Green 8-11 alkali Blue 11-14 Strong alkali Violet/Purple Dry-Ice Dry ice, sometimes referred to as "Cardice" or as "card ice" (chiefly British English), is the solid form of carbon dioxide. It is used primarily as a cooling agent. Its advantages include
LAB 1 NAME: Amy Rampersad. DATE: Saturday 7th April, 2012. TITLE: PREPARATION OF A SOLUBLE SALT BY A TITRATION METHOD. AIM: To prepare Sodium Chloride crystals by Titration of Sodium Hydroxide with Hydrochloric Acid. APPARATUS: Burette (50 cmᶾ), Pipette (25 cmᶾ), two conical flasks (250 cmᶾ), two beakers (250 cmᶾ), funnel, wash bottle, retort stand, boss and clamp, evaporating dish, pipette filler, hot-plate.
Use the incinerator to allow it to dry completely. Result * Erythrocytes: Pink or yellowish red. * Platelets: Violet or purple granules. * Neutrophils: Blue nucleus, pink cytoplasm, violet granules. * Eosinophils: Blue nucleus, blue cytoplasm, red granules.
Title : Reaction of Carboxylic Acids Objective : To Determine The Reaction of Carboxylic Acids Procedure : As referred to Lab manual. Results: A. Salt Formation |Compound |Solvent |Solubility | |Benzoic Acid |Cold Water |Partially soluble | |Benzoic Acid |10 % NaOH |Soluble | B. Salt Hydrolysis Sodium acetate solution changed the color of litmus from red to blue. C. Reaction With Sodium Carbonate Observation : A lot of gas bubbles was released.
When in flame it produces gas rapidly and bubbles. Liquid turns into gas quickly. When liquid disappears solution (now a solid) turns white | 4 | A Initial temperature is 15 degrees Celsius and the final temperature is 17 degrees Celsius. BThe blue hydrated copper sulphate turned white, evidence of condensation of a clear liquid present on the inside of the test tube.C concentrated sulphuric acid turns black on paper towel and is clear on the white cottonD Carbon pillar grows cause of air bubbles, it is brittle, it is both corrosive with a hole and there is evidence of carbon produced | 5 | No temperature change and iodine brown/yellow gas produced | Properties of Sulphuric acid results table Aim: To investigate and observe the properties of sulphuric acid through five different experiments where we will determine its extent of ionisation in aqueous solution, reaction of sulfate ions, action as a strong acid, affinity for water and action as an oxidising agent. Background: Sulfuric acid (H2SO4) is a diprotic acid (can donate 2 protons to a base).
Prediction: Water: 7.0, Green, neutral. Orange Juice: 3.0, red, strong acid. Lido Lemonade: 5.0, red-orange, weak acid. Coca Cola: 3.0, red, strong acid. Skim milk: 5.0, red-orange, weak
The reduction of permanganate requires strong acidic conditions. Introduction: In this experiment a purple colored solution of potassium permanganate, with an approximate concentration of 0.025M, will be added to a solution containing Fe2+ ions. The manganese is reduced from a 7+ oxidation state in the permanganate ion to form colorless Mn2+ ions. The equivalence point is indicated at the point when all of the Fe2+ ions in the solution are oxidized and the colorless mixture retains a purple tint. Procedure: Fill a buret and tip with KMnO4.
Mixture is gently swirled and drained out into an Erlenmeyer flask. Anhydrous magnesium sulfate is added to dehydrate the washed mixture. The solution is then filter into a weighed, dry, 100mL Erlenmeyer flask. Dichloromethane in the mixture is vaporized with a rotary evaporator. The Caffeine, white powder residue, (0.0486g) should be obtained.