Pour all the filtrate and washings into a 250cm3 volumetric flask. Make up to 250cm3 with 1.0mol dm-3 sulphuric acid(VI) acid. Stopper the flask and invert several times to thoroughly mix the solution. 5. Fill the burette with 0.005mol dm-3 potassium manganate(VII) solution.
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. MATERIALS: Approximately 2.0 mol dmˉ³ hydrochloric acid, 1.0 mol dmˉ³ sodium hydroxide, methyl orange indicator. METHOD: 1. Firstly, the burette was rinsed with a little hydrochloric acid and filled up to just above the zero mark. 2.
2. A 250mL volumetric flask was washed three times with distilled water. 3. A funnel was used to wash the crystals in to the volumetric flask with the aid of the glass rod and the wash bottle. All the washings were placed into the volumetric flask.
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.
The buret had used the NaOH thoroughly rinsed three times because at the first titration the NaOH solution was used. About 50Ml the NaOH solution was in a clean beaker and brought it to experiment area. A funnel was used to fill the NaOH into the buret and recorded the initial volume on the buret to the correct number of significant figures. A pipette was used to take 10.00ml HCl into a clean 50mL Erlenmeyer flask. Three drops of phenolphthalein indicator was added into the HCl solution.
A mixture of Br-, Cl- and PO43- ions was subjected to an anionic column packed with polym-N(CH3)3+OH-, eluted with 9mM sodium carbonate. (i) Arrange the above analyte ions in order of increasing retention time in the anionic column. (3 marks) (ii) Describe how the analyte ions were separated in the anionic column according to order of retention time answered in part (2)(i). (8 marks) 3. An unknown compound is irradiated with an excitation photon.
Then by writing a balanced chemical equation and using the titration formula, Nb+Ma+Va=Na+MbVb , the molarity is able to be determined. Procedure: 1) Using the graduated cylinder add 10.0 mL of water into the Erlenmeyer flask. 2) Add 5.0 mL of HCl into the flask using another graduated cylinder because acid goes into water when mixing them. 3) Add three drops of phenolphthalein indicator into the flask. 4) Swirl the flask in circular movements to mix the substances.
The second experiment, procedure 1, combined [Co(NH3)5 (H2O)]Cl2 (0.0060M, 1.52g) and (25mL) of distilled water to an 125mL Erlenmeyer flask. The flask was gently heated (dial 5-6) and stirred until all the compound was dissolved. The heated solution was then vacuum filtered through a fritted funnel and the filtrate was cooled in an ice bath until the
Prepare the apparatus according to diagram A. 2. Prepare 100 cm3 of 0.2 M hydrochloric acid by mixing 10 cm3 of 2 M hydrochloric acid with 90 cm3 of distilled water. 3. Fill the conical flask with 50 cm3 of 0.2 M hydrochloric acid.
When the solution is acidified during diazotization to form nitrous acid, the sulfanilic acid is precipitated out of solution as a finely divided solid, which is immediately diazotized. The finely divided diazonium salt is allowed to react immediately with dimethlaniline in the solution in which it was precipitated. Mechanism Diazotization: [pic] Diazo Coupling: Methyl orange is often used as an acid-base indicator. In solutions that are more basic than pH 4.4, methyl orange exists almost entirely as the yellow negative ion. In solutions that are more acidic than pH 3.2, it is protonated to form a red dipolar ion.