How do you make Ethanoic acid?<\/strong><\/h2>\nMaking ethanoic acid<\/strong><\/span><\/p>\n\n- The most common laboratory preparation of a carboxylic acid is by the oxidation of an alcohol.<\/strong><\/li>\n
- The oxidation of ethanol is used to prepare ethanoic acid.<\/li>\n
- This is carried out by refluxing ethanol with an oxidising agent<\/strong> such as acidified potassium dichromate(VI) solution or acidified potassium manganate(VII) solution.
\n<\/li>\n- The reaction is carried out using the set-up of the apparatus as shown below.
\n
\nThe flask is fitted with an upright condenser to prevent the loss of a volatile liquid by vaporisation. This method of retaining a volatile liquid during heating is called refluxing.<\/strong><\/li>\n- During the oxidation of ethanol, the orange dichromate(VI) ions turn to green.<\/li>\n
- The ethanoic acid formed is removed by fractional distillation.<\/li>\n<\/ul>\n
Physical properties of ethanoic acid<\/strong><\/span><\/p>\n\n- Ethanoic acid is a colourless liquid<\/strong> at room conditions. Pure ethanoic acid is known as glacial ethanoic acid.<\/strong><\/li>\n
- It has a sour smell<\/strong> like vinegar.<\/li>\n
- Ethanoic acid is very soluble in water.<\/strong><\/li>\n<\/ol>\n
Chemical properties of ethanoic acid<\/strong><\/span><\/p>\n\n- The chemical reactions of the carboxylic acids can be understood by studying the reactions of ethanoic acid.<\/li>\n
- The reactive site<\/strong> in the carboxylic acids is the carboxyl group, -COOH.<\/strong> This is the group that controls the chemical reactions of the carboxylic acids.<\/li>\n
- Acid properties<\/strong>
\n(a) Ethanoic acid is a weak monoprotic acid.<\/strong> It ionises partially in water to produce a low concentration of hydrogen ions.
\n
\n(b) Only the hydrogen atom in the carboxyl group, -COOH can ionise in water to produce hydrogen ion.
\n(c) Ethanoic acid turns moist blue litmus paper red and reacts just like any typical acid. Unlike strong mineral acids such as sulphuric acid and hydrochloric acid, the weak ethanoic acid reacts slowly with metals, bases and carbonates.<\/li>\n- Reactions with metals
\n<\/strong>(a) Dilute ethanoic acid reacts with reactive metals to produce a salt<\/strong> and hydrogen.<\/strong> Copper and metals below it in the reactivity series cannot react with ethanoic acid.
\n(b) The following equation shows the reaction between zinc and ethanoic acid.
\n
\nA colourless solution of zinc ethanoate is formed.<\/li>\n- Reactions with bases<\/strong>
\n(a) Dilute ethanoic acid neutralises alkalis such as sodium hydroxide solution to give a salt<\/strong> and water.<\/strong> The salt formed is sodium ethanoate.
\n
\n(b) Black copper(II) oxide power dissolves in hot dilute ethanoic acid to form a blue solution of copper(II) ethanoate and water.
\n<\/li>\n- Reactions with carbonates
\n<\/strong>(a) Acids react with metal carbonates to produce a salt, carbon dioxide<\/strong> and water.<\/strong>
\n(b) Ethanoic acid behaves the same way. Reaction between ethanoic acid and calcium carbonate produces a colourless solution of calcium ethanoate and effervescence of carbon dioxide.
\n<\/li>\n- Reactions with alcohols
\n<\/strong>(a) Carboxylic acid reacts with alcohol to form an ester<\/strong> and water.<\/strong> This reaction produces a sweet-smelling compound called an ester. The reaction process is called esterification.
\n<\/strong>
\n(b) When a mixture of ethanoic acid and butan-l-ol with a few drops of concentrated sulphuric acid is heated, an ester called butyl ethanoate is formed.
\n
\n(c) Butyl ethanoate is a colourless sweet-smelling liquid. It forms an oily layer which floats on water.
\n(d) Concentrated sulphuric acid is a catalyst. It helps to speed up the reaction and is not used up in the reaction.<\/li>\n<\/ol>\nChemical properties of ethanoic acid experiment<\/strong><\/h2>\nAim:<\/strong> To investigate the chemical properties of ethanoic acid.
\nMaterials:<\/strong> 1.0 mol dm-3<\/sup> ethanoic acid, 1.0 mol dm-3<\/sup> sodium hydroxide solution, magnesium ribbon, copper(II) oxide, calcium carbonate, iron(III) carbonate, zinc, limewater, glacial ethanoic acid, absolute ethanol, propan-1-ol, concentrated sulphuric acid, water, wooden splint.
\nApparatus:<\/strong> Test tube, stopper with delivery tube, spatula, rubber stopper, Bunsen burner, evaporating dish, dropper, boiling tube, beaker, test tube holder.<\/p>\nA. Reaction of ethanoic acid with a metal<\/strong><\/p>\nProcedure:<\/strong><\/p>\n\n- About 2 cm3<\/sup> of dilute ethanoic acid is placed in a test tube.
\n<\/li>\n- A piece of clean magnesium ribbon is dropped into the test tube.<\/li>\n
- The test tube is closed to collect the gas liberated. The gas is tested with a lighted wooden splint.<\/li>\n
- Steps 1 to 3 are repeated using zinc to replace magnesium.<\/li>\n<\/ol>\n
Observations:
\n<\/strong><\/p>\n\n\n\nMetal<\/strong><\/td>\nObservation<\/strong><\/td>\n<\/tr>\n\nMagnesium<\/td>\n | \n\n- The metal ribbon dissolves to form a colourless solution.<\/li>\n
- Effervescence occurs.<\/li>\n
- The colourless gas produced burns with a ‘pop’ sound.<\/li>\n<\/ul>\n<\/td>\n<\/tr>\n
\nZinc<\/td>\n | \n\n- The metal powder dissolves to form a colourless solution.<\/li>\n
- Effervescence occurs.<\/li>\n
- The colourless gas produced burns with a ‘pop’ sound.<\/li>\n<\/ul>\n<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n
Discussion:<\/strong><\/p>\n\n- Magnesium reacts with dilute ethanoic acid to produce magnesium ethanoate and hydrogen gas.
\n<\/li>\n - Zinc reacts with dilute ethanoic acid to produce zinc ethanoate and hydrogen gas.
\n<\/li>\n<\/ol>\nB. Reaction of ethanoic acid with a base<\/strong><\/p>\nProcedure:<\/strong><\/p>\n\n- About 2 cm3<\/sup> of dilute ethanoic acid is placed in a test tube.
\n<\/li>\n- About 2 cm3<\/sup> of 1.0 mol dm-3<\/sup> sodium hydroxide solution is added to the acid and the mixture is shaken.<\/li>\n
- The mixture is poured into an evaporating dish and heated to dryness.<\/li>\n
- The solid residue is examined.<\/li>\n
- Steps 1 to 4 are repeated using one spatulaful of copper(II) oxide powder to replace 2 cm3<\/sup> of sodium hydroxide solution.<\/li>\n<\/ol>\n
Observations: \n<\/strong><\/p>\n\n\n\nBase<\/strong><\/td>\nObservation<\/strong><\/td>\n<\/tr>\n\nSodium hydroxide solution<\/td>\n | \n\n- A colourless solution is formed.<\/li>\n
- The residue formed is a white solid.<\/li>\n<\/ul>\n<\/td>\n<\/tr>\n
\nCopper(II) oxide<\/td>\n | \n\n- The black powder dissolves to form a blue solution.<\/li>\n
- The residue formed is a blue solid.<\/li>\n<\/ul>\n<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n
Discussion:<\/strong><\/p>\n\n- Sodium hydroxide solution neutralises ethanoic acid to form a salt, which is sodium ethanoate and water.
\n<\/li>\n - Ethanoic acid dissolves copper(II) oxide to produce copper(II) ethanoate and water.
\n \nThe copper(II) ions cause the solution to become blue.<\/li>\n<\/ol>\nC. Reaction of ethanoic acid with a metal carbonate<\/strong><\/p>\nProcedure:<\/strong><\/p>\n\n- About 2 cm3<\/sup> of dilute ethanoic acid is placed in a test tube.
\n<\/li>\n- One spatulaful of calcium carbonate is added to the acid.<\/li>\n
- The test tube is closed with a stopper fitted with a delivery tube dipping into limewater. Any change to the limewater is noted.<\/li>\n
- Steps 1 to 3 are repeated using iron(III) carbonate to replace calcium carbonate.<\/li>\n<\/ol>\n
Observation: \n<\/strong><\/p>\n\n\n\nMetal carbonate<\/strong><\/td>\nObservation<\/strong><\/td>\n<\/tr>\n\nCalcium carbonate<\/td>\n | \n\n- The white powder dissolves to form a colourless solution.<\/li>\n
- Effervescence occurs.<\/li>\n
- The colourless gas produced turns limewater milky.<\/li>\n<\/ul>\n<\/td>\n<\/tr>\n
\nIron(III) carbonate<\/td>\n | \n\n- The reddish-brown powder dissolves to form a brown solution.<\/li>\n
- Effervescence occurs.<\/li>\n
- The colourless gas produced turns limewater milky.<\/li>\n<\/ul>\n<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n
Discussion:<\/strong><\/p>\n\n- Calcium carbonate reacts with dilute ethanoic acid to produce calcium ethanoate, water and carbon dioxide.
\n<\/li>\n - Iron(III) carbonate reacts with ethanoic acid to produce iron(III) ethanoate, water and carbon dioxide.
\n \nThe iron(III) ions make the salt solution brown.<\/li>\n<\/ol>\nD. Reaction of ethanoic acid with alcohol<\/strong><\/p>\nProcedure: \n \n<\/strong><\/p>\n\n- About 2 cm3<\/sup> of glacial ethanoic acid is poured into a boiling tube.<\/li>\n
- About 2 cm3<\/sup> of absolute ethanol is added to the acid.<\/li>\n
- The boiling tube is shaken to mix the liquids well.<\/li>\n
- A dropper is used to add about 1 cm3<\/sup> of concentrated sulphuric acid to the mixture. The boiling tube is shaken well.<\/li>\n
- The mixture is carefully heated over a small flame. The mixture is allowed to boil gently for about 2 to 3 minutes.<\/li>\n
- A beaker is half-filled with some water.<\/li>\n
- The contents of the boiling tube are poured into the beaker.<\/li>\n
- Any change that occurs is observed.Steps 1 to 7 are repeated using butan-1-ol to replace absolute ethanol.<\/li>\n<\/ol>\n
Observations: \n<\/strong><\/p>\n\n\n\nAlcohol<\/strong><\/td>\nObservation<\/strong><\/td>\n<\/tr>\n\n | | | | | | | | | | | | | |