Acid-Base Extraction: Separation of an Organic Acid‚ Base and a Neural Compound Introduction/Background Acid base extraction is a widely used commercial method in separating acids‚ bases and neutral compounds. This is concept is based on several physical properties of the compounds‚ such as boiling point‚ melting points and solubility. The different solubility properties of the protonated and non-protonated forms of these compounds depend on the functional groups present‚ such
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Acids And BAses Acids And BAses 8.1 8.2 8.3 8.4 18.1 18.2 18.3 18.4 18.5 Theories of acids and bases Properties of acids and bases Strong and weak acids & bases The pH scale Calculations involving acids and bases (AHL) Buffer solutions (AHL) Salt hydrolysis (AHL) Acid-base titrations (AHL) Indicators (AHL) 8 8.1 THeORies OF Acids And BAses 8.1.1 Define acids and bases according to the Brønsted–Lowry and Lewis theories. 8.1.2 Deduce whether or not a species could act as a Brønsted–Lowry
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E XPE RIME NT 4 . 5 Reactions of acids Aim To investigate and compare some reactions of a strong acid‚ hydrochloric acid‚ and a weak acid‚ ethanoic acid (common name‚ acetic acid) Equipment Dropper bottles containing: • 0.1 M hydrochloric acid‚ HCl • 0.1 M ethanoic acid (acetic acid)‚ CH3COOH • 0.1 M sodium hydroxide‚ NaOH • 1 M hydrochloric acid‚ HCl • 1 M ethanoic acid (acetic acid)‚ CH3COOH • universal indicator solution • limewater (calcium hydroxide‚ Ca(OH)2) Marble chips (calcium carbonate
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Essay March 28‚ 2014 ACID RAIN ENVIRONMENAL EFFECTS What is acid rain? It’s a rain or any other form of precipitation that is unusually acidic‚ meaning that it possesses elevated levels of hydrogen ions (low pH). It can have harmful effects on plants‚ aquatic animals and infrastructure. Acid rain is caused by emissions of sulfur dioxide and nitrogen oxide‚ which react with the water molecules in the atmosphere to produce acids. The most obvious environmental effect of acid rain has been the loss
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TITLE : * Analysis of an unknown acetic acid solution OBJECTIVES : * To prepare the sodium hydroxide solution‚ NaOH * To standardise the base against potassium hydrogen phthalate * To analyse the unknown acetic acid RESULTS : A. Preparation of the sodium hydroxide solution Volume of NaOH taken from the stock solution = 3.33 mL B. Standardisation of the base against potassium hydrogen phthalate | 1 | 2 | 3 | Weight KHP | 1.0000 | 1.0004 | 1.0006 | Final volume
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Separation of a Carboxylic Acid from a Neutral Compound by Extraction Reference: Smith‚ Chapter 2 (Acids and Bases) Introduction Carboxylic acids and phenols are two families of organic compounds that contain carbon‚ hydrogen and oxygen‚ and also react with water to yield an excess of hydronium ions over hydroxide ions. Pure water has a pH of 7‚ which means it has a hydronium ion concentration‚ [H3O+] of 10-7 M (M = molarity‚ moles/Liter). The hydronium ions in pure water come from the self-ionization
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Chapter 10 ComMon Acids and Alkalis 10.1 Acids and Alkalis 1. Acids taste sour. Many fruits contain acids. 2. The three mineral acids commonly found in the laboratory are hydrochloric acid‚ sulphuric acid and nitric acid. 3. Alkalis taste bitter and feel soapy or slippery. 4. The common alkalis found in the laboratory are sodium hydroxide solution‚ potassium hydroxide solution‚ calcium hydroxide solution and ammonia solution. 10.2 Acid-Alkali Indicators 1. An acid-alkali indicator
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Acids and Bases Are Everywhere Every liquid you see will probably have either acidic or basic traits. Water (H2O) can be both an acid and a base‚ depending on how you look at it. It can be considered an acid in some reactions and a base in others. Water can even react with itself to form acids and bases. It happens in really small amounts‚ so it won’t change your experiments at all. It goes like this: 2H2O --> H2O + H+ + OH- --> H3O+ + OH- See how the hydrogen ion was transferred? Most of the
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Worksheet - Acids‚ Bases and Salts 1. I am pure water. When heated my pH (increases‚ decreases)‚ because more of my water molecules dissociate. 2. I am a 0.020 M solution of weak acid‚ HA. If I only dissociate to the extent of 1.50%‚ what is the value of my Ka? 3. I am a 0.20 M solution of hydrocyanic acid‚ HCN‚ with a Ka of 4.93 x 10¯ 10 . What is my pH? 4. I am a buffer made from 0.10 M acetic acid and 0.15 M sodium acetate. If the Ka for acetic acid is 1.77 x 10¯ 5 ‚ what is my pH? 5. I am
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solution of an acidic and organic compound and purify its respective acidic product through the techniques of an acid base extraction‚ recrystallization‚ and use of Melt Temp (melting point range). The reaction of an unknown acid (3-chlorobenzoic acid) with diethyl and sodium hydroxide was observed‚ and the solution naturally separated into an aqueous and organic solution. The mixture of acid and organic solution was created and then separated through the Hirsch funnel into separate beakers of an aqueous
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