1. Gather all the equipments needed. 2. Measure 50ml of HCL in a 250 ml measuring cylinder and pour it into a flask‚ then measure 50ml of HCL again and pour it into the second flask. 3. Measure the 50ml of KOH in a measuring cylinder. Repeat it again in another measuring cylinder. 4. Attach both of the burette clamps to both of the burette stands and clamp the burette at a certain level so that it can fit a flask underneath. 5. Then‚ place a funnel on top of each burette. 6. Place a flask underneath
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Chemistry Coursework – Titration Background Science A titration is the neutralisation of an acid or an alkali. To achieve this‚ one must be added to the other in a specific amount‚ strength and concentration. A substance is neutral when its pH is 7. It is most acidic closer to 0 and is most alkaline closer to 14. 28492453194050 0 7 14 595423979670
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Contents 1. Introduction 2 2. Concrete attacks 2 3. Alkali-Silica Reaction – ASR 3 4. Sulphate Attack 5 5. Reference List 8 1. Introduction This report was issued in order to provide an in depth understanding of how a surveyor can differentiate between Alkali-Silica Reaction and Sulphate attacks in concrete when inspecting a building. In order to satisfy the requirements for this report‚ the author will give a detailed description of both kind of attacks‚ different study areas
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Solubility Rules Chart Negative Ions (Anions) + Positive Ions (Cations) = Solubility of Compounds in water Example any anion + Alkali Ions (Li+‚ Na+‚ K+‚ Rb+‚ Cs+‚ Fr+) = soluble Sodium fluoride‚ NaF‚ is soluble any anion + hydrogen ion [H+ (aq)] = soluble hydrogen chloride‚ HCl‚ is soluble any anion + ammonium ion (NH4) = soluble ammonium chloride‚ NH4Cl‚ is soluble nitrate NO3- + any cation = soluble potassium nitrate‚ KNO3‚ is soluble acetate (CH3COO-) + any cation (except
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Vinegar is an acid and there fore can be neutralised by an alkali. Acid + Alkali à salt + water Hydrochloric acid + Sodium Hydroxide à Sodium chloride + water Vinegar is a weak acid and therefore it only partially ionises in solution. CH3COOH ßà CH3COO- + H+ An alkali such as Sodium Hydroxide has a formula NaOH. If the alkali is strong then it ionises fully in solution. NaOH ßà Na+ + OH- When the acid H+ reacts with the alkali OH- the solution neutralises. Prediction: If
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Acids * sour taste * able to conduct electricity * corrosive if concentrated * able to react with metals‚ carbonate compounds & bases/alkalis* * able to turn blue litmus paper red Reactions of Acids 1. Acid + Metal Salt + Hydrogen 2. Acid + Carbonate Salt + Carbon Dioxide + Water 3. Acid + Base/Alkali Salt + Water (Neutralisation) Note: Salts formed always takes the cation (positive ion which is usually a metal) + name of acid. e.g. : Sulphuric acid
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range of C3A contents (6.0 to 11.8%) and SO3 contents (0.09 to 2.90%)‚ made with clinkers having a wide range of alkali contents (0.07 to 0.87% of Na2Oeq)‚ have been selected to highlight the key cement factors that control the compatibility between ordinary Portland cements and the naphthalene-based superplasticizers. The soluble alkalis (in fact the soluble SO4 2- ions from alkalis)‚ the fineness‚ the C3A content‚ and the type of CaSO4 of the cement are among the key cement factors that control
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BRONSTED-LOWRY ACIDS AND BASES 1. The Bronsted-Lowry definition There are many definitions of acids and bases in existence‚ but the most useful one is the Bronsted-Lowry definition: An acid is a substance which can behave as a proton (re presented as a hydrogen ion‚ H+) donor. Any substance which contains hydrogen bonded to a more electronegative element can thus behave as an acid: HCl == H+ + Cl- H2SO4 == H+ + HSO4- A base is a substance which can behave as a proton acceptor. Any
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Substances that neutralize acids are called alkalis. An acid is a substance that forms hydrogen ions (H+ ) when placed in water. It can also be described as a proton donor as it provides H+ ions. An example of an acid is hydrochloric acid (HCl)‚ Sulphuric acid (H2SO4) etc. An alkali is a soluble base and forms hydroxyl ions (OH-) when placed in water. It can be called a proton acceptor and will accept hydrogen ions to form H2O. An example of an alkali is Sodium Hydroxide (NaOH). Neutralization
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PH changes during a titration experiment. Concentration of the alkali Having a higher concentration of alkali will mean that there will be more molecules closer together for the acid to collide with. This will speed up the reaction as collision theory suggests that molecules have to collide to react and if there are more molecules to collide with the reaction will happen faster as there is a higher chance of a collision. Volume of alkali An increase in volume would mean that the neutralisation would
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