Form 4 Chapter 7: Acid and Bases

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1 Form 4 Chapter 7: Acid and Bases The ph Scale Properties Acids Alkalis Physical. Substances that ionized in water to produce hydrogen ions.. Sour taste.. Turn blue litmus paper red. 4. Give a ph value of less than Show acid properties when dissolved in water. 5. Not corrosive. Chemical. Acid + Base Salt + Water. Acid + Reactive Metal Salt + Hydrogen Gas. Acid + Carbonate Salt + Water + Carbon Dioxide **Strong Acids Completely ionized in water to produce high concentration of hydrogen ions (example: nitric, hydrochloric / sulphuric acid) with low ph around or.. Their reactions are irreversible.. Monoprotic: (a) HCl (aq) H + (aq) + Cl - (aq) (b) HNO (aq) H + (aq) + NO (aq). Diprotic: HSO4 (aq) H + (aq) + SO4 - (aq) (a) The above HSO4 has completely been ionized in water forming: (i) H + ions (double concentration) (ii) SO4 - ions. Soluble bases that dissolved in water to produce OH -.. Bitter taste and soapy feel.. Turn red litmus paper blue. 4. Give a ph value of more than 7.. Alkalis + Acid Salt + Water. Alkalis + Ammonium Salt Salt + Water + Ammonia Gas **Strong Alkalis Ionized completely in water (example: NaOH, KOH). **Weak Alkalis Partially ionized in water (example: ammonia).. Low concentration of hydroxide ions, the ph value high.

2 (iii) HO molecules 4. React more vigorously with metals than weak acids hydrogen gas bubbles are produced rapidly. **Weak Acids Partially ionized in water to produce the low concentration of hydrogen ions (example: ethanoic acid) with high ph around 5 or 6.. Phosphoric acid, carbonic acid.. The remaining molecules remain unchanged as acids.. Their reactions are reversible. 4. CHCOOH (aq) CHCOO - (aq) + H + (aq) 5. HPO4 (aq) H + (aq) + PO4 (aq) 6. Weak acids react slowly with metals than strong acids hydrogen gas bubbles are produced slowly.. Add acid to alkali will release heat to the surrounding.. Particle presence in glacial ethanoic acid is molecule. Glacial ethanoic acid (example: vinegar) shows acidic properties only when it is dissolved in water. When glacial ethanoic acid dissolves in water, it can conduct electricity and change the colour of litmus paper. *Silver Nitrate Solution Aim: To confirm the predictions on the metal displacement reaction. Problem statement: How to confirm the predictions on the metal displacement reaction? Hypothesis: If the metal displacement reaction occurs, then there is a change of colour of the solution or a precipitation of metal. Variables: Manipulated variables: Pairs of metal and salt solution used Responding variable: Precipitation of metal or change of colour of solution Controlled variable: Concentration of salt solution Materials: 0. mol dm silver nitrate solution, 0. mol dm potassium nitrate solution, 0. mol dm tin(ii) nitrate solution, copper strip, magnesium ribbon, iron nail and sandpaper.

3 Apparatus: Test tubes and test tube rack. Procedure:. Silver nitrate solution, potassium nitrate solution and tin(ii) nitrate solution are poured into three separate test tubes, X, Y and Z, until they are half full.. Pieces of copper strip, magnesium ribbon and iron nail are cleaned with sandpaper and placed in different salt solutions in the test tubes as shown in figure below.. The reactions (if any) are allowed to take place for five minutes. 4. Any change in the colour of the solutions and whether any metals are deposited are observed. Results: Test Tube X Y Z Prediction Copper is above silver in the electrochemical series. Thus, copper will displace silver from silver nitrate solution. Magnesium is below potassium in the electrochemical series. Thus, magnesium will not displace potassium from potassium nitrate solution. Iron is above tin in the electrochemical series. Thus, iron will displace tin from tin(ii) nitrate solution. Observation The copper strip dissolves. A shiny grey solid is deposited. The colourless solution turns blue. No visible change. The iron nail dissolves. A shiny grey solid is deposited. The colourless solution turns light green. Discussion:. Test tube X: The shiny grey solid is silver metal. The colourless solution turns blue because the copper(ii) ions have been released into the solution. The equation for the reaction is:

4 The prediction is correct. The metal displacement reaction occurs.. Test tube Y: The prediction is correct. The metal displacement reaction does not occur.. Test tube Z: The shiny grey solid is tin metal. The colourless solution turns light green because the iron(ii) ions have been released into the solution. The equation for the reaction is: The prediction is correct. The metal displacement reaction occurs. Conclusion: The ability of a metal to displace another metal from its salt solution can be predicted using the electrochemical series. The prediction can be confirmed through an experiment. The hypothesis is accepted. Concentrations of Acids and Alkalis Definition: The amount of substance in water. Important Formulae: - Mass of solute (g) Concentration, g dm Volume of solution (dm ) - Number of moles of solute (mol) Molarity, mol dm Volume of solution (dm ) Number of moles MV 000, wherem molarity in mol dm - ; V volume in cm Dilution Equation: MV M V M = Concentration of solution before dilution V = Volume of solution before dilution M = Concentration of solution after dilution V = Volume of solution after dilution Neutralisation Examples: Acid + Base Salt + Water 4

5 Application of Neutralisation in Daily Life Health Magnesium hydroxide in toothpaste neutralises the organic acids produced by bacteria in gaps between teeth. Antacid (which contains calcium carbonate and calcium bicarbonate) and milk of magnesia (which contains magnesium hydroxide) can neutralise the hydrochloric acid in the stomachs of gastric patients. Vinegar (weak acid) is used to apply on insect bites / jelly fish stings (alkaline stings) because strong acid like H SO 4 will burn our skin. This is because after the alkaline poison is neutralised by acid, the pain will lessen. Vinegar is not corrosive and does not produce a lot of heat when neutralise. Agriculture Lime (consisting of calcium oxide) which produces calcium hydroxide in water is used to neutralise acidic soil. Industries Ammonia is used to neutralise the organic acids produced by bacteria so that latex can remain in the liquid state. Neutralisation reactions are also used in industry to produce manufactured products such as fertilizers, soaps and detergents. Engineering Dilute hydrochloric acid is used to remove the oxide layer on the surface of steel used to make the body of the car. A metal oxide is a base. Experiment: To prepare 00cm of mol dm aqueous NaOH solution Apparatus: Volumetric flask (00 cm ), electronic balance, dropper, glass rod, beaker, filter funnel. Materials: Sodium hydroxide pellets, distilled water in bottle. Procedure: 5

6 . The mass of sodium hydroxide pellets required is as follows: MV 00 n RMM g g of sodium hydroxide in a beaker is weighed on an electronic balance (the beaker is weighed first before adding on the alkali).. Volume of distilled water and mass of NaOH is measured accurately in order to prepare the standard solution. 4. Some distilled water is added to the alkali in the beaker and stirred to dissolve all the NaOH pellets. 5. The solution is poured into the volumetric flask through a clean filter funnel, along the glass rod to prevent spillage. 6. Distilled water is added to the beaker and washed down into the volumetric flask to ensure that there is no wastage. This step is repeated a few times. This is to make sure that all NaOH is transferred into volumetric flask. 7. Distilled water is added into the volumetric flask until it is slightly below the 00 cm mark. Using a dropper, distilled water is added until it reaches the 00 cm mark. (Caution: Do not add water too quickly from a beaker as it may exceed the 00 cm level!) 8. The flask is closed with its cover to prevent contaminants from entering the flask and evaporation of solution and shaken gently to obtain a homogeneous solution. 9. A volumetric flask has been specially calibrated to be more accurate than a beaker and more suitable to be used in the preparation of standard solution. 0. Substance Meaning Standard Solution in which its concentration is accurately Solution known. Concentration It is the amount of the solute (sodium hydroxide) in grams that is dissolved in.0 dm of distilled water. Molarity The number of moles of sodium hydroxide dissolved in.0 dm of distilled water. Conclusion: The concentration (molarity) of the sodium hydroxide solution is mol dm. Acid-Base Titration Experiment: To determine the end point of neutralisation through titration Procedure:. 5 cm of sodium hydroxide solution is transferred into the conical flask using a pipette. drops of phenolphthalein are added to it.. Acid is poured into the burette using a filter funnel.. The apparatus is set up as shown in the diagram. The first reading on the burette 6

7 is recorded. 4. The acid is allowed to flow a little at a time into the alkali. The conical flask is shaken constantly and the colour of the solution is checked. The end point is obtained when the colour changes suddenly from pink to colourless. The reading on the burette is recorded as the final reading. 5. Steps - 4 are repeated twice more, using a fresh solution of NaOH each time, this time slowing down at the end point by adding acid drop by drop. (This is to ensure a more accurate result.) Results / Calculations: The average volume of acid used is: 0.05cm. Therefore, 0.05 cm H SO4 of molarity M is needed to neutralise 5 cm NaOH,.0 mol dm. The reaction between the acid and alkali is: HSO4 NaOH NaSO4 HO That is, mole of acid neutralises moles of alkalis.. The number of moles of acid, n, is: MV n [ M : molarity of acid ; V = volume of acid] The number of moles of alkali, n, is: M V n [ M : molarity of alkali ; V = volume of alkali] 000 n MV 5. Thus, n M V n M V M ; [ n = mole of acid; n = moles of alkali] n V mol dm 0.05 Discussion:. The burette should be washed with distilled water followed by acid to ensure that water does not dilute the acid. Similarly too, the pipette should be washed with distilled water, followed by alkali.. The conical flask should not be washed with alkali to ensure that no alkali remains in the flask before NaOH is added.. The end point is the point at which a drop of acid added to the mixture in the. 7

8 conical flask will change the indicator's colour from pink to colourless. The indicator is phenolphthalein. 4. The conical flask becomes warm / hot after experiment. Conclusion: The molarity of sulphuric acid used to neutralise 5 cm of.0 mol dm NaOH is 0.6 mol dm. The concentration of hydroxide ions / OH decreases with time. 8

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