9 Experiment A Volumetric Analysis A titrimetric analysis requires the careful addition of titrant. • To prepare and standardize a sodium hydroxide solution • To determine the molar concentration of a strong acid Objectives The following techniques are used in the Experimental Procedure Techniques 2 4 16b 16a 90 80 5 16c 6 13c 15a 15b ! A chemical analysis that is performed primarily with the aid of volumetric glassware (e.g.‚ pipets‚
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negatively charged hydroxide ion (OH-) in water. *The strength of a base is determined by the concentration of Hydroxide ions (OH-). The greater the concentration of OH- ions the stronger the base. Example: NaOH (Sodium Hydroxide-a strong base) in water **Solutions containig bases are often called alkaline. Characteristics of Bases: **Bases taste bitter **Bases feel slippery **Strong bases are very dangerous and can burn your skin Examples: 1. lye (Sodium Hydroxide) 2. Ammonia
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(aq) + H2O (l) ) Question= Neutralization reactions typically occur between a strong acid and a strong base to produce a salt and water question When sodium carbonate (Na2CO3) dissolves in water‚ it partially ionizes. The carbonate (CO3-) ion takes up a hydrogen ion and forms HCO3-. What type of substance is sodium carbonate? Answer (weak base Questio Which of the following correctly describes the corrosive nature of strong acids and strong bases? Strong acids and strong
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CHEMISTRY DETERMINATION OF ENTHALPY CHANGE OF NEUTRALIZATION IA Criteria Assessed: DCP CE MS Introduction When an alkali neutralizes an acid‚ a salt and water are formed. Aqueous hydrogen ions (H+(aq)) from the acid react with the hydroxide ions (OH- (aq)) from alkali‚ forming water. The identity of salt will depend on the nature of the acid and alkali used. H+(aq) + OH- (aq) → H2O(L) The combination of H+ and OH- ions in this way releases energy. In this practical‚ the enthalpy
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substance as acidic‚ neutral or basic. Materials: * Distilled water * 250ml beaker X2 * Test tube X9 * Tripod * Wire Gauze * Bunsen burner * Safety goggles Test Object: * Hydrochloric acid (HCl) * Sodium hydroxide (NaOH) * White Vinegar * Lemon Juice * Baking soda (NaHCO3) * Hair conditioner * Shampoo * Hand soap * Cloudy Ammonia * Dish washing detergent Method: 1) Tear off leaves from the cabbage and tear them
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4/2/14 Period: 1st Chemistry Sour Acids and Bitter Bases Purpose: The purpose of this lab was to observe the different reactions formed between various acids and bases with the aid of indicators. Equipment: 1. Safety goggles. 2. Droppers. 3. Red Litmus paper. 4. Blue Litmus paper. 5. pH paper. 6. Well plate. 7. Micro spatula. Materials: 1. Zinc. 2. Magnesium. 3. Iron. 4. Copper. 5. HCL. 6. HC₂H₃O₂. 7. NaOH. 8. Phenolphthalein. Procedure: Part A: 1. Add five drops
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the final few millilitres of distilled water. 8. Stopper the flask and invert several times to mix the contents and thereby ensure the solution is of uniform concentration throughout. Standardisation of Sodium Hydroxide 1. Prepare the burette and fill with the sodium hydroxide solution to 50ml. 2. Pipette the KH(C8H4O4) solution into a conical flask. Use three drops of phenolphthalein as the indicator. 3. Titrate carefully until a colour change from colourless to pink is observed
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High School Department Effect of Crab Shells and Acacia Seeds In Purifying Water In Partial Fulfillment of the Requirements in BIOLOGY 1st Quarter Submitted by: Submitted to: I. STATEMENT OF THE OBJECTIVES To determine if the purified water is safe to drink and not cause complications when drinking the purified water. To establish if crab shells and acacia seeds can purify water To identify what specie of crab can purify the water better To know if
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concentration Method: You will need: * Solution of ‘acid rain’ (dilute sulphuric acid) * Sodium hydroxide solution‚ 0.1mol dm-3 * 250cm3 conical flask * 10cm3 pipette and filler * Burette * Phenolphthalein indicator. * Clamp * Funnel * White tile (to help reading endpoint) Firstly prepare your burette‚ your burette should be filled with 0.1mol dom-3 of the sodium hydroxide solution. When filling a burette‚ close the stopcock at the bottom and use a funnel. Check
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ACID BASE TITRATION OBJECTIVES 1. To demonstrate the basic laboratory technique of titration 2. To learn to calculate molarity based on titrations INTRODUCTION Molarity (M) or molar concentration is a common unit for expressing the concentration of solutions. It is defined as the number of moles of solute per liter of solution (or millimoles of solute per milliliter of solution). The concentration of a basic solution can be determined by titrating it with a volume of a standard acid solution (of
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