hydroxide. Monoprotic (x=1): HCl (aq) + NaOH (aq) → H2O (l) + NaCl (aq) Diprotic (x=2): H2SO4 (aq) + 2 NaOH (aq) → 2 H2O (l) + Na2SO4 (aq) Triprotic (x=3): H3PO4 (aq) + 3 NaOH (aq) → 3 H2O (l) + Na3PO4 (aq) Any acid with more than one proton (hydrogen) is called a polyprotic acid. Citric acid is a weak‚ polyprotic acid that undergoes the following reaction with sodium hydroxide: H3C6H5O7 (aq) + 3 NaOH (aq) → 3 H2O (l) + Na3C6H5O7 (aq) You will perform
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equals amount of base) of the titration. This was then titrated to the end point (the indicator’s colour change) with .1M sodium hydroxide (NaOH) to discover how much base was required to neutralize the acid (Table 1). This required volume of NaOH was used in calculations to discover the neutralizing capacity of the antacid. Table 1 – NaOH Required to Neutralize
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volumetric flask ±0.30cm3 Electronic Balance ±0.10g 50cm3 Burette±0.1cm3 25cm3 Pipette±0.06cm3 Materials: 0.20M HCl (±0.02moldm-3) 1.1g solid NaOH (±0.1g) A solution of vinegar of unknown concentration (density= 1.05gcm-3) Phenolphthalein Method: * A solution of NaOH was prepared by dissolving 1.1g in 250cm3 of water * 1.1g of solid NaOH was weighed and then dissolved in the stirred until dissolved in 250cm3 of water * 25cm3 of this solution was placed into a conical flask and
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in a vinegar solution and compared to the standard value for % acid present in vinegar. The second part of the experiment was to see if by titrating a solution of NaOH and an unnamed mystery acid‚ you could find the molar mass of the unknown acid (solving the mystery). It must be understood that the number of moles of the reacting NaOH and the number of moles of the product NaX acid‚ must both equal (in this case 1:1) in order for the calculation to find the molar mass to work. Procedure: Begin
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iii)Titration for normality of NaOH * take 20ml of NaOH solution in 100ml conical flask add 1 drop of phenolphthalein * the colour changes to pink colour * take oxalic acid in 50ml burette and titrate against NaOH solution .The end point is the appearance of pale permanent pink colour. Formula for normality Normality of NaOH=(burette reading*strength of oxalic acid)/20ml of NaOH Strength of oxalic acid=amount of OXALIC ACID(gm)* amount of NaOH /mol.wt of oxalic acid PROCEDURE
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Experiment N | Kinetics of the Depolymerization of Diacetone Alcohol via Basic Catalysis | | Ingrid Tafur -5672578 | 2/11/2011 | CHM233O Partner: Laura Marrongelli Demonstrator: Cheryl McDowall Objective The rate constant of the depolymerization of diacetone alcohol via basic catalysis was determined by monitoring the change in volume as a function of time at constant temperature of a pseudo first order reaction where the species in excess was sodium hydroxide. This was accomplished
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1 1 1 1 1 1 1 Procedures 1. Dilute both solutions H2SO4 and NaOH‚ from the given concentration to 1M and 2M. The volumes of the diluted solutions H2SO4 and NaOH with concentration 1M are 90ml which contains 0.09 moles H2SO4 and 60 ml which contains 0.06 moles NaOH respectively. And the volumes of the diluted solutions H2SO4 and NaOH concentration 2M are 45ml which contains 0.09 moles H2SO4 and 60 ml which contains 0.12 moles NaOH respectively. 2. Package the constant temperature tank. Insert the
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different acids is needed to neutralize 25mls of sodium hydroxide solution (NaOH). Hypothesis: The strongest alkali will need the smallest amount of an acid to cancel out and the weakest will need more acid. Variables: Control | Independent | Dependent | The indicator‚ NaOH | H2SO4 HClHNO3 | The chemical reaction between the acids and alkali. | Materials / Apparatus: * H2SO4 * HCL * HNO3 * Alkali (NaOH) * Stand * Burette * Beaker * Funnel * Bunsen Burner
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molar ratio. If a solution of NaOH of known concentration will used titrate vinegar‚ it is possible to determine the amount of acetic acid. The main three things from this experiment are: to determine the concentration of vinegar‚ to verify the description on the product labels‚ practice the chemical testing technique of titration. The balanced chemical equation for the neutralization of acetic acid with NaOH is: Safety notes: Wear safety glasses and if available. NaOH is corrosive to flesh and can
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hydroxide (NaOH) pellets Potassium acid phthalate (HKC8H4O4) Phenolphthalein Soft drinks samples B. Apparatus 250-ml beaker 250-ml Erlenmeyer flask 100-ml volumetric flask 50-ml buret 10-ml pipet buret holder Stirring rod triple beam balance Bunsen burner Iron stand and ring wire gauze III. Schematic diagram of the procedure IV. Data and Observations Table 1.1. Preparation of the Sodium hydroxide solution Mass before standing Mass after standing Beaker (g) beaker and NaOH pellets(g)
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