________________________ Internal Assessment Criteria Aspect 1 Aspect 2 Aspect 3 Total DCP CE Aim: The aim of this practical is to plot and investigate the pH titration curves for the titration of a strong acid with a strong base and of a weak acid with a strong base‚ and find Ka of the weak acid. Procedure: Part I 1. Pour 30 ml of the HCl solution of unknown concentration in a 100 ml beaker. 2. Add a stirring magnet. 3. Place the beaker on the magnetic heater and activate the rotating motor
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Preparation of Sodium Chloride through titration Abstract: acid-base titration is a technique commonly used to determine the moles of acid in a sample by adding a known volume of strong base of a known concentration. The strong base provides the hydroxide ion‚ to react quantitatively with the acid. The point at which the acid is completely and exactly consumed the known quantity of base is called the equivalence end point and is signalled by a colour change in the solution (end point). This colour
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experiment‚ the primary standard is oxalic acid dihydrate‚ H2C2O4 ( 2H2O. It will be used to standardize a solution of sodium hydroxide. Sodium hydroxide solutions pick up carbon dioxide from the air. This contamination can affect the strength of the base solution and can spoil the sharpness of the end point in the titration. The procedure below is designed to prepare and standardize carbonate-free NaOH. Equation 2 NaOH(aq) + H2C2O4 ( 2H2O(s) ( Na2C2O4(aq) + 4 H2O(l) PROCEDURE
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O R-C-O-R’ + NaOH ---- R-C-O-Na+ + R’OH Ester(fat) + base(caustic soda) ---- salt of fatty acid(soap) + alcohol(glycerol). Caustic potash (potassium hydroxide) can be used instead of caustic soda (sodium hydroxide)but is more expensive. The base used to come from wood ash containing potassium carbonate which formed potash as this was not plentiful it made soap a luxury. The cheapest source of the
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have a molar concentration of .5 however when we standardized the solution we found the actual molarity of the solution to be .4761. This may be due to the fact that NaOH is almost impossible to have pure because it reacts with CO2 in the air. Strong bases are generally very reactive and it makes it hard to have a pure solution of NaOH
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In the experiment preformed the objective is to titrate a weak acid with a strong base. In a titration of a weak acid with a strong base the titrant is the strong base and the analyte is a weak acid. The reaction that will occur is the direct transfer of protons from the weak acid to the hydroxide ion. The data gathered will be represented on the titration curve‚ a graph of the volume of titrant being the strong base plotted against the pH .The pH is an indicator of an acids strength. The titration
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involved a double displacement reaction 3. The addition of zinc sulfate to potassium chromate formed a yellow coloured solution and when base was added‚ the solution turned into a bright yellow colour. This was difficult to observe as the colour change was very subtle‚ however‚ interpretation was manageable as pH paper was used to find when the addition of base should be stopped. Chromium oxide green was synthesized from the reaction between potassium dichromate and sulfur. The reaction involved
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Discussion The second experiment of the semester focuses on separating and identifying the components of Panacetin‚ which is a common medication that relieves pain. The label reveals that Panacetin is composed of sucrose (10%)‚ aspirin (40%)‚ and Tylenol (50%). Although this information is reported‚ the true composition of Panacetin is questionable. While sucrose and aspirin are present in Panacetin‚ Tylenol may be replaced by an unknown component (acetanilide or phenacetin). Separation of the components
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Introduction: The purpose behind (the first step in) this experiment is to show that similarly to week 1‚ the molarity of an acid or base in solution can be determined (so long as one value’s is known) using titration. In this case though‚ finding the molarity of the acid used in the reaction is then used to determine the percent of that acid 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
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concentration of an acetiuc acid solution. In this case the concentration of vinegar‚ which is diluted acetic acid. Hypothesis: The sodium hydroxide used in this titration would balance out the acetic acid in vinegar. The phenolpthalein‚ a acid –base color indicator will let us know the vinegar have reach a point of neutralization once the vinegar turns pink. We can then calculate the concentration of acetic acid in the vinegar. Procedure: Data: Set up the lab: Take a tick text book and place
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