(2) To specifically use solution stoichiometry to determine the percent of acetic acid in vinegar. (3) To prepare a standard solution by the method of titration. Consider the following balanced chemical equations: (1) HCl + NaOH ------> NaCl + HOH (2) H2SO4 + 2NaOH --------> Na2SO4 + 2HOH (3) 2HCl + Ca(OH)2 ---------> CaCl2 + 2HOH (4) H2SO4 + Ca(OH)2 ---------> CaSO4 + 2HOH (5) 2H3PO4 + 3Ca(OH)2 ----------> Ca3(PO4)2
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concentration of acetic acid in a sample of vinegar by titrating it with a standard solution of NaOH. CH3COOH(aq) + NaOH(aq) -> CH3COONa(aq) + H2O(l) By adding the sodium hydroxide‚ which is a basic solution‚ to the acetic acid‚ which is an acidic solution‚ a neutralization reaction occurs. An indicator known as phenolphthalein‚ is also added to the vinegar. This indicator turns the solution to a dark pink when excess NaOH is added
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determine the percentage by mass of aspirin aspirin present in different commercial preparations and to find out‚ which the best value is‚ using a neutralization reaction followed by a direct titration with NaOH. Chemicals Used: 100 ml of distilled water in a wash bottle 50 ml of 0.100 M NaOH 40 mL of 96% ethanol phenolphthalein as an indicator (3 drops per titration) 325 mg non buffered aspirin tablets Materials Used: One spatula Two Erlenmeyer flasks‚ 250 ml One weighing scale (with uncertainly
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leaks. The ring stand is then set up with a buret clamp and the cleaned buret placed in it. Then the buret is filled with 5-10mL of sodium hydroxide‚ M .0466 NaOH‚ three times and emptied after each time to completely rinse the buret. The buret is now filled will NaOH until it reads at the 0.00mL mark on the buret. The initial volume of NaOH in the buret is then recorded into lab books for future reference. The soda must now be readied for titration. Both sodas require the same set up. The
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Volume of NaOH Needed to Neutralize 10.00 ml of Unknown HCl Molarity of NaOH= Trial 1 Trial 2 Trial 3 Trial 4 Trial 5 Initial volume of NaOH (ml) Final volume of NaOH (ml) Volume of NaOH used Average volume of NaOH Part II Determination of Percentage Composition of Vinegar Table 2 Volume of NaOH Needed to Neutralize 10.00 ml of Vinegar Molarity of NaOH= Trial 1 Trial 2 Trial 3 Trial 4 Trial 5 Initial volume of NaOH (ml) Final volume of NaOH (ml) Volume of NaOH used
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Volumetric Analysis The purpose of this experiment is to determine the [NaOH] of a solution by titrating it with standard HCl solution‚ to neutralize a known mass of an unknown acid using the NaOH solution as a standard‚ to determine the moles of NaOH required to neutralize the unknown acid‚ and to calculate the molecular mass of the unknown acid. Procedure: Part A: Standarized 0.10M HCl solution and unknown NaOH solution were poured into two beakers. The burets were then filled with the
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|[pic] | | | | |UNIVERSITI TEKNOLOGI MARA | | | |FAKULTI KEJURUTERAAN KIMA | | | |CHEMICAL ENGINEERING LABORATORY III | | | |(CHE575)
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reaction. In this experiment you will use calorimetry to measure the heats of reaction for three reactions: Reaction 1 Reaction Equation NaOH(s) → Na+(aq) + OH-(aq) Solid NaOH is dissolved in water 2 Na+(aq) + OH-(aq) + H+(aq) + Cl-(aq) → Na+(aq) + Cl-(aq) + H2O(l) Solutions of NaOH and HCl are mixed 3 NaOH(s) + H+(aq) + Cl-(aq) → Na+(aq) + Cl-(aq) + H2O(l) Solid NaOH is dissolved in a HCl solution The third reaction is actually a combination of the first two reactions. Notice that the equation for Reaction
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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 Wear your safety glasses while doing this experiment. Place 300 mL of deionized water in a large beaker and bring it to the boiling point. Boil it vigorously for
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To determine the weight-to-volume percent of acetic acid present in commercial vinegar and the weight-to-volume percent of ammonia present in window cleaners. Acid-base titrations can be conducted using the above samples against standardized aqueous NaOH and standardized aqueous HCl solutions respectively. 2. Introduction: Acetic acid‚ commonly known as ethanoic acid CH3COOH‚ is found in commercial vinegar. It is a weak organic acid that gives vinegar its characteristic pungent smell‚ sour taste
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