Titration and 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
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Experiment 5- Standardization of NaOH and determination of Molarity of an unknown Acid Objectives 1. Preparation and standardization of a 0.1M NaOH solution 2. To learn the technique of titration 3. Determination of the concentration of an unknown diprotic acid. Introduction Titration can be traced to the origins of volumetric analysis‚ which began in the late eighteenth century. Study of analytical chemistry began in France and the first burette was made by Francois Antoine Henri
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Name: ____________________________________Period: _____ Date:____________ Lab 9: Formula of a Hydrate Lab Purpose: To utilize mole conversions to determine the ratio between copper (II) sulfate molecules and water of hydration. Materials: 1 Hot Plate 1 Wire Mesh 1 Small beaker 1 Glass Stirring Rod 1 Electronic Scale 1 Crucible Tong Copper II Sulfate Hydrate (approx. 5g) Procedure: 1. Mass small beaker (empty) 2
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crystal in any way and can be extracted by heating the compound. 1b. Anhydrous compound: a compound without water. 2a. The dot means that there are water molecules present in the crystal lattice in a specific ratio. 2b. For every mole of copper sulfate‚ there are five moles of water. 2c. The molar mass of copper (II) sulfate is 159.61 grams/mol 2d. The molar mass of 5H2O is 90.10 grams/mol 2e. The molar mass of the entire compound is 159.61 + 90.10 = 249.71 grams/mol 2f. The percent of water in
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Chemistry 2202 Review Final Exam Chapter 2: The Mole 1. Isotope – atoms of an element that have the same number of protons but different numbers of neutrons. Ex. The three forms of oxygen are called oxygen-16‚ oxygen-17‚ and oxygen-18. They all have 8 electrons and are written as 16/8 O (8 protons + 8 neutrons)‚ 17/8 O (8 protons + 9 neutrons)‚ and 18/8 O (8 protons + 10 neutrons). 2. 3. Mass Number – the sum of the protons and neutrons in the nucleus of one atom of a particular
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^-4 in HCl. Solution: pH = -log [H3o+] pH= -log[5.4 x 10 ^-4 ] = 3.27 pNa = -log [2.00 x 10^-3 ] pNa = 2.669 For pCl = -log[Cl NaCl] + -log[ClHCl] pCl = 2.595 Concentration of Solutions 2. Normality (N) is the ratio between the no. of moles of solute in one equivalent per liter of solution. • An equivalent is the ratio between Reacting units can be a: the molar mass of the substance •Base‚ Acid or salt and the Avogadro’s number of the reacting
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Trial 1: Molar Mass of H2O = 2 x (1.01) + 16.00 = 18.02gmol1- How many moles of H2O evaporated Trial 1: 0.72g±0.04g/18.02gmol1- = 0.03995… ≈ 0.040mol±6.25% = 0.040mol±0.003mol Molar Mass of CuSO4 Cu: 63.55 gmol1- S=32.07 gmol1- O x 4= (16.00) x 4=64.00 gmol1- CuSO4= 159.62 gmol1- Moles of anhydrous part (CuSO4) 1.35g±0.02g/159.62 gmol1-=0.0084575… ≈ 0.00846mol±1.48%=0.00846mol±0.00013mol Moles of H2O in 1 mole of CuSO4 0.00846mol of CuSO4-----------> 0.040mol of H2O 1mol of CuSO4
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Experiment 4 SOLUTION STOICHIOMETRY ACID-BASE TITRATIONS Determination of the Percent Acetic Acid in Vinegar Objectives: (1) To introduce and use the concept of solution stoichiometry (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
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following in order of increasing number of atoms a. 27g of Aluminum (Al) b. 0.5 mol of Al 3 c. 50 dm of HNO3 at STP d. 1 x 10 –2 mol of Al e. 2.1 mol of Al 2. What information does the formula of ethanol (CH3CH2OH) contain? How many moles of ethanol are present in 920 g of ethanol? 3. Mr. Deeble recently opened his own chemical plant in Basseterre. His financial advisor Tyrah‚ has discovered a new technique for boosting company profit. If the company can cheaply extract the pure
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of Co2+ to Co3+ is apparent by the colour change of the new complex formed which is a shiny greenish black colour from a dull brown colour. Experimental Procedure A slurry of cobalt (II) carbonate and acetylacetone was made using (2.53g‚ 0.021 mole) of cobalt (II) carbonate and approximately (20ml‚ 0.2mole) of acetylacetone‚ these were added to an 100ml Erlenmeyer flask and were stirred with a glass stirring rod to produce the slurry. The mixture was then heated to 100°C on a hot plate the temperature
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