The aim of this experiment was to calculate the concentration of an unknown solution of Sodium Hydroxide (NaOH) by titrating it with Hydrochloric Acid (HCl) and to identify any possible sources of error. A colour change from pink to yellow signified the end of each individual titre as the NaOH had been neutralised. Experimental: Method: Firstly two solutions were prepared to show the colour of the Phenol Red indicator in acid and alkaline conditions. These colours were then used to determine the
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(AlK(SO4)2 ∙ 12H2O). These tests like the process of filtration heating the solution will reveal things such as melting point‚ percent hydrate‚ as well as percent sulfate. After the experiment‚ the experimental mole ratio of alum to water will be calculated and then compared with the accepted mole ratio. (This is 12 to 1). Theory If this lab if conducted properly‚ the unknown substance will be determined to be alum because of melting point‚ percent hydration and percent sulfate. The first test that
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the solution is raised. Thus‚ a 0.1 M acetic acid solution has a pH of 2.87 but a solution of 0.1 M acetic acid and 0.1 M sodium acetate has a pH of 4.74. Thus 4.74 is the pH of the buffer. On addition of 0.01 mole NaOH the pH changes from 4.74 to 4.83‚ while on the addition of 0.01 mole HCl the pH changes from 4.74 to 4.66. Obviously the buffer solution maintains fairly constant pH and the changes in pH could be described as marginal. Buffer Action: A buffer solution containing equimolar
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the hydrogen gas produced was calculated using Dalton’s Law of partial pressure. With this partial pressure value along with known values in the experiment the number of moles of hydrogen gas produced could be calculated using the ideal gas law equation and this experimental value was compared to the theoretical number of moles that should have been produced in the reaction. It was found that the average comparison value between the theoretical value and the experimental value was 97.8% with a standard
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The number of people diagnosed with cancer is increasing from year to year. When it comes to women‚ their biggest threat is breast cancer. According to the American Cancer Society at the end of 2016 there will be 246‚660 new cases of breast cancer among American women‚ and that around 40‚450 of those women will probably die from breast cancer. What the experts from the American Cancer Society also stated is that one in eight women in the U.S. are going to develop invasive breast cancer during their
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Aim: To Find and test the Iron content in different food sources INTRODUCTION: A Redox titration was used in order to perform this experiment. Reduction/oxidation (redox) process occurs when electrons are transferred from a donor species (the reducing agent) to another acceptor species (the oxidizing agent). It happens between an analyte and a titrant. A redox titration is done just as a normal titration is done‚ however instead of titrating an acid against a base‚ an oxidizing agent is titrated
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KHC8H4O4 (aq) + NaOH (aq) KHC8H4O3 - Na+ (aq) + H2O (l) Average volume of NaOH titrate used = ½ (5.00 + 5.00) = 5.00 cm3 No. of moles of KHC8H4O4 reacted = 0.01 × 0.05044 = 5.044 x 10-4 mol From the equation‚ mole ratio of NaOH ≡ KHC8H4O4 is 1:1‚ No. of moles of NaOH reacted = 5.044 x 10-4 mol
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EXPERIMENT 3 Name: Flame Tests & Electron Configuration Pre-Laboratory Questions and Exercises Due before lab begins. Answer in the space provided. 1. Write electron configuration for the alkali metals Li‚ Na‚ K‚ and Rb. Li ____He 2s1_____________________________________________ Na ____Ne 3s1______________________________________________ K _______Ar 4s1___________________________________________ Rb _______Kr 5s1___________________________________________ 2. Write the electron configuration
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MA‚ PAULINE Date Performed: 10 SEPTEMBER 2014 NACIONGAYO‚ DANIELLE Date Submitted: 17 SEPTEMBER 2014 TEDERA‚ YVES HEAT EFFECTS AND CALORIMETRY Experiment No. 2 I. RESULTS A. Determination of Heat Capacity In this experiment‚ an improvised calorimeter was used to determine the heat capacity. The calorimeter weighed 4.47 grams prior to the addition of water. Tap water‚ 40 mL to be exact‚ was added to the calorimeter which increased the weight to 43.87 grams. The water was measured using
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mL | 46.6-34.8=11.8 mL 46.6-34.8=0.0118 L | 1) Number of moles of NaOH used=0.0118 L of NaOH0.1 M of NaOH 1) Number of moles of NaOH used=0.00118 mol 2) The number of moles of NaOH used is equal to the number of moles of H+ions present in the solution‚ which is equal to the number of moles of the unknown salt. Moles of NaOH=Moles of H+=Moles of Unknown Salt=0.00118 mol 3) Molecular weight is equal to grams per mole. The mass of the salt was measured before the titration was carried
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