parts during the experiments that the group could not distinguish when the color change occurred so there was more solute going into the mix than there should have been. Also at one point there was the mistake in part B of using KHP and HCl together instead of the NaOH so that mistake skewed results just a little. Conclusion: For this experiment‚ it was essential to make sure the correct solutes were being used properly‚ as we found out‚ it would not produce a color change if the wrong things were
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Analysis of Soda Ash and Carbonate-Bicarbonate Mixture Submitted: February 27‚ 2013 Department of Chemical Engineering‚ Faculty of Engineering University of Santo Tomas España‚ Manila Abstract A standard acid solution like HCl can be used as titrant for the analysis of both soda ash and a carbonate-bicarbonate mixture. In the analysis of soda ash‚ the volume needed to neutralize the soda ash is used to compute for its alkalinity‚ in this experiment we obtained a 17.6 % alkalinity with an error
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measuring the pH levels of each. The experiment also helped students classify different substances through their conductivity properties. The preparation of a 1 M stock solution from NaOH pellets diluted to a 0.1 M NaOH solution was also utilized in making the students understand the concept of titration. Using 0.1 M NaOH as a standard solution‚ the concentration of an unknown acid was calculated from the endpoint of an acid-base titration. II. Keywords: acid‚ base‚ salt‚ pH‚ electrolytes‚ conductivity
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is enthalpy of products – reactants. (ΔHrxn = Hprod-Hreact). 2. In today’s lab you will be using 50.0 mL of 2.0 M HCl. Using Equation 3 (M=mol/L) from above‚ calculate the number of moles of acid used. M=mol/L 2.0M = x / 0.0500L x = 0.10 mol HCl 3. You will also be using 50.0 mL of 2.0 M NaOH. How many moles of base are used? M=mol/L 2.0M = x / 0.0500L x = 0.10 mol NaOH 4. The specific heat of a solution is 4.18 J/g ºC. The solution is formed by combining 25.0 g of solution A with 25
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Acid/ Base Titration Lab Design III Materials: Goggles HCl NaOH Distilled Water Label Beaker Graduated Cylinder Pipet Stirring rod Buret with clamp Stopper Ring Stand Utility Clamp Computer Computer Program pH probe Procedure: 1) 2) Goggles were put on. 3) 0.1 M NaOH solution was made using 0.4 g NaOH and 100 mL distilled water. The ingredients were added together in a beaker and stirred. 4) The buret was standardized by adding 10 mL of distilled water‚ rolling
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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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sparker 2 -250mL beakers 10mL grad cylinder 0.2M FeCl3 0.2M KSCN 0.2M KCl 0.2M Fe(NO3)3 6.0M NaOH CoCl26H2O 6.0M HCl water 0.1M K2CrO4 0.1M K2Cr2O7 1M NaOH 1M HCl 0.1M Ba(NO3)2 Procedure PART I 1. Use a 10mL graduated cylinder to measure 1mL of 0.2M FeCl3 and pour it into a 250mL beaker. Using another 10mL graduated cylinder‚ measure
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BIOL 140 Lab—The Chemical Composition of Cells Name ____________________________ I) Introduction All cells contain four major types of macromolecules: carbohydrates‚ lipids‚ nucleic acids‚ and proteins. In today’s lab‚ we will be studying three of the four-proteins‚ carbohydrates and lipids. Various chemical tests can be used to detect the presence of each of these molecules. Most of the tests involve a color change visible to the eye. If a color change is observed‚ the test is considered positive
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alkalinity of the unknown soda ash sample was determined by titrating it with standard HCl solution. After three trials‚ the researchers obtained an average percent alkalinity of 33.20% that resulted to a percent error of 12.63%. The percentage of carbonate and bicarbonate of the same unknown soda ash sample was also determined in the experiment‚ following the same procedures and using the same titrant that is the standard HCl solution; however‚ this time‚ the researchers made use of a pH meter. Subsequently
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point where the hydrochloric acid comes into contact with the solution containing phenolphthalein and base in the receiving flask‚ disappear more slowly near the endpoint? (2I) At the start of the titration‚ the NaOH solution in the flask will be pinkish and the pH is quite high. As HCl drops are added‚ the indicator colour will change momentarily to colourless as the pH is lower in the area around the drop(s). As the endpoint nears‚ the clear colour disappears more slowly as the solution has a
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