thermometer so as to not puncture a hole in the calorimeter) to determine the heats of reaction for Magnesium (Mg) with Hydrochloric Acid (HCl) and Hydrochloric Acid with Magnesium Oxide (MgO). Then using mathematical formulas we were able to calculate the heat formation of MgO‚ which is measured in kJ/Mol. Since both reactions are in dilute water solutions of HCl it was necessary to know the heat capacity of water‚ but because some heat would be transferred to the calorimeter whose heat capacity was
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A SUMMER TRAINING ON WORKING MANAGEMENT IN HCL CDC. SUBMITTED BY: SUBMITTED BY: Kavita Singh Enroll. NO. – 2008 CBA032 Kavita Singh Enroll. NO. – 2008 CBA032 Under the guidance Ms. Arti faculty‚ MU‚ Aligarh (U.P) INSTITUTE OF BUSINESS MANAGEMENT MANGALAYATAN UNIVERSITY‚ 33rd KM STONE‚ ALIGARH-MATHURA HIGHWAYBESWAN‚ ALIGARH DECLARATION
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SUMMARY OF ORGANIC REACTIONS SECTION 1 - ALIPHATIC Aldehydes and ketones |Type of reaction |Mechanism | |1. oxidation (aldehydes only): aldehyde ( carboxylic acid |n/a | | | | |reagents: potassium
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HKDSE CHEMISTRY – A Modern View (Chemistry) Coursebook 3 Suggested answers Chapter 25 Simple molecular substances with non-octet structures and shapes of simple molecules Page Number Class Practice 1 Chapter Exercise 2 Chapter 26 Bond polarity Class Practice 4 Chapter Exercise 5 Chapter 27 Intermolecular forces Class Practice 7 Chapter Exercise 9 Chapter 28 Structures and properties of molecular crystals Class Practice 11 Chapter Exercise 12 Part Exercise 14 Chapter 29 Chemical cells in daily life
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very different further supporting an error in measurement of data. In addition‚ the temperature of the room‚ and of the solution‚ were not measured. These temperatures may have been above 25℃. Data - Part B (80℃): Volume of HCl (mL) pH Volume of HCl (mL) pH Volume of HCl (mL) pH 0 11.22 4.5 9.16 6.6 2.85 2.5 11.06 4.7 8.35 7.1 2.77 3 10.94 4.8 6.64 7.6 2.72 3.5 10.72 5.6 3.37 4 10.35 6.1
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Irresistible? By Mikayla Messing 8/3/12 Section 623 Abstract To examine the effectiveness of buffers by titrating two sets of five different solutions using HCl and NaOH and monitoring the pH change of the various solutions. The data collected shows that the buffer systems made with sodium acetate and acetic acid were effect when titrated with the strong acid and the strong base. Comparison of all the solutions shows that the concepts of buffers holds true for the results from the experimentation
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sample | Metal fizzed when dissolved in HCl | Volume of HCl | 100 mL | Initial Temperature | 220 C | Mass of Mg | 0.1485 g | Part B Calculations Tf from graph | 50 C | Mass of HCl | 100 g | ∆TCW for HCl | -2092 J | qHCl for solution | -204.4 J | qCal for cup | -2296.4 J | qRXN | -47594 J | ∆HRXN for Mg | | NET REACTION: 2HCl(aq) + Mg(s)→MgCl2(aq) + H2(g) Part C Description of sample | | Volume of HCl | 100 mL | Temperature of HCl | 220 C | Mass of MgO | 0.5052 g |
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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 lower pH than when the titration started
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Measurement Mass of eggshell = 3.15 ± 0.01 g Volume of HCl added = 50.00 ± 0.5 〖cm〗^3 Volume of solution = 250.0 ± 0.3 〖cm〗^3 Volume of NaOH pipetted = 25.00 ± 0.03 〖cm〗^3 Titration number Rough 1 2 Initial burette reading of NaOH/ ± 0.05 cm3 0.00 0.00 0.00 Final burette reading of NaOH / ± 0.05 cm3 11.80 11.70 11.20 Volume of NaOH titrated / ± 0.10 cm3 11.80 11.70 11.20 Titration table: data collected from burette of amount of HCl used for the colour of the solution with methyl orange
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molar NaOH solution. 2. Record volume. 3. Measure out between 20 milliliters and 40 milliliters of the unknown HCl solution. 4. Record volume. 5. The amount of unknown HCl is then added to the 100-milliliter Erlenmeyer flask. 6. Add two drops of the indicator‚ phenolphthalein‚ to the acid in the flask. 7. Using the slider on the right hand side‚ add NaOH to the HCl in the Erlenmeyer flask (This action is known astitrate). Add the indicator until the color of the indicator turns
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