will test this by seeing how much drops of hydrochloric acid (HCl) are required to neutralize a certain amount of the antacid. Antacids are used to resist heartburn. We sometimes use them to treat this because antacids are a mild base that can neutralize acids in our stomachs‚ such as HCl. The purpose of this lab is to see how well each antacid neutralize hydrochloric acid. Procedure: 1. Obtain two burets‚ one for use with the HCl and others for use with the NaOH. 2. Record the exact molarity
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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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experiment where zinc reacts with hydrochloric acid in order to find out the number of moles and atoms of zinc reacted. This can be accomplished by weighing the sample before and after the reaction with hydrochloric acid. Data: Material Mass in grams (g) Initial mass of dry beaker 49.37 Initial mass of dry beaker + zinc 51.03 Initial mass of zinc 1.66 Final mass of beaker + zinc 50.40 Final mass of dry beaker 49.36 Final mass of zinc 1.04 Observation: We placed the zinc inside the
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Practice Final Exam Version 2 Name___________________________________ Chemistry 201 (Eikey) Part 1: MULTIPLE CHOICE (48 points). Choose the one alternative that best completes the statement or answers the question. Record your answer on the scantron. Each question is worth 3 points. 1) A student weighed 30.00 µg of sulfur in the lab. This is the same mass as A) 3.000 × 10 4 ng. B) 3.000 × 10 -5 mg. C) 3.000 × 10 -8 g. D) 3.000 × 10 -5 kg. 2) 1) 2) A student performs an experiment to determine
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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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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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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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