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Q: Why is rinsing of the burettes both with distilled water and solution a critical step in titration?
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Q: A. The sodium hydroxide solution was not mixed thoroughly after diluting with deionized water. B. A…
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Q: Which of the following will result to an unlit light bulb when subjected to the conductivity test?…
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Q: Write the mass balance and charge balance equation of 0.20 HNO2. Note that HNO2 is a weak acid
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Q: 1. What type of precipitate is BaSO4? 2. Why is a filter paper preferred over a sintered glass…
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Q: In the conductivity test, ________________ will result to an unlit light bulb. a. Glacial acetic…
A: In the conductivity test, glacial acetic acid will result to an unlit light bulb.
Q: Briefly describe the hazards of working with a 0.5M NaOH solution
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Q: Describe how you would prepare 1 litre of 4% v/v acetic acid using glacial acetic acid.
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Q: Explain the problem with each of the following techniques. The sodium hydroxide solution was not…
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Q: Why is it not necessary to know the exact volume of deionized water added when preparing the samples…
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Q: Assuming
A: Extinction co-efficient = 0.01662 Lmg-1cm-1 Concentration of unknown sample = 14.634g/ Explanation~
Q: 1. Using some of the following reagents, describe the preparation of 500 mL, pH 7 citric acid 1.8 M…
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Q: How do you differentiate the method of standardizing the NaOH solution from that of HCl solution?
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Q: 1. Discuss the hazards of working with the solutions used in this experiment including HNO,,…
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Q: Why is it important to keep the NaOH solution stoppered at all times when it is not in use?
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Q: 1. What type of precipitate is BaSO4? 2. Why is a filter paper preferred over a sintered glass…
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Q: This should be displaced from tips of buret before titration 2. The chemical name of a weak…
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Q: What is the minimum number of changes of 500 mL dialysate required to reduce a 100 mL sample at 1M…
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Q: If the 125 mL Erlenmeyer flasks used in this experiment, (Standardization of a Sodium Hydroxide…
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Q: Explain the half drop titration technique
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Q: Why should be solution of sodium bicarbonate be boiled during titration with HCI?
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Q: One mL of an unknown solution is placed in a test tube and a few drops of NaOH are added and shaken…
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Why Should a pipette be rinsed with HCI and a burette with NaOH? prior to use of these solutions?
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- 1. What type of precipitate is BaSO4? 2. Why is a filter paper preferred over a sintered glass filter? 3. What made an ashless filter paper ashless? 4. What does the number in a filter paper's brand represent? 5. Why is a porcelain crucible used in this procedure?Why is rinsing of the burettes both with distilled water and solution a critical step in titration?Why you should not start a titration with zero mL as an initial volume What is the use of white paper (or background) at the bottom of the erlenmeyer flask? How to deliver a droplet (a.k.a. partial drop or half drop) How to remove air bubbles in the buret Why remove air bubbles? Correct way to empty the contents of a volumetric pipet Arrangement of volume markings on the buret Steps to properly clean and rinse the buret With how many trials or replicates should titrations be performed? Difference between end point and equivalence point? Which hand should be holding the Erlenmeyer flask? How should the meniscus be read?
- A. The sodium hydroxide solution was not mixed thoroughly after diluting with deionized water. B. A student fails to swirl the Erlenmeyer flask during the addition of NaOH solution during the titration.Why is it important to keep the NaOH solution stoppered at all times when it is not in use?1.In using a burette, why is it important (a) to rinse it with a little of the solution it is going to contain, (b) to clamp it vertically, (c) to have the part below the tap full? 2. The following procedures were carried out during the titration: (a) The sides of the conical flask were washed down with deionized water. (b) The conical flask was frequently swirled or shaken.
- For titration, what is the purpose of a dropwise rate?Why is it not necessary to know the exact volume of deionized water added when preparing the samples for titration?ANALYSIS OF VINEGAR A 25.00 mL vinegar sample was diluted to 250-mL using a volumetric flask. A 50.00 mL aliquot portion of the dilute vinegar solution needed 35.45 mL of 0.1200 M NaOH to reach the phenolphthalein end point. Calculate the number of mmoles of acetic acid present in the 50-mL aliquot portion that was titrated.
- Which of the following will result to a dimly lit light bulb when subjected to the conductivity test? a. 1.0 M citric acid b. Glacial acetic acid c. Mixture of 10.0 mL 1.0 M Mg(OH)2 and 10.0 mL 1.0 M HNO3 d. 70% (v/v) ethanol200 ml of a water sample required 20 ml 0.025M Hydrochloric acid using methyl phenolphthalein. What type of alkalinity is present? Express in mg/LDiscuss the role of indicators for the titration procedure *