In the acid-base titration lab (Lab X), we used NaOH to neutralize a diluted H5SO4solution.i) Write a balanced chemical reaction for this neutralization reaction:ii) Identify the acid and the base in this reaction.iii) We used an indicator (Phenolphthalein) in this titration. Can we do this titration without an indicator? Briefly explain your answer.iv) When we started adding NaOH to the acid solution, it turned pink and quickly the color disappeared. What is the reason for this observation?v) Using the above balanced reaction, find the volume of 1.6 M NAOH needed to neutralize 25.0 mL of 2.0 M H2S04 solution (give the answer in mL)?For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac)

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In the acid-base titration lab (Lab X), we used NaOH to neutralize a diluted H5SO i) Write a balanced chemical reaction for this neutralization reaction: ii) Identify the acid and the base in this reaction. iii) We used an indicator (Phenolphthalein) in this titration. Can we do this titrati

In the acid-base titration lab (Lab X), we used NaOH to neutralize a diluted H5SO i) Write a balanced chemical reaction for this neutralization reaction: ii) Identify the acid and the base in this reaction. iii) We used an indicator (Phenolphthalein) in this titration. Can we do this titrati

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A student is making a titration curve. To do so, they added 25.00 mL of 0.1390 M HCl to a flask. They then added 36.78 mL of 0.1080 M KOH to the flask. What is the pH at this point in the titration curve?
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Haley conducted a titration experiment of a waek acid and stong base. For the experiment she used Malonic acid and should have gotten a molar mass of ~104.06 g/mol, but after completing her experiment she calculated her molar mass and it came out to 71.4 g/mol. What are possible reasons/ factors that could have lead to a lower molar mass during the experiment.
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How do you find Keq if given an equation and Ka and Kb? EX: Someone found a smashed box of smelling salts in a storage closet of Fauver Stadium. The field hockey team manager, being a chemistry pro, knew that if she could convert all of the ammonia (NH3) found in the smelling salts into an ammonium salt (NH4+ + X), she could get rid of the horrid smell. If the closet contained 100 mL of 1.0 M NH3 solution and the field hockey team manager/chemistry pro added 100 mL of a 1.0 M solution of H2SO4. Kb for NH3 = 1.73 • 10-6, Ka for H2SO4 = 1000, Ka for HSO4-= 1.2 • 10-2 a. Provide a keq value for each of the following... H2SO4 + NH3 =HSO4 + NH4 HSO4 + NH3=SO4+ NH4 NH3 + H20= OH- + NH4 NH4 + H20= NH3 + H30 SO4 + H20= HSO4 + OH-
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