10:57H₂O0.1 NaClSolution ASolution BInitial pH7.05.D3.010.0Acid-Base Titration% acidity from vinegar labelMolarity of NaOH2030Volume of Vinegar (ml)Initial Volume of NaOH (ml)Final Volume of NaOH (mL)Report Table AB.3: Effect of Adding BasepH after 5Drops NaOH11.09.03.011.0Acid/Base Titration, Buffers, and PH Report SheetpH after 10Drops NaOH5%0.101Trial 1Report Table AB.4: Concentration of Acetic Acid in Vinegar11.012.03.011.0**5.00 ML0.00 ML41.20 MLTotal pHChangeTrial 25,00 ML000 ML38.40mLBuffer? (Y orN)Trial 3Show your calculations for calculating the %(m/v) for acetic acid in vinegar for Trial 1 in ReportTable AB.4.X5.00 ML0.01 ML41.30mL

Report Table AB.3 Effect of Adding Base To determine: The total pH change. Solution is Buffer or…

Answered: Initial pH Report Table AB.3: Effect of…

Initial pH Report Table AB.3: Effect of Adding Base pH after 5 Drops NaOH pH after 10 Drops NaOH Total pH Change Buffer? (Yor N)

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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Calculate the molarity of the acetic acid in the vinegar solution. given: Given: Molarity of sulfuric acid:0.205 M (Sodium hydroxide with sulfuric acid)Approx Titration- initial buret reading : 0mL finak buret reading : 31.8mL titration 1- initial buret reading : 0mL finak buret reading : 31.5 mL titration 2- initial buret reading: 0mL final buret reading : 31.7mL Analysis of vinegar Volume of vinegar solution:5mL Approx titration - initial buret reading : 0mL final buret reading : 20.1 mL titration 1- initial buret reading : 0mL final buret reading : 20.9mL titration 2- Volume of vinegar solution: 5mL initial buret reading : 0mL Final buret reading :20.0mL
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If you are given sodium acetate and asked to make a 250 mM acetate buffer and titrate it to a final pH of 4.76, will you have to add acid, base, or nothing in order to achieve the proper pH? Why? Please explain the “why” part of the question. Please type answer note write by hend.
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Part A Review Constants | Periodic Table Learning Goal: To understand how buffers use reserves of conjugate acid and conjugate base to counteract the effects of acid or base addition on pH. A buffer is a mixture of a conjugate acid-base pair. In other words, it is a solution that contains a weak acid and its conjugate base, or a weak base and its conjugate acid. For example, an acetic acid buffer consists of acetic acid, CH3COOH, and its conjugate base, the acetate ion CH3COO. Because ions cannot simply be added to a solution, the conjugate base is added in a salt form (e.g., sodium acetate NaCH, COO). Buffers work because the conjugate acid-base pair work together to neutralize the addition of H+ or OH ions. Thus, for example, if H+ ions are added to the acetate buffer described above, they will be largely removed from solution by the reaction of H+ with the conjugate base: H++ CH3COO→CH3COOH Similarly, any added OH ions will be neutralized by a reaction with the conjugate acid: OH +…
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