Molarity of the standard solution of sodium hydroxide = 0.1010 mol/L %3D Volumes of NaOH(aq): First Third Rough titration Second titration titration titration Final burette reading: (mL) Initial burette reading: (mL) Volume of NaOH(aq) Titrated (added) (mL) 18.48 33.58 48.40 23.72 3.48 18.48 33.60 8.73 Fourth Fifth titration titration Final burette reading: 38.68 20.62 (mL) Initial burette reading: (mL) Volume of NaOH(aq) Titrated (added) (mL) 23.80 5.75 2. What is phenolphthalein and why is it required in this experiment?

Molarity of the standard solution of sodium hydroxide = 0.1010 mol/L %3D Volumes of NaOH(aq): First Third Rough titration Second titration titration titration Final burette reading: (mL) Initial burette reading: (mL) Volume of NaOH(aq) Titrated (added) (mL) 18.48 33.58 48.40 23.72 3.48 18.48 33.60 8.73 Fourth Fifth titration titration Final burette reading: 38.68 20.62 (mL) Initial burette reading: (mL) Volume of NaOH(aq) Titrated (added) (mL) 23.80 5.75 2. What is phenolphthalein and why is it required in this experiment?

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter18: Acids And Bases

Section: Chapter Questions

Problem 92A

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Molarity of the standard solution of sodium hydroxide 0.1037 mol/L Volumes of NaOH(aq): Rough titration First titration Second titration Third titration Final burette reading: mL) Initial burette reading: (mL) Velume of NaOII(aq) Titrated (added) (mL) 18.53 32.02 21.64 35.53 4.78 18.55 7.89 21.63 Fourth Finh titration titration Final burette reading: (ml) Initial burette reading: (mL) Volume of NaOH(aq) Titrated (added) (ml) 23.78 37.32 10.27 23.80 1. When HaSO<(aq) was reacted with NAOH(aq) in the titration, why was a precipitate not formed? 2. Why did the colour of the solution in the conical flask change at the end of the titration? 3. In this acid-base titration, what did we use to measure the volume of the Ha$O.(aq)? 4. What do we mean by stoichiometric point of a titration?
NaOH (ag) + HKCgHO4 (ag) -- NakCgHO4 laa) • HyO () 1.557 gof KHP is dissolved in 25.00 ml of water with 2 drops of indicator. NaOH is added to a burette. Shown below are pictures of the burette before the titration has begun (initial reading) and after the endpoint of the titration has been reached (hnal reading). Burette before titration (Initial reading, mL) Burette aftertitration (Final reading mL) 28 46 29 30 On your scratch paper, answer the following questions: A. Record the volume of NaOH to the correct number of sig figs in the burette before the titration. B.Record the volume of NaOH to the correct number of sig figs in the burette after the titration. C. What is the volume of NaOH required to reach the endpoint of the titration? Use correct significant higures D. Calculate the original molarity of the NaOH Enter your final answer in the blank below to the correct number of significant fgures Show your work
Molarity of the standard solution of sodium hydroxide = 0.1010 mol/L Volumes of NaOH(aq): Third titration First Second Rough titration titration titration Final burette reading: (mL) Initial burette reading: (mL) Volume of NaOH(aq) Titrated (added) (mL) 18.48 33.58 48.40 23.72 3.48 18.48 33.60 8.73 Fourth Fifth titration titration Final burette reading: (mL) 38.68 20.62 Initial burette reading: (mL) Volume of NaOH(aq) Titrated (added) (mL) 23.80 5.75 1. Circle the volumes of the titrated NaOH(aq) which you want to use for your calculations. How and why did you choose these volumes of NaOH(aq)?
From the solubility data given, calculate the solubility products for the following compounds. (a) SrF₂, 7.3 × 10-² x 10 g/L: x 10 Enter your answer in scientific notation. (b) Ag3PO4, 6.7 × 10-³ g/L: Enter your answer in scientific notation.
An analyst was titrating a solution of unknown acetic acid concentration with 0.01 M NaOH using phenolphthalein as indicator. After adding exactly 39.4 ml of the titrant drop-wise, the analyte solution started to turn light pink. The titrant volume 39.4 ml is best referred to as the O equivalence point. Onone of the choices O standardization point. O equilibrium point. O endpoint.
Molarity of the standard solution of sodium hydroxide = 0.1010 mol/L %3D Volumes of NAOH(aq): Third Rough titration First Second titration titration titration Final burette reading: 18.48 33.58 48.40 23.72 (mL) Initial burette reading: (mL) Volume of NaOH(aq) Titrated (added) (mL) 3.48 18.48 33.60 8.73 Fourth Fifth titration titration Final burette reading: (mL) Initial burette reading: (mL) Volume of NaOH(aq) Titrated (added) (mL) 38.68 20.62 23.80 5.75 4. (a) The sodium ion did not take part in this chemical reaction. What do we call such an ion? (b) Draw a simple diagram which shows how the sodium ion mixes with water in solution. What do we call this physical process? 4
Molarity of the standard solution of sodium hydroxide = 0.1010 mol/L %3D Volumes of NAOH(aq): Third Rough titration First Second titration titration titration Final burette reading: 18.48 33.58 48.40 23.72 (mL) Initial burette reading: (mL) Volume of NAOH(aq) Titrated (added) (mL) 3.48 18.48 33.60 8.73 Fourth Fifth titration titration Final burette reading: (mL) Initial burette reading: (mL) Volume of NaOH(aq) Titrated (added) (mL) 38.68 20.62 23.80 5.75 3. What type(s) of reactions occurred in this titration?
For a titration to be effective, the reaction must be rapid and the yield of the reaction must essentially be 100%. Is Kc > 1, < 1, or ≈ 1 for a titration reaction? Kc is the product of all reaction products (choose from: Multiplied by, added to, divided by, subtracted from) the product of the reactants, with all concentrations of reactants and products raised to their respective stoichiometric powers. As the titration proceeds, the amount of reactants (choose from: Increases, decreases, remains the same) and the amount of products (choose from: Increases, decreases, remains the same). Because the value of the numerator is (Choose from much greater than, much less than, approximately equal to) the value of the denominator, the value of Kc will be (Choose from much greater than, much less than, approximately equal to)1 for an effective titration reaction.