5. Calculate the molarity of the diluted solution of H2SO4. Show clearly your method.6. Calculate the molarity of the stock solution of H2SO4If you want to know if the molarity of the solution of H2SO, is accurate, what information doyou require? Molarity of the standard solution of sodium hydroxide 0.1037 mol/LVolumes of NaOH(aq):RoughtitrationFirsttitrationSecondtitrationThirdtitrationFinal burette reading:mL)Initial burette reading:(mL)Velume of NaOII(aq)Titrated (added) (mL)18.5332.0221.6435.534.7818.557.8921.63FourthFinhtitrationtitrationFinal burette reading:(ml)Initial burette reading:(mL)Volume of NaOH(aq)Titrated (added) (ml)23.7837.3210.2723.801. When HaSO<(aq) was reacted with NAOH(aq) in the titration, why was a precipitate notformed?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?

1. When H2SO<(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 H2SO«(aq)?

1. When H2SO<(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 H2SO«(aq)?

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 7RQ: Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations...

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Consider the titration of HF (K a=6.7104) with NaOH. What is the pH when a third of the acid has been neutralized?
Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)â€”which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acid
Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a primary standard. It has the formula KHC8H4O4. This is often written in the short-hand notation as KHP. If 25.0mL of a potassium hydroxide solution are needed to neutralize 2.26g of KHP, what is the molarity of the potassium hydroxide solution? Potassium hydrogen phthalate sometimes called potassium biphthalate, as shown on this bottle is an acid that is convenient to store and use because it is a solid.
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
Molarity of the standard solution of sodium hydroxide = 0.1010 mol/L Volumes of NaOH(aq): Second Third Rough titration First 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 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)?
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.
In the experiment conducted to determine the amount of acetic acid in vinegar, 8.2 mL of NaOH standard solution adjusted to 0.098 M was spent besides the phenolphthaleley indicator. Accordingly, which of the following is the amount of acetic acid in the vinegar sample in grams? (Ma (CH3COOH): 60.05 g/mol) A. 0.048 B. 0.024 C. 0.096 D.0.072
Molarity of the standard solution of sodium hydroxide = 0.1110 mol/L Volumes of NaOH (aq): Second Third Rough Titration First Titration Titration Titration Final burette reading: (mL) 23.19 26.88 25.99 29.39 Initial burette reading: (mL) 4.13 7.74 7.54 11.19 Volume of NaOH (aq) Titrated (added) (mL) Fourth Fifth Titration Titration Final burette reading: (mL) 39.83 21.96 Initial burette reading: (mL) 21.37 3.46 Volume of NaOH (aq) Titrated (added) (mL) 1. Circle the volumes of the titrated NaOH (aq) which you want to use for your calculations. Explain how and why did you choose these volumes of NaOH (aq)? 2. Few drops of phenolphthalein were used in this titration. Why was phenolphthalein used in the titration? 3. What type(s) of reaction is occurred in this experiment?
(f). Following are the titre values of two students when 25 mL of KIO3(aq) is titrated against Na2S2O3(aq).Titration no. Student 1 Student 21 2 3 24 24.9 25.7 25 24.1 24.0Which student is best in doing titration and why do you say so?(g). Taking the values of best student, calculate the concentration of the solution for which molarity is not known.(Note: first calculate moles of pipet solution in 25 mL, then moles of I2 and then moles of solution of unknown concentration and then its molarity by using average titre)
Molarity of the standard solution of sodium hydroxide = 0.1110 mol/L Volumes of NaOH (aq): Second Titration Third Rough Titration First Titration Titration Final burette reading: (mL) 23.19 26.88 25.99 29.39 Initial burette reading: (mL) 4.13 7.74 7.54 11.19 Volume of NaOH (aq) Titrated (added) (mL) Fourth Titration Fifth Titration Final burette reading: (mL) 39.83 21.96 Initial burette reading: (mL) 21.37 3.46 Volume of NAOH (ag) Titrated (added) (mL) 1. Circle the volumes of the titrated NaOH (aq) which you want to use for your calculations. Explain how and why did you choose these volumes of NaOH (aq)? 2. Few drops of phenolphthalein were used in this titration. Why was phenolphthalein used in the titration? 3. What type(s) of reaction is occurred in this experiment?

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