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Why do you have to titrate until or above pH = 12.5 ± 0.2 to properly identify the unknown acid solution?

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.9QAP

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Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

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Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

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Why do you have to titrate until or above pH = 12.5 ± 0.2 to properly identify the unknown acid solution?

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by titration we can get the quantitatively amount of the acid solution .

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The titration curves for two acids with the same base are shown on this graph. (a) Which is the curve for the weaker acid? Explain your choice. (b) Give the approximate pH at the equivalence point for the titration of each acid. (c) Explain why the pH at the equivalence point differs for each acid. (d) Explain why the starting pH values of the two acids differ. (e) Which indicator or indicators, phenolphthalein, bromthymol blue, or methyl red, could be used for the titration of Acid 1? For the titration of Acid 2? Explain your choices.
Do you always have to use a primary standard in the standardization of titrant? Why or why not?
What is a primary reason for needing to standardize strong base titrants like KOH? Select the single best answer. OKOH is not very soluble in aqueous solutions, thus making the concentrations difficult to determine. KOH reacts with moisture in the air, thereby making accurately-determined concentrations of their solutions difficult. O Standardization is the process of reacting a strong base, like KOH, with an acid. O Standardization is the process of dissolving KOH in aqueous solution. OKOH is a very inexpensive, highly soluble, and easy-to-use base.
Identify the definition of a primary standard in titration? Identify the characteristics of a substance to be considered as a primary standard
When 30.00 mL of 0.1011 M HCl in 50 mL of deionized water is titrated against 0.09889 M NaOH, the pH increases. Find the pH when the volume of NaOH added is 0.02 mL more than the volume required to reach the equivalence point. Comment on the significance of the changes in pH values in relation to the increments of sodium hydroxide added when going “through” the endpoint.
What is the methodology of acid base titration for sodium hydroxide and hydrochloric acid.
2. After dissolving the KHP with water, a student noticed some undissolved solid, but continued with the titration as instructed by the procedure. He titrated until the pink color persisted for 30 sec and recorded the volume of titrant required. Preparing for the second determination, he set the reaction solution aside and added some more NaOH to the buret. He was about to pour the reaction solution down the drain, so he could rinse and reuse the flask, when he saw that the pink color had disappeared! a) What happened? b) What can the student do to correct for this erTor and salvage this trial? How should the data sheet be modified to reflect this correction? 3. Another student began adding titrant to the acid solution, but stopped when she suddenly realized that she forgot to add the 3 drops of phenolphthalein. When she did, the solution immediately turned dark red! a) What happened? b) What can the student do to correct for this error and salvage this trial? How should the data sheet…
Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC4H,O2 with 0.100 M Sr(OH)2 after 10.0 mL of the strong base has been added. The value of Ka for HC4H,O2 is 1.5 x 10-5. 1 2 4 > Use the table below to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of liquid water in the reaction. HC,H,O2(ae OH-(aq) → H20(1) +CgH;Oz¯(aq) Before (mol) Change (mol) After (mol) 5 RESET 0.100 0.200 +x 0.100 + x 0.100 - x -x 0.200 + x 0.200 - x 1.00 x 10-3 -1.00 x 10-3 2.00 x 10-3 -2.00 x 10-3 6.00 x 10-3 -6.00 x 10-3 7.00 x 10-3 -7.00 x 10-3 8.00 x 10-3 -8.00 x 10-3
Review the list of common titration errors. Determine whether each error would cause the calculation for moles of analyte to be too high, too low, or have no effect. adding titrant past the color change of the analyte solution recording the molarity of titrant as 0.1 M rather than its actual value of 0.01 M spilling some analyte out of the flask during the titration starting the titration with air bubbles in the buret filling the buret above the 0.0 mL volume mark Answer Bank no effect too low too high 7
Titrations are acid-base reactions in which the amount of acid and base in solution are known quite precisely. The specific case where the acid and base have been added in equivalent molar amounts, is called the equivalence point. At this point, mol acid = mol base %3D At all other points in a titration, either the base is the limiting reactant (and there is excess acid) or the acid is the limiting reactant (and there is excess base). So, except at the equivalence point, titration problems are limiting reactant problems, which means we can do them- a lot of them! One additional point: when there is left over strong acid (acid in excess), 100% of that excess acid is ionized to become H* ions: [strong acid] = [H*] and pH = -log[H"] Something similar happens for strong bases. 1. Calculate the pH of the solution after the following amounts of 0.250 M NaOH have been added to 50.0 mL of 0.200 M HCI. Show all your work for each calculation (including the volumes for which the pH is given).…
3 A 0.6423 g sample that might contain NaOH, Na₂CO₃, NaHCO₃, or a permissible mixture of the bases is titrated with 0.1062 M HCl by the double indicator method. It is found that 40.83 mL of the acid are required to reach the phenolphthalein end point. Methyl orange is then added to the solution and the titration continued using an additional 12.38 mL of the acid. Calculate the percentage of each component in the sample.
10.00mL of 0.10M acetic acid were collected in an Erlenmeyer flask, and then diluted to 100mL with distilled water. After that, two drops of indicator were added. Then, the buret was filled with 0.100M NaOH. The titration was started by slowly adding NaOH to acetic acid. (Note: Ignore the volume of the indicator added, as the volume is tiny compared to 100mL.) What is the pH of the solution in the Erlenmeyer flask after adding 10.00mL of 0.100M NaOH? Question 3 options: 7.22 6.9 8.35 7.00