13.In sampling, a producer's risk (type 1 error) is usually occur when a bad batch was accepted 14.A blank titration is a titration conducted without the use of indicator 15. In double indicator titration, If the volume of the standard acid consumed in phenolphthalein end point is more than in methyl orange end point, the sample is a mixture of Na₂CO₂ & NaHCO3

13.In sampling, a producer's risk (type 1 error) is usually occur when a bad batch was accepted 14.A blank titration is a titration conducted without the use of indicator 15. In double indicator titration, If the volume of the standard acid consumed in phenolphthalein end point is more than in methyl orange end point, the sample is a mixture of Na₂CO₂ & NaHCO3

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...

See similar textbooks

Similar questions

Which indicator is the best to use for the following titration? Strong Acid with Weak Base Bromcresol green (pH = 4-5.5) Phenol red (pH = 6.5-7.5) Phenolphthalein (8.5-10)
(b) Shown in the graph below is the titration curve that results when 25.0 mL of 0.200 M HCIO is titrated with 0,200 M NaOH, Carefully draw a second curve on the graph that would result from the titration of 25.0 mL. of 0.200 M HCIO, with 0.200 M NaOH. 14- 13 12 11 10- 9. 8 명 7- 6- 5- 4 3 2. 1 35 Volume of 0:200 M NAOH Added (mL.) 10 15 20 25 30 40 45
Consider a titration between a strong acid and a weak base. What is the pH at the equivalence point? O PH 7
For the titration of a strong acid with a strong base, which statement below is FALSE? A. At V = 0 mL titrant added, the pH is due to initial concentration of strong acid. B. The indicator changes color at the end point due to excess acid. C. Between V = 0 mL and the equivalence point, the pH is due to diluted unreacted strong acid. D. Past the equivalence point, the pH is due to diluted excess strong base. E. At the equivalence point, the pH is due to the auto-ionization of water.
The following graph shows the pH curve for the titration of 25 mL of a 0.1 M monoprotic acid solution with a 0.1 M solution of a monoprotic base. 14 pH 12 10 8 6 4 2 0 0 5 10 15 20 25 30 35 40 45 50 mL of 0.1 M base added (1) The pH curve represents the titration of a (2) Choose a suitable indicator for the endpoint of the titration from the following pulldown list. 0 Malachite green Thymol blue Methyl orange Bromocresol green Methyl red Bromothymol blue Cresol red Phenolphthalein Thymolphthalein Alizarin yellow 0.2 1.8 pH 0 1 1.2 2 2.8 3 3.2 4.4 3.8 5.4 4 4.8 6.0 5 6.0 6 25 7.0 71 7 8.0 9.6 7.6 8.2 8 8.8 10.0 94 10.6 10.1 9 10 11 acid with a 12.0 12 13 14 base.
In order to determine the chloride concentration in a solution, a Mohr titration is perform. This involves adding a small amount of chromate to the solution and then slowly adding silver nitrate. Silver chloride is pale yellow solid while Silver chromate is a dark red. The appearance of the red silver chromate is the endpoint of the titration. Answer the questions below about this process. (Ksp of AgCl= 1.7x10^-10 and Ksp of Ag2CrO4= 1.12x10^-12) A 100 mL sample of water from a potentially contaminated stream is collected. A 0.0010 g of sodium chromate is dissolved in the sample. 1) if the solution had been 0.015 M in NaCl, what percent of the chloride is still in solution? Given the answer to the question above, it should be clear that "all" of the chloride is removed before the silver chromate appears. This is why we can use it as an endpoint. 2) if it requires 21.4 mL of a 0.1 M solution of silver nitrate to reach the equivalence point with 100 mL of solution, what was the original…
A titration was performed where a weak acid was titrated with a strong base. Use the following graph of the titration curve to estimate the volume of the strong base, along the x-axis, that was dispensed to reach the equivalence point. 14.00- 12.00- 10.00- 8.00- 6.00- 4.00 2.00- ● ● ● 0.00- 0.00 5.00 10.00 15.00 20.00 25.00 30.00 35.00 40.00 45.00 50.00 Volume (ml)
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…
Why you can't always use M1V1 = M2V2 in all titration problems?
How is activity related to the 1/2 equivalence point in a titration? activity=activity coefficient x Molarity
Answer Questions #27 through #31 about the titration curves below (labeled a and b) for two different bases. The titrant acid used in both cases was 0.100 M HCl and the volume of the base solutions in both cases was 75.0 mL mL. 14 14 12 12 - 10- 10 8- 6. 4. 2- 2- 20 40 60 80 100 20 40 60 80 100 Volume of acid added (mL) (a) (b) Volume of acid added (mL) 2014 Pearson Education Inc P Type here to search 11:17 AM (? 3/18/2021 -> ort sc 80 6. ece num ER/TY || на 0 04 2C Hd
Titration Curve Using the table of indicators identify which of the given 13 12 indicators would be appropriate for the titration 11 10 represented in the titration curve. 9 thymol blue 8 pH 7 6 alizarin yellow R 5 O quinaldine red 4 3 O clayton yellow 2 1 metacresol purple 4 6 8 10 12 14 16 18 20 Volume of Titrant (mL) O methyl green 2.