Please correct answer and don't use hand rating Problem 33 to 35A 500-mg sample of each mixture was analyzed for itsalkaline content using 0.1025 M HCl via double titrationindicator method.Mixture1234 5Vo-Ph (mL)4.270.015.12 6.37 5.63Vo-MR (mL)10.186.19 10.24 6.38 9.0433. Which of the following mixtures contains NaHCO3?a.Mixture 2 and 4b. Mixture 4 and 5c. Mixture 3 and 4d. Mixture 1 and 2

Step 1:In the case where the amount of HCl titrated at the methyl red endpoint is significantly more…

Answered: Problem 33 to 35 A 500-mg sample of…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.38QAP

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Phenolphthalein is a commonly used indicator that is colorless in the acidic form (pH 8.3) and pink in the base form (pH 10.0). It is a weak acid with a pKa of 8.7. What fraction is in the acid form when the acid color is apparent? What fraction is in the base form when the base color is apparent?
ANSWER BI AND ANY OTHER THREE QUESTIONS SECTION D Question B1 One way to delermine the pKa value is by use ofa pli curve. One student used thie pH curve to determine thc pka value of the weak monoprotic acid. She transferred 25.0 cm' of 0.100 M solution of the acid into a conical flask and measured the pll of the acid solution using a pH mcter accurate to one decimal place. A solution of sodium hydroxide of concentration 0.100 mol dni was added from the burette in small portions until the alkali was present in excess. The pH of the mixture was recorded after each addition of the sodium hydroxide solution. Then she plotted the pH of the solution versus volume of alkali added from the burette and used this graph to determine the acid dissociation constant. 14 12 10- 10 20 30 40 50 VNaOH (ml) a) Calculate mass of the acid required to prepare 100 cm' of 0.1 solution of this acid.(Molar mass of the acid 150 g mol) b) What is the volume of sodium hydroxide added at cquivalence point? c) What…
Indicator A B C pKIndicator 3.8 9.3 5.0 Actual Transition Range (pH) 3.0 to 4.6 3.0 to 4.6 4.4 to 6.2 Consider titrating 50 mL of 0.1 mol L-1 NH4OH (Kb = 1.75 x 10-5) with 0.1 mol L-1 HCl. Based on the table above, select the most appropriate indicator to accompany this titration. Justify your choice. What is the theoretical transition range of indicators A, B and C?
Indicator A B C pKIndicator 3.8 9.3 5.0 Actual Transition Range (pH) 3.0 to 4.6 3.0 to 4.6 4.4 to 6.2 Consider the titration of 50.00 mL of 0.1000 mol L-1 NH4OH (Kb = 1.75 x 10-5) with 0.1000 mol L-1 HCl.Based on the table above, select the most appropriate indicator to accompany this titration. Justify your choice. What is the theoretical transition range of indicators A, B and C?
Please answer all the questions. It's all one question, just Separated
BURETTE READING SAMPLE Pp Mo A 12.4 25.0 6.2 6.2 9.2 16.8 D. 0.0 5.3 Use the table below to identify the basic compound C: *Note that double indicator titration for each compound was done using a standard acid solution with 0.0 mL as initial reading. O NaHCO3 O NaOHANazCO3 O NaOHANaHCO3 O Nazco3
Aqueous Equilibria Strong Acid/ Strong Base Titrations H 14 13 12 11 Phenolphthalein color- change interval 10 9 8 pH 7 Equivalence point 2 Steps for Strong Acid/Strong Base Titrations: 1. 2. Methyl red color- change interval 3. 0 10 20 30 40 50 60 70 80 mLNaOH Na+ Initial acid Remaining acid Example: Calculate the pH when the following quantities of 0.200 M NaOH solution have been added to 50.0 mL of a 0.100 M HCI solution. a. O mL NaOH b. 10 mL NaOH c. 25 mL NaOH d. 40 mL NaOH
A 10.00-mL aliquot of a known HCl solution (3.800 g/L) was titrated with a 4.100 g/L NaOH solution. Calculate the range of the blank corrected titration volumes using the titration data below: Blank Trial 1 Trial 2 Trial 3 Initial Volume (mL) 12.50 0.50 12.30 34.75 Final Volume (mL) 13.10 10.45 22.35 45.27
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Part A A 680.0 mL sample of 0.20 M HF is titrated with 0.10 M NaOH. Determine the pH of the solution after the addition of 680.0 mL of NaOH. The K₂ of HF is 6.8 x 10-4. 3.47 1.94 2.87 3.17 4.15 Submit Request Answer
14. Consider this titration curve and answer questions a-h. (2 pts each) 14 12 10 pH 9. 10 15 20 25 30 35 40 ml base added a) This is a (strong/weak) acid titrated with a strong base. b) Place a dot () on the curve at the equivalence point. c) The pH at the equivalence point is d) What volume of base was used to titrate the acid solution to the equivalence point? e) Place a box () on the curve at the half-equivalence point. ) What is the pH at this point?

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