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?
Can you help me answer these questions 1. Find the equivalence point and M of the acid 2. Find the Ka from pH at 0.0mL NaOH 3. Find the Ka at 1/2 equivalence (or midpoint) of NaOH
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…
Molarity of HCl used: 1.013 M Volume of HCl used: 25ml Trial 1 Trial 2 Trial 3 Volume of NaOH soln. used 21.50 21.15 21.90 Moles of NaOH used Moles of HCl titrated Volume of HCl soln. titrated: Calculated molarity of NaOH
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?
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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
2. Measurement of the pK, of Acetic Acid by the Half-Neutralization Method 1.00 Concentration of standardized NaOH titrant mole/L Trial 1 Trial 2 Trial 3 Mass of acetic acid solution 20.0 20.0 Volume of NaOH added to half-neutralize the acetic acid 0.40 mL 0.40 mL mL Measured pH of half-neutralized solution 4.68 4.66 28-7 Average pH value pk - K, = Calculate the [H,0*) and the concentrations of A- and HA, in the half-neutralized solution (Note: In this solution, [H,O*] # [A-].)
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titration curve in acid-base titration is: a. less steep curve for strong analyte versus strong titrant than weak ones b. all acid-base indicator are suitable for use c. the end point does not necessary match pH=7 for all types of acid and base analytes d. weak acid can be used for titrating weak bases
Question 3 Choose the best indicator to use in the titration of a weak base (CH3NH2) methylamine with HCl. Indicator Titration Range Color Change Methyl Orange 3.1 - 4.4 red to orange Oa. Indicator Titration Range Color Change Ob. Methyl red 4.2 -6.3 red to yellow Indicator Titration Range Color Change Oc. Bromothymol blue 6.2 – 7.6 yellow to blue Indicator Titration Range Color Change Od. Thymol blue 8.0 - 9.6 yellow to blue Indicator Titration Range Color Change Oe. Alizarin yellow 10.0 12.0 Colorless to yellow A Moving to the next question prevents changes to this answer. NOV 21 427
find the mol Na2S203 delivered for sample 1 and 2 find the mol of IO3- present for sample 1 and 2 find M of IO3- for sample 1 and 2 from the given information in the data table

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