Problem 33 to 35 A 500-mg sample of each mixture was analyzed for its alkaline content using 0.1025 M HCl via double titration indicator method. Mixture Vo-Ph (mL) 1 2 3 4 5 4.27 0.01 5.12 6.37 5.63 Vo-MR (mL) 10.18 6.19 10.24 6.38 9.04 33. Which of the following mixtures contains NaHCO3? a. Mixture 2 and 4 b. Mixture 4 and 5 c. Mixture 3 and 4 d. Mixture 1 and 2

Problem 33 to 35 A 500-mg sample of each mixture was analyzed for its alkaline content using 0.1025 M HCl via double titration indicator method. Mixture Vo-Ph (mL) 1 2 3 4 5 4.27 0.01 5.12 6.37 5.63 Vo-MR (mL) 10.18 6.19 10.24 6.38 9.04 33. Which of the following mixtures contains NaHCO3? a. Mixture 2 and 4 b. Mixture 4 and 5 c. Mixture 3 and 4 d. Mixture 1 and 2

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
Please answer all the questions. It's all one question, just Separated
Pls help ASAP
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?
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-].)
ase Titration Curve 14 12 10- pH 8 6 4 2 0 0 4 8 12 Titrant Volume (mL) 16 20
29 In GC, the sample injected in liquid state vaporizes inside the column. * True False 30 In GC, the sample is carried through the column by inert gas. True False
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
A 30.0-mL sample of 0.20 M HCOOH was titrated with 0.20 M NaOH. The following data were collected during the titration. mL NaOH added pH B. C. D. 5.00 E. 3.07 What is the Ka for HCOOH? A. 1.1 x 10-7 1.7 x 10-4 1.2 x 10-8 4.9 x 10-11 None of these choices is correct. 10.00 3.47 15.00 3.77 20.00 4.07 25.00 4.77