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

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.14QAP

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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
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
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
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
the volume of HCL and acetic acid is 250 mL
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-].)
plz solve it within 30-40 mins I'll give you multiple upvote
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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?
ase Titration Curve 14 12 10- pH 8 6 4 2 0 0 4 8 12 Titrant Volume (mL) 16 20

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