Experiment 11: ACID-BASE TITRATION Sample Data Collection and Results Pages Volume of NaOH used in the Titration: Rough trial Trial 3 Trial 1 Trial 2 Initial reading (mL) o.00mL Z1.0SmL O .0om o.00ML Final reading (mL) 43.15 mL Z1.50mL 21.6om L z1.45ML Volume dispensed (mL) 21.55ML ZI. L5mL 21.5OML 21.o0OmL 21.6omL Average volume of NaOH used (Trials 1-3) O. 2012 M Molarity of NaOH MOLES MOLARITY = Unknown Vinegar #_N A LITERS Calculation of moles HC2H3O2 in 5.00 mL vinegar: acetie acid =21. o om Ha0H Moles of

Experiment 11: ACID-BASE TITRATION Sample Data Collection and Results Pages Volume of NaOH used in the Titration: Rough trial Trial 3 Trial 1 Trial 2 Initial reading (mL) o.00mL Z1.0SmL O .0om o.00ML Final reading (mL) 43.15 mL Z1.50mL 21.6om L z1.45ML Volume dispensed (mL) 21.55ML ZI. L5mL 21.5OML 21.o0OmL 21.6omL Average volume of NaOH used (Trials 1-3) O. 2012 M Molarity of NaOH MOLES MOLARITY = Unknown Vinegar #_N A LITERS Calculation of moles HC2H3O2 in 5.00 mL vinegar: acetie acid =21. o om Ha0H Moles of

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter21: Potentiometry

Section: Chapter Questions

Problem 21.22QAP

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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?
Which of the indicators in Fig. 14-8 could be used for the titrations in Exercises 61 and 63?
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
Figure 15-3 outlines the classic scheme for separating a mixture of insoluble chloride salts from one another. Explain the chemistry involved in the various steps of the figure.
Data Table: (include units!) Unknown Acid # Your NaOH concentration 0.10 Trial 1 Trial 2 Volume of Acid (in mL) 17ml 15ml Initial Buret reading for 15.00ml 0.00ml your NaOH Final Buret reading for 39.06ml 21.23ml your NaOH Total volume of NaOH 0.024L 0.021L used in titration
In the experiment, we used titration to determine the total acid content ofsamples, which we reported in terms of molarity. Reporting acidity through pHmeasurements is quite different, in that we can only measure the amount of theacid in its ionized form. You were tasked to investigate a clear aqueous solutionof an unknown monoprotic acid. You decided to use two methods togather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mLdistilled water. Two drops of phenolphthalein were added and then it was titrated3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip toestimate the pH, which turned out to be around 3.3. Another 1 mL of the samplewas diluted with 9 mL of water. The pH was taken again and is now around 3.8.a) Calculate the molarity of the acid using the titration data.b) If we assume that the titrated unknown is a strong acid, predict thepH of the sample.c) Using pH strip results,…
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?
q eq req Use the References to access important values if needed for this question. A 27.6 mL sample of 0.355 M dimethylamine, (CH3)2NH, is titrated with 0.339 M nitric acid. At the equivalence point, the pH is Use the Tables link in the References for any equilibrium constants that are required. Submit Answer Retry Entire Group 8 more group attempts remaining Previous Email Instructor M
help find titration concentration from given data (use sig figs please)
Refer to the acid-base titration curve shown below. Which point is best described as a solution containing an equimolar mixture of H₂A and HA™? F E D C B Volume of Titrant Added, mL Hd A Select one: O a. point A O b. point B O c. point C d. point D e. point E O f. point F
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
Exp #14: Titration 1) Standardization of NaOH with HCl. Molarity of HCl_ 1.013 Volume HCI Used Volume HCI Used 25.00 ml M Moles HCI Used mol ml Final Vol NaOH 21.5 mL Initial Vol of NaOH_0.00 Volume NaOH Used Molarity of NaOH Standard_{, 78 m Show Calculations for Molarity of NaOH: 2) Determination of Acetic Acid Concentration mly or o.02000 L Molarity of NaOH_0.50 M Volume Vinegar Used 20.00 L Initial Vol of NaOH 0.60 mL Final Vol NaOH 35.45 mL Volume NaOH Used L Moles NaOH Used mol Moles of CH,COOH_ mol Molarity of Vinegar M Show Calculations for moles of NaOH and molarity of vinegar: