Four 10.0 mL unknown samples of a solution containing hydronium ions andbromothymol blue were titrated using 0.125 mol/L sodium hydroxide solution. Thefollowing data was obtained. Please note that the buret was refilled between the thirdand fourth trials. Find the concentration of the unknown solution. * Volume of Trial acid (mL) Indicator initial Volume of Standard Solution (mL) Endpoint Final Initial colour Added Colour 1 10.0 yellow 15.30 0.35 lt. blue 2 10.0 yellow 29.94 15.30 green 3 10.0 yellow 44.59 29.94 green 4 10.0 yellow 14.94 0.28 green Your answer

Four 10.0 mL unknown samples of a solution containing hydronium ions andbromothymol blue were titrated using 0.125 mol/L sodium hydroxide solution. Thefollowing data was obtained. Please note that the buret was refilled between the thirdand fourth trials. Find the concentration of the unknown solution. * Volume of Trial acid (mL) Indicator initial Volume of Standard Solution (mL) Endpoint Final Initial colour Added Colour 1 10.0 yellow 15.30 0.35 lt. blue 2 10.0 yellow 29.94 15.30 green 3 10.0 yellow 44.59 29.94 green 4 10.0 yellow 14.94 0.28 green Your answer

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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50.0 mL of 0.31 M acrylic acid (C2H3COOH, Ka = 1.71 x 10 ) solution is titrated with 0.31 M NaOH to the equivalence point. The %3D reactants are completely transformed into sodium acrylate C2H3COONA at this point. What is the pH of the titration solution at equivalence point? Please keep your answer to two decimal places.
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A Consider the pH titration curve above (pH vs volume in ml). The pk, of the weak base being titrated and the pH of the equivalence point are, respectively: 12 11 10 8 7 5 4 2 1 10 20 30 40 O 2.5 and 4.0 • 5.4 and 4.5 O 11.2 and 5.4 O 11.2 and 4.5 O 4.5 and 5.4 Based on the indicator information above, which of the following indicators could be used successfuly in the titration in Part A? (Select all correct responses. Indicator Colour (low pH – high pH) pK, methyl yellow red-yellow 3.1 methyl orange red-yellow 3.7 bromophenol blue yellow-blue 4.2 bromocresol green yellow-blue 4.7 methyl red pink-yellow 5.1 bromocresol purple bromothymol blue yellow-purple 6.3 yellow-blue 7.0 phenol red yellow-red 7.9 O phenol red cresol red yellow-red 8.3 O bromocresol purple thymol blue yellow-blue 8.9 O methyl yellow thymolphthalein colourless-blue 9.2 O bromothymol blue O thymol blue O thymolphthalein Part C Baseu on the table above, what colour is methyl orange at pH3? Submit Request Answer Part…
Name: Date: Section: Report Sheet: pH: Measurement and Application. A: Determination of pH Using Acid-Base Indicators: Indicator Color NaH,PO, HC,H,O, ZNSO, Methyl Violet Thymol Blue Methyl Yellow Congo Red Bromocresol Green pH Range B: Measurement of the pH of Solutions Record the measured pH and the color observed using bromocresol green for each 0.1 M solution NaH,PO, HC,H,O, ZNSO, C: Determination of K, for a Weak Acid Volume Used(Liters) Moles [HC,H,O,] M HC,H;O, () HC,H,O, |NaC,H;O,] M NaC,H,O, (L) NaC,H,O; Buffer pH pK, HC,H,O, K, HC,H,O, 115
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