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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A sample containing NaOH only was titrated with standard 0.1280 M HCl, requiring 25.45 mL to reach a point beyond the endpoint. To compensate for this, the sample was back titrated with 0.1030 M NaOH solution, requiring 0.35 mL to reach the desired endpoint. If 9.00 mL of the sample was used for titration, calculate % (w/v) NaOH in the sample
The following titration data was collected by a students in CH1031. Based on the results, determine the concentration of the aqueous hydrochloric acid. Concentration of NaOH used: 0.25 M Volume of NaOH used: 25.0 mL Indicator: phenolphthalein Colorless to pale pink Endpoint color change: Table 1 Volume of hydrochloric acid Required Burette reading (mL) Trial 1 Trial 2 Trial 3 29.28 1.78 Final reading Initial reading Volume HCI used (mL) 36.62 43.98 9.28 16.62
Complete solution -Buffer Preparation-
None
Part C. Determination of Unknown Balanced chemical equation: Hcl+ Na OH -o Nacl t Hg0 Unknown number NA Trial 1 Trial 2 Trial 3 Volume of unknown HCl titrated 10.00mL NA NA Initial burette reading 0.90mL Final burette reading 30.90mL Volume NaOH added 20 00ML 50.00MLXO.144 m=43.2m moles NaOH added 4.335m (Use average molarity from part B and multiply it by the volume you added) 0.4335 M moles HCl 4.335m 04335m 10.00 mL molarity of HCl Actual Molarity (from instructor) 0.3150M percentage error
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Could someone help me answer these questions? I am unsure on how to go about this.
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
A potentiometric titration of acetic acid and 0.100 M NaOH produced the 2nd derivative curve below. Identify the volume of NaOH used to neutralize the acetic acid.
Data: Mass of Sodium Acetate :4.0 g Volume of Sodium Acetate Solution: 100.00mL Acetic Acid Concentration (mass percent from label) :4.5% pH of Prepared Buffer Solutions Buffer Solution Acetic Acid; 4.5% Sodium Acetate Solution Recorded pH A 5.0 mL 5.0 mL 4.3 B 5.0 mL 1.0 mL 4.2 C 10.0 mL 1.0 mL 3.4 D 1.0 mL 10.0 mL 5.0 E 1.0 mL 5.0 mL 4.5 The answers must have the correct units and the correct number of significant figures 1. Sodium acetate moles __________________________ (molar mass = 82.0 g/mol) Molarity of sodium acetate = _______________________ Concentration of acetic acid (from bottle) = ____________ Molarity of acetic acid = ___________________________ (molar mass = 60.0 g/mol; density of the solution is 1.0 g/mL)
Measurement of the pk, of an unknown acid by the half-neutralization method 0.1037 Concentration of standardized NaOH titrant mol/L Trial 1 Trial 2 Mass of unknown acid solution 30.01 30.00 Volume of NaOH added to half-neutralize the unknown acid 14.68 14.68 ml. ml Measured pH of half-neutralized solution 4.92 4.74 Average pH value pk, - Calculate the (H,0') and the concentration of A and HA, in the half-neutralized solution. K- (Note: In this solution, (H,0'1 (A 1) MH,0 MA M HA