Q4. A 5.00 mL aqueous sample containing hydrogen peroxide was diluted to 25 mL and analyzed by titration with permanganate in acidic pH: GER Mn04 + H202 → 02 + Mn2+ The sample required 84.2 mL of 0.0175 M permanganate to reach the endpoint. concentration of hydrogen peroxide in the original sample? NOT COPY NERSITY is the

Q4. A 5.00 mL aqueous sample containing hydrogen peroxide was diluted to 25 mL and analyzed by titration with permanganate in acidic pH: GER Mn04 + H202 → 02 + Mn2+ The sample required 84.2 mL of 0.0175 M permanganate to reach the endpoint. concentration of hydrogen peroxide in the original sample? NOT COPY NERSITY is the

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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For the titration of 50.00 mL of 0.300 M R6C7H5O2 (WB) with 0.200 M HNO3 (SA). Ka (HC7H5O2) = 6.3 x 105 Express pH value to two decimal places. Determine the pH after the addition 12.50 mL of HNO3.
> C V B M Alt Alt Ctrl + Hc 9. I.C. Calculate the volume of a 0.50 M NaOH(aq) necessary to completely neutralize 50.0 mL of an aqueous 0.1 M CH3COOH solution. This would be considered equimolar amounts of acid and base (a.k.a. the equivalence point of a titration). Show your work.
What phenomenon is observed when the two solid starting materials are blended together? Why does this happen?
8.) a. i. The graph indicates the pH change during the titration of 20.0 cm of 0.100 mol dm of CH:COOH (aq)with 0.100 mol dm-³ KOH (aq). From the graph, identify the volume of KOH (aq) and the pH at the equivalence point. 14 Volume : 13 12 pH: 11 10 ii. Sketch on the graph above, to indicate the change in pH during a titration of 25.0 cm³ of 0.100 mol dm- HNO3(aq) (Strong acid) with 0.100 mol dm- 0.100 KOH (aq)(strong base). On your graph, clearly indicate the starting pH value, the equivalence point, the pH at the equivalence point and the final pH reached. (Describe the curve if you cannot sketch it) pH 6. 4 3 2 1 30 Volume of KOH (aq) added / cm 10 20 40 50 b. Determine the pH of the solution resulting when 100 cm3 of HCl(aq) is mixed with 200 cm of 0.10 mol dm- NaOH(aq).
A different titration experiment using a 0.122M standardized NaOH solution to titrate a 26.48 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4) gave the following molarities for 3 trials. Initial Burette Reading (mL) Final Burette Reading (mL) Delivered vol (mL) Acid Concentration (M) Trial 1 0.0345 Trial 2 0.0334 Trial 3 0.0381 From the 3 trials, determine the average Molarity concentration of the H2SO4 to 3 significant digits. Don't include a unit.
There was a titration between 0.15 M NaOH with a monobasic acid HCI (10.0 mL). Phenolphthalein was added as an indicator which showed the color change at the volume of 18.5 mL. Find the concentration of HCI.( Show all required work).
Please don't provide handwritten solution ....
Q.2.
Could someone help me answer these questions? I am unsure on how to go about this.
Determine the hydroxide, carbonate, bicarbonate and total alkalinity for the following water samples. The titrant used was 0.02 N H:SO. and the sample volume was 50 mL. Express your results in mg/L as CaCO, Explain the differences between the samples. Jumlah ml titran untuk mencapai takat akhir Total mL titrant to reach end point Sampel Sample pH Bromkresol Hijau/ Bromcresol Green, pH 4.5 Fenolftalin/ Phenolphthalein, pH 8.3 A 8.1 0.0 9.2 B 10.4 6.7 13.4 10.4 10.3 24.6 D 10.4 10.3 4.3
#5 plz
For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K data in the ALEKS Data tab. sp compound Does solubility change with pH? highest solubility pH = 4 pH = 5 pH = 7 O yes PbF, 0 O no O yes AgCN Ο O PbCl₂ О по Oyes O no 0