Exp #14: Titration 1) Standardization of NaOH with HCL. Molarity of HCI_I. DI 3 L. Volume HCI Used Volume HCI Used 25.00 Moles HCI Used M ml mol Initial Vol of NaOH_0.00 ml. Final Vol NaOH 21.5 ml Volume NaOH Used Molarity of NaOH Standard_{. 178 M Show Calculations for Molarity of NAOH: 2) Determination of Acetic Acid Concentration mly or Volume Vinegar Used 20.00 L 0.02000 L Molarity of NaOH_ 0.50 M Initial Vol of NaOH_ 0.60 mL Final Vol NaOH 35.45 mL Volume NaOH Used Moles NaOH Used mol Moles of CH,COOH mol Molarity of Vinegar M Chow Calculations for moles of NaOH and molarity of vinegar:

Exp #14: Titration 1) Standardization of NaOH with HCL. Molarity of HCI_I. DI 3 L. Volume HCI Used Volume HCI Used 25.00 Moles HCI Used M ml mol Initial Vol of NaOH_0.00 ml. Final Vol NaOH 21.5 ml Volume NaOH Used Molarity of NaOH Standard_{. 178 M Show Calculations for Molarity of NAOH: 2) Determination of Acetic Acid Concentration mly or Volume Vinegar Used 20.00 L 0.02000 L Molarity of NaOH_ 0.50 M Initial Vol of NaOH_ 0.60 mL Final Vol NaOH 35.45 mL Volume NaOH Used Moles NaOH Used mol Moles of CH,COOH mol Molarity of Vinegar M Chow Calculations for moles of NaOH and molarity of vinegar:

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 118CP: Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH,...

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In an acid-base titration, 21.16 mL of an NaOH solution are needed to neutralize 20.04 mL of a 0.0997 M HCl solution. To find the molarity of the NaOH solution, we can use the following procedure: First note the value of MH in the HCl solution. ____________M Find MOH- in the NaOH solution. Use Eq.3. ____________M Obtain MNaOH from MOH. ____________M
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.)
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Given an unknown solid mixture of NaCl and Na2CO3, determine the mass percent of each compound via titration. I'm given 0.1 M HCl standard solution and bromocresol green pH indicator, as well as standard lab equipment including a buret. What would the procedure for this look like? Will upvote