7 Please! 7) Oxalic acid is the simplest diprotic organic acid. How many milliliters of 0.800 MKOH should be added to 3.38 g oxalic acid to give a pH of 4.40 when diluted to a totalvolume of 500.0 mL?Oxalic AcidOH90.035 g/molpKal = 1.27, pKa2 = 4.266Formula mass =НО8) Given a buffer solution that is 0.250 M in formic acid (HCOOH) and 0.150 M sodiumformate (HCOONA), what will be the pH if to 50.0 mL of this solution is added 50.0 mLof 0.0100 M HCI ?9) Concentrated sulfuric acid has a density of 1.84 g/cm3 and is 95.0% (mass) H2SO4.Recall this is why you never want to touch it. (It will pull the water out of your skin,since it has such a low water content.) Calculate the molarity, molality and molefraction of this solution. (See Chapter 17)

7) Oxalic acid is the simplest diprotic organic acid. How many milliliters of 0.800 M KOH should be added to 3.38 g oxalic acid to give a pH of 4.40 when diluted to a total volume of 500.0 mL? Oxalic Acid ОН Formula mass = 90.035 g/mol pKa1 = 1.27, pKa2 = 4.266 %3D Но

7) Oxalic acid is the simplest diprotic organic acid. How many milliliters of 0.800 M KOH should be added to 3.38 g oxalic acid to give a pH of 4.40 when diluted to a total volume of 500.0 mL? Oxalic Acid ОН Formula mass = 90.035 g/mol pKa1 = 1.27, pKa2 = 4.266 %3D Но

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

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Question

7 Please!

7) Oxalic acid is the simplest diprotic organic acid. How many milliliters of 0.800 M
KOH should be added to 3.38 g oxalic acid to give a pH of 4.40 when diluted to a total
volume of 500.0 mL?
Oxalic Acid
OH
90.035 g/mol
pKal = 1.27, pKa2 = 4.266
Formula mass =
НО
8) Given a buffer solution that is 0.250 M in formic acid (HCOOH) and 0.150 M sodium
formate (HCOONA), what will be the pH if to 50.0 mL of this solution is added 50.0 mL
of 0.0100 M HCI ?
9) Concentrated sulfuric acid has a density of 1.84 g/cm3 and is 95.0% (mass) H2SO4.
Recall this is why you never want to touch it. (It will pull the water out of your skin,
since it has such a low water content.) Calculate the molarity, molality and mole
fraction of this solution. (See Chapter 17)

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