You are provided 0.800M KOH, 3.38 grams of oxalic acid. Oxalic
acid pKa1 = 1.250, pKa2 = 4.266
How would you prepare a buffer with the following pH?
i) pH 4.4
ii) pH 2.3
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You are provided 0.800M KOH, 3.38 grams of oxalic acid. Oxalic acid pKa1 = 1.250, pKa2...
According to your pKA1 and pKA2 values, at which pH ranges would maleic acid be usable as a buffer? Could maleic acid be used as a buffer at physiological pH? Explain.
You have 10 uM (1*10^-6M) of Tartaric Acid. pKa1=2.89, pKa2=4.4 Calculate pH.
You have 10 uM (1*10^-6M) of Tartaric Acid. pKa1=2.89, pKa2=4.4 Calculate pH
Phosphoric acid is a triprotic acid with the following pKa values: pKa1=2.148 pKa2=7.198 pKa3=12.375 You wish to prepare 1.000 L of a 0.0100 M phosphate buffer at pH 7.580. To do this, you choose to mix the two salt forms involved in the second ionization, NaH2PO4 and Na2HPO4, in a 1.000 L volumetric flask and add water to the mark. What mass of each salt will you add to the mixture? Mass NaH2PO4=? Mass Na2HPO4=?
A diprotic acid has the following equilibrium constants Pka1- 2.160, pka2- 4.30 a. Calculate the pH of a solution of 0.750 M KHA ii. Calculate the fraction of dissociation (in percent) of species in (i)
work check and help with the last question. pka2 is more accurate
than pka1.
58 5. Calculation of molar mass: Use class-average NaOH molarity and your part B data. (Be sure this calculation is consistent with your choice reported in #1 and 2 above.) 6. Complete the following table, having consulted a table of diprotic acids; taking into account molar mass and pKa's, identify your unknown: I Molar mass pKa1 pKa2 From titration data Data from reference | 6-1 Unknown:...
. Tricarballylic acid, H3T, has pKa1 = 2.9, pKa2 = 4.4 and pKa3 = 6.0. At pH 2.0, the principal species in solution is a. H3T b.H2T - c. HT2- d. T3 Please explain Thank you!!
6. Oxalic acid H2C2O4 is a diprotic acid and can be used, in
dilute form, as wood bleach. pKa1 = 1.237 and pKa2=4.187
A. How many milliliters of 0.0500 M NaOH would be required to
completely neutralize 10.0 mL of 0.100 M H2C2O4? (5 pts)
B. Estimate the pH at the first equivalence point of the
titration. (6 pts)
C. What is the pH at the second equivalence point of the
titration. (8 pts)
Please help with work shown, especially...
You have prepared a solution by dissolving 0.20 mol glutaric acid (C5H8O2, pKa1 = 4.34, pKa2 = 5.42) and 0.10 mol mandelic acid (C8H8O3, pKa = 3.86) in 1.00 L of water. Write all equilibria occurring in solution as well as mass balance and charge balance expressions for this system. Determine the pH of this solution. I was suggested to use a spreadsheet. I can work the spreadsheet, but I can't get to equations that describe the whole system.
How you would prepare a solution of 250.0 mL of a 0.150M phosphate buffer at ph=7. (phosphoric acid pka1=2.12, pka2=7.21, pka3=12.32). What would the pH of the buffer be if 5.00mL of 1.10M HCL was added to 100mL sample of the prepared buffer.