Calculate the concentration of Y4-ion in 0.0100 M EDTA solution at pH 6. for pH 6, α4 = 2,2 x 10-5
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Calculate the concentration of Y4-ion in 0.0100 M EDTA solution at pH 6.
for pH 6, α4 = 2,2 x 10-5
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- Calculate the concentration of Y4-ion in 0.0100 M EDTA solution at pH 6. α4 = 2.2 x 10-5 for pH 6.What mass of sodium glycolate (NaC2H3O3) should be added to 400.0 mL of 1.00 M glycolic acid to produce a buffer solution with a pH of 4.00? Ka = 1.47 x 10-4. Please indicate the full solutions.If an aqueous solution has a hydroxyl ion concentration of 1 × 10-6 M, what is the concentration of hydrogen ion ([H+]) ? [H+] = 1.0 x10-5 M
- What mass of sodium glycolate (NaC2H3O3) should be added to 400.0 mL of 1.00 M glycolic acid to produce a buffer solution with a pH of 4.00? Ka = 1.47 x 10-4Calculate the pH of a solution that is 0.05000 M NH4Cl and 0.0300 M NH3 (Kb for NH3 = 1.8 x 10-5)Quinine ( C20 H24 N2 O2) is the most important alkaloid derived from cinchona bark. It is used as an antimalarial drug. For quinine, pK, = 5.1 and pK, = 9.7 ( pKp = – log Kp). Only 1 g quinine will dissolve in 1920.0 mL of solution. Calculate the pH of a saturated aqueous solution of quinine. Consider only the reaction | Q+ H2O= QH+ + OH- described by pK, where Q = quinine. pH =
- Compare the solubility of lead carbonate in each of the following aqueous solutions: Clear All 0.10 M Pb(NO3)2 More soluble than in pure water. 0.10 M K,CO, Similar solubility as in pure water. 0.10 M NH,NO3 Less soluble than in pure water. 0.10 M NACH3C00Given the titration curve of the hypothetical polyprotic acid X at 0.100 M concentration (pKa1=4.0, pKa2=8.0, pKa3=12.0) titrated with 0.600 M NaOH, identify the pH at point C, H, E, and M.Calculate the pH of a buffer that contains 0.75 M acetic acid and 0.35 M acetate ion in 1 L solution. What will the pH of the buffer be upon the addition of 100.0 mL of 1.0 M NaOH? (Ka of acetic acid is 1.75 x 10-5 M)
- 200 microliters of a standard solution of 0.200 mg/mL caffeine was mixed with 4.8 mL of 50 mM sodium phosphate buffer, pH 3: methanol (60:40 v/v). What is the concentration of caffeine, in mg/mL, in this solution? Give your answer to two significant figures.Compare the solubility of lead carbonate in each of the following aqueous solutions: Clear All 0.10 M Pb(CH3C00)2 More soluble than in pure water. 0.10 M (NH4)2CO3 Similar solubility as in pure water. 0.10 Μ KNΟS Less soluble than in pure water. 0.10 Μ ΝΗCH, COOThe isoelectric point of eIF4a is 5.02. Students are given a sample of cell lysate containing eIF4A at pH 7.4. They are also provided with two buffers of pH 7.4 to use for ion exchange chromatography. One buffer has a very high salt concentration (1 M), the other has a low salt concentration (0.1 M). Mariela decides to use an anion exchange column, while Ashok chooses a cation exchange column. Who made the better decision? Provide a detailed explanation of why one student will end up with a purer sample of eIF4A. Which buffer will you use while washing away impurities (high or low salt), and which would you use to remove eIF4A from the column? Explain your choice.