Calculate the concentration of Y4-ion in 0.0100 M EDTA solution at pH 6. α4 = 2.2 x 10-5 for pH 6.
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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.
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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 10-5What 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.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
- 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 MQuinine ( 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 =Calculate the pH of a solution that is 0.05000 M NH4Cl and 0.0300 M NH3 (Kb for NH3 = 1.8 x 10-5)
- 9. 3 μL of a 45 mM stock solution of a substrate is added to 8 mL of water. Calculate the following values. The substrate molecular weight is 125 g/mol. Substrate volume in mL Dilution factor Substrate number of moles Substrate concentration for the diluted solution in mM Substrate concentration for the diluted solution in mole/L Substrate concentration for the diluted solution in mg/mLDetermine the fluoride ion concentration for a saturated solution of magnesium fluoride. K sp = 7.4 x 10-11Consider a mixture of two proteins with molecular weights of 20,000 and 200,000. For simplicity of calculation, both may be approximated as unhydrated spheres with VB 0.740 mL g1. a. Calculate the ratio of the sedimentation coefficients of the proteins in the same medium (density=1.05 g mL¯1) at the same temperature.
- Example The reference range for blood pH is 7.35 – 7.42. What is this range expressed as [H+] in nmol l-1? Calculation: pH = - log [H+] 7.35 = - log [H+] [H+] = antilog -7.35 = 4.47 x 10-8 mol.l-1 = 44.7nmol.l-1 similarly: pH 7.42 = 38.0 nmol.l-1 Range [H+] = 38 – 44.7 nmol.l-1 If the blood pH decreases in an acidosis from 7.42 to 7.15, what is the change in [H+] in nmol.l-1? so this is example on the worksheet, but i still understand how to answer the question.Determine the pH for the following solutions. {H3O+}=2.4x10^-2 M200 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.