A 10.00-mL aliquot of unknown oxalic acid solution required 15.44 mL of 0.011 17 M KMnO4 solution to reach the purple end point. A blank titration of 10 mL of similar solution containing no oxalic acid required 0.04 mL to exhibit detectable color. Find the concentration of oxalic acid in the unknown.
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A 10.00-mL aliquot of unknown oxalic acid solution required 15.44 mL of 0.011 17 M KMnO4 solution to reach the purple end point. A blank titration of 10 mL of similar solution containing no oxalic acid required 0.04 mL to exhibit detectable color. Find the concentration of oxalic acid in the unknown.
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- 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.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 =Describe the preparation of 2.00 L of 0.100 M glycine buffer, pH 9.0, from glycine and 1.00 M NAOH. What mass of glycine is required, and what volume of 1.00 NaOH is required? The appropriate pK, of glycine is 9.6.
- A glucosamine solution of unknown concentration was diluted as follows: 1 mL of the solution was diluted to 5.0 mL. A 0.3 mL aliquot of this solution was diluted with 0.7 mL of water; the absorbance of this was measured and found to be 0.440 (uncorrected, must subtract blank). What is the concentration of the original undiluted glucosamine hydrochloride solution in µmol/mL? Given: Corrected absorbance = 0.395 y= 1.165x+0.055 Standard equation80mL of a 0.3M solution of hexapeptide Leu-His-Cys-Glu-Asn-Arg is adjusted to pH=pI. The solution is then titrated with 0.2M HCL to a final pH of 2.1. Sketch the titration curve, labelling the pH and volume axes. Indicate the volume of HCL needed to reach relevant pKa value and equivalence point(s)z Relevant pKa values are: 2.1, 4.3, 6.0, 8.3, 9.8, and 12.5.80mL of a 0.3M solution of hexapeptide Leu-His-Cys-Glu-Asn-Arg is adjusted to pH=pl. The solution is then titrated with 0.2M HCI to a final pH of 2.1. Sketch the titration curve, labelling the pH and volume axes. Indicate the volume of HCl needed to reach each relevant pKa value and equivalence point(s). Relevant pka values are: 2.1, 4.3, 6.0, 8.3, 9.8, and 12.5.
- Calculate the concentration of Y4-ion in 0.0100 M EDTA solution at pH 6. α4 = 2.2 x 10-5 for pH 6.Consider 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.Consider a buffer solution of acetate. The volume is 500 ml, the concentration is 200 mM, and the pH is 5.0. a. How many total moles of acetate plus acetic acid are present in the solution? Express answer as x.y with one digit before and one after the decimal place. b. What is the ratio of acetate ions (Ac-) to acetic acid ions (HAc) in the buffer solution (pH 5.0) if the pka is 4.76? Express the answer as x.yz with one digit before and two after the decimal place. c. How many moles of acetate are present in the solution? Express your answer to one decimal place. d. How many moles of acetic acid are present in the solution? Express your answer to one decimal place.
- Describe the preparation of 2.00 L of 0.100 M glycine buffer, pH 9.0, from glycine and 1.00 M NaOH. What mass of glycine is required, and what volume of 1.00 NaOH is required? The appropriate pKa of glycine is 9.6439 mL of 0.270 M hydrochloric acid is exactly neutralized with 0.920 M potassium hydroxide solution. What volume of base solution is required?