A 10.010.0 mL sample of whiskey was diluted to 500.0 mL. A 4.004.00 mL aliquot of...

A 10.010.0 mL sample of whiskey was diluted to 500.0 mL. A 4.004.00 mL aliquot of the diluted sample was removed and the ethanol, C2H5OHC2H5OH , was distilled into 50.00 mL of 0.022500.02250 M K2Cr2O7K2Cr2O7 and oxidized to acetic acid.

3C2H5OH+2Cr2O2−7+16H+⟶4Cr3++3CH3COOH+11H2O3C2H5OH+2Cr2O72−+16H+⟶4Cr3++3CH3COOH+11H2O

The excess Cr2O2−7Cr2O72− was then back titrated with 23.523.5 mL of 0.13300.1330 M Fe2+Fe2+ , producing Cr3+Cr3+ and Fe3+Fe3+ . Calculate the weight per volume percent (% w/v) of ethanol in the original whiskey sample.

Expert Solution

queen_honey_blossom answered 1 year ago

1. A 25ul aliquot of cells was diluted with 75ul of PBS. An aliquotof the diluted...

1. A 25ul aliquot of cells was diluted with 75ul of PBS. An aliquotof the diluted cells was diluted 1:2 using 25ul of trypan. What is the total cell dilution factor? 2. A 25ul aliquot of cells was diluted with 75ul of PBS. An aliquot of the diluted cells was diluted 1:2 using 25ul of trypan.What was the volume(ul) of diluted cells used?

Consider a solution made by mixing 500.0 mL of 0.03158 M Na2HAsO4 with 500.0 mL of...

Consider a solution made by mixing 500.0 mL of 0.03158 M Na2HAsO4 with 500.0 mL of 0.04202 M NaOH. Complete the mass balance expressions below for Na and arsenate species in the final solution. [Na+] = ____ M [HAsO42-] + [__] + [__] + [__] = ____ M

A 10.0 mL sample of liquid bleach is diluted to 100. mL in a volumetric flask....

A 10.0 mL sample of liquid bleach is diluted to 100. mL in a volumetric flask. A 25.0 mL aliquot of this solution is analyzed using the procedure in this experiment. If 10.4 mL of 0.30 M Na2S2O3 is needed to reach the equivalence point, what is the percent by mass NaClO in the bleach? Hint: Percent by mass is grams of NaClO / mass of bleach. Presume a density for the bleach of 1.00 g/mL.

Consider the titration of a 50.00 mL aliquot of a water sample containing Fe3++ and Pb2++...

Consider the titration of a 50.00 mL aliquot of a water sample containing Fe3++ and Pb2++ with 19.62 mL of 0.00243 M EDTA to reach the end point. Excess CN- was added to a separate 20.00 mL aliquot of the same water sample, causing Fe(CN)3 to precipitate. This aliquot was titrated with 2.01 mL of 0.00243 M EDTA to reach the end point. What is the molarity of Fe3+ in the water sample? Please explain every step. Thank you.

A 0.4 g sample of CMA was dissolved in HCL and diluted to 100 mL. A...

A 0.4 g sample of CMA was dissolved in HCL and diluted to 100 mL. A 10 mL aliquot of the sample was titrated with 25.5 mL of 0.01 M EDTA. The calcium was removed from a second 10 mL aliquot by precipitation with ammonium oxalate, and the remaining filtrate was titrated with 17.25 mL of 0.01 M EDTA. a) Multiply the concentration (molarity) of EDTA by the volume, in liters, of EDTA added in the first titration to determine...

Question 1) A 1.0 mL aliquot (sample) is taken from a 1.0L solution. Which of the...

Question 1) A 1.0 mL aliquot (sample) is taken from a 1.0L solution. Which of the following is/are true when comparing the 1.0 mL solution to the 1.0L solution? Choose all that are true. -The molarity of the 1.0 mL solution is less than the molarity of the 1.0L solution -The molarity of each is the same -The number of moles of solute in each solution is the same -The number of moles of solute in the 1.0mL solution is...

A solution is made by mixing exactly 500.0 mL of 0.167 M NaOH with exactly 500.0...

A solution is made by mixing exactly 500.0 mL of 0.167 M NaOH with exactly 500.0 mL of 0.100 M CH3COOH. Calculate the equilibrium concentrations of H3O+, CH3COOH, CH3COO-, OH-, and Na+. [H3O+] = M [CH3COOH] = M [CH3COO-] = M [OH-] = M [Na+] = M

Jackie diluted 7.5 mL weak acid with 7.5 mL distilled water. Then she titrated the diluted...

Jackie diluted 7.5 mL weak acid with 7.5 mL distilled water. Then she titrated the diluted weak acid with 0.100 M NaOH. It takes 22.52 mL of NaOH to reach the equivalence point. What is the original concentration of the weak acid? What is the diluted concentration of the weak acid?

Johnny had a 50.0 mL sample of 0.4360 M NH4NO3 that he diluted with water to...

Johnny had a 50.0 mL sample of 0.4360 M NH4NO3 that he diluted with water to a total volume of 250.0 mL. He has to figure out what is the ammonium nitrate concentration in the resulting solution? Go to this link https://youtu.be/MG86IFZi_XM a) what equation is used? And what 2 pieces of glassware are used – explain what for Johnny has to make the 0.1510 M NaOH solution needed for his lab. If he uses a 100.00mL volumetric flask, how...

A buffer is prepared by adding 300.0 mL of 0.050 M Ch3COONa to a 500.0 mL...

A buffer is prepared by adding 300.0 mL of 0.050 M Ch3COONa to a 500.0 mL of 0.100 M CH3COOH. What is the pH of this buffer? Ka=1.8x10^-5 What is the pH of the buffer upon the addition of 10.0 mL of a 1.2x10^-3 M HCl solution?

Question