The activity of H, O in 35 wt% H, SO4, measured by lowering of the vapor pressure of H,O, is -Al1,0 can be measured. For a salt C„ A, with cation C"+ and anion A"¯, the mean activity coefficient is defined as Y± = (y" y")(m+", where y+ and y_ are the individual activity coefficients. The mean activity is a thermodynamic defined, measurable quantity. For 5.5 m H,SO,, Y± = (ri+Yso? -)3 = 0.22 at 25 °C27 (as measured from galvanic m,0YH,0 0.66 at 25 °C.27 Activities of SO?- and H* cannot be measured separately, but the mean act %3D 0.22 in the Nernst equation, along with mµ+ containing H, SO,). Use A¡1,0 = 0.66 and y± mso?- 11.0 mol/kg and 5.5 mol/kg, to calculate the voltage of the lead-acid battery.

The activity of H, O in 35 wt% H, SO4, measured by lowering of the vapor pressure of H,O, is -Al1,0 can be measured. For a salt C„ A, with cation C"+ and anion A"¯, the mean activity coefficient is defined as Y± = (y" y")(m+", where y+ and y_ are the individual activity coefficients. The mean activity is a thermodynamic defined, measurable quantity. For 5.5 m H,SO,, Y± = (ri+Yso? -)3 = 0.22 at 25 °C27 (as measured from galvanic m,0YH,0 0.66 at 25 °C.27 Activities of SO?- and H* cannot be measured separately, but the mean act %3D 0.22 in the Nernst equation, along with mµ+ containing H, SO,). Use A¡1,0 = 0.66 and y± mso?- 11.0 mol/kg and 5.5 mol/kg, to calculate the voltage of the lead-acid battery.

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

ChapterA1: Evaluation Of Analytical Data

Section: Chapter Questions

Problem A1.22QAP

See similar textbooks

Similar questions

A 10.0 mL sample of CO2 is collected by the downward displacement of water at 23.0°C and a room pressure of 100.5 kPa. What is the volume of dry CO2 at 0.00°C and 90.0 kPa?
An experiment was conducted to determine the effect of glucose on the freezing point of water. Experimental data showed thatthe freezing point depression of water in solution was –2.6°C when 1.0 g of glucose was dissolved in 10g of solvent. Calculatethe expected freezing point for such solution and compare the expected freezing point to the value found experimentally. Give aplausible explanation for any discrepancies. (M.W. of glucose= 180.16g/mol; i=1). Show all your work.
Determine the activity coefficients and effective concentrations (activities) of Na+ and Ca2+ ions in an aqueous solution having the following composition: [Ca2+] = 3.25x 10-3 M; [Na+] = 0.96x 10-3 M; [HCO3-] = 5.75x 10-3 M; [SO42-] = 0.89x 10-3 M. (Note: Solvated ionic radii are: a(HCO3-) = a(SO42-) = 4 Å; a(Ca+) = 6 Å)
An aqueous waste stream that has a maximum concentrationof 0.50 M H₂SO₄ (d=1.030 g/mL at 25C) will be neutralized by controlled addition of 40% caustic soda (NaOH; d=1.430 g/L) before it goes to the process sewer and then to the chemical plant waste treatment facility. However, a safety re-view finds that the waste stream could meet a small stream of animmiscible organic compound, which could form a flammable vapor in air at 40.°C. The maximum temperature of the causticsoda and the waste stream is 31°C. Could the temperature in-crease due to the heat of neutralization cause the vapor to ex-plode? Assume the specific heat capacity of each solution is 4.184 J/gK.
A 150-mL aqueous solution containing two dissolved sodium salts namely, sodium sulfate (with a density of 2.66 g/mL) and sodium chloride (with a density of 2.16 g/mL), was produced by a BSMLS student. The concentrations of the solutes in 150 ml of solution were 4% (w/v) and 10% (w/w), respectively. To complete the experiment performed by the student, calculate for the following: A. Mole fraction of the solute with the higher number of moles, B. Molarity of the solution if it contains ONLY the solute with the higher number of moles, C. Molality of the solution that you have computed in letter B, and D. Normality of the solution that you have computed in letter B.
KMnO4 and Na2C2O4 solutions were used in the reactions that took place in a back titration to determine the amount of H2O2 in a sample. Calculate the concentration of H2O2 in the sample (w / v) as% by making appropriate assumptions for the volumes and normality of all these solutions.
Suppose the concentration of a solute decays linearly along the length of a container according to c(x) = c0 - αc0x, where c0 is the concentration at x = 0. Calculate the thermodynamic force on the solute at 25 °C and at x = 10 cm and 20 cm given that the concentration falls to 1/2c0 when x = 10 cm. Hint: Start by finding the value of α.
Describe the primary and secondary criteria for having achieved V ̇O2 max.
a. Ethanol vapours were allowed to completely fill a large jug with a volume of 15.5L. The ethanol was burned yielding 5.5mL of pure liquid water in the bottom of the jug at the end of the reaction. C2H5OH + 3 O2 ? 2 CO2 + 3 H20 If the room temperature was 21.5 oC and the pressure was 0.996atm, calculate the percentage yield of the water gathered in the jug. b. A 10.0 mL sample of sulfuric acid with an unknown concentration was titrated with 3.5 x 10-4 mol/L NaOH. If 20.4mL of the sodium hydroxide was required to completely neutralize the acid, determine the concentration of the sulfuric acid in the sample. Then, determine the original pH of the sulfuric acid sample
The mean activity coefficient of a 0.010 m H2SO4 solution is 0.544. What is its mean activity?
Was the gradual color change observed when the sodium thiosulfate (Na2S2O3) crystal was added to the aqueous solution of KI/12 in Station Cevidence of a chemical or physical change?
Many rivers are affectwd by illegal small scale mining. Study have revealed extremlly high deposite of heavy metals and particulate matters in rivers, making them unwholesome for drinking. With your knowledge in analytical seperation and analysis, .outline a suitable analytical protocol that can be employed to recover polluted water bodies and make them wholesome for drinking.