To determine the identity of an electrolyte in a solution, the solution's osmotic pressure may be measured. A solution containing 0.250 mol L1 of an unknown electrolyte was prepared and the osmotic pressure of the solution at 298 K was determined to be 1053 KPa. Use the reference table below in helping you to suggest the possible identity of the unknown electrolyte Electrolytic substance Van't Hoff factor (i) at 0.25 mol L1 NacI 1.70 NaBr 1.76 NaNO3 NH,CI 1.83 1.88 NH,Br 1.91 NH,NO3 1.96 ONACI ONaBr ONH4Br ONH4CI ONANO3 ONH4NO3

To determine the identity of an electrolyte in a solution, the solution's osmotic pressure may be measured. A solution containing 0.250 mol L1 of an unknown electrolyte was prepared and the osmotic pressure of the solution at 298 K was determined to be 1053 KPa. Use the reference table below in helping you to suggest the possible identity of the unknown electrolyte Electrolytic substance Van't Hoff factor (i) at 0.25 mol L1 NacI 1.70 NaBr 1.76 NaNO3 NH,CI 1.83 1.88 NH,Br 1.91 NH,NO3 1.96 ONACI ONaBr ONH4Br ONH4CI ONANO3 ONH4NO3

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Solve the value of x in the expression and express your answer in correct significant figures log ([3.0 x 10-2][2.0 x 104]/ [2.0 x]3) = 1.347 The value of x, in correct significant figures, is
A polymer of large molar mass is dissolved in the organic solvent dimethylformamide (C3H7NO) at 25 °C, and the resulting solution rises to a final height of 10.8 cm above the level of the pure solvent, as solvent molecules pass through a semipermeable membrane into the solution. If the solution contains 3.80 g polymer per liter, calculate the molar mass of the polymer. Take the density of the solution to be 0.944 g cm-³. Molar mass polymer = g mol-1
Osmosis is the process responsible for carrying nutrients and water from groundwater supplies to the upper parts of trees. Since the tree sap has a higher solute concentration than ground water, water passes through root membranes into the tree, where osmotic pressure can be as high as 20 atm in the tallest trees.What would the molar concentration of the tree sap (a non-electrolyte) have to be to achieve an osmotic pressure of 17.9 bar on a day when the temperature is 22.5 °C?
Give detailed Solution with explanation needed (no need Handwritten answer
The Rast camphor method is a cryoscopic technique for molar mass determination. Exactly 1.00 g of an isoprenoid of known formula (C5H8)n was dissolved in 5.00 g of camphor. The freezing point of the resulting solution decreased by 27.7 ℃ relative to pure camphor. Knowing that the Kf of camphor is 37.7 deg·kg/mol: Calculate for the molar mass of the isoprenoid. Calculate the value of n in the given formula of the isoprenoid. Report in whole number. The normal freezing point of camphor is 178.4 ℃. At what temperature did the isoprenoid-camphor solution freeze?
You have a sucrose solution of 28°Brix or 28 grams of sugar per 100 grams solution in a ripe grape ready to be made into wine. What is the molality of the solution? Look up the freezing point depression constant KF and figure out what the new freezing temperature would be for that solution.
. The vapor pressure of benzene is 10 kPa while methylbenzene is 2.8 kPa. Determine the total pressure of an equimolar solution.
A certain dilute solution has an osmotic pressure of 11.1 atm at 25°C. Calculate the difference between the chemical potential of the solvent in the solution and that of pure water. Assume that the density is the same as that of water at 25°C, 0.99705 g-cm-3. (Hint: Express the chemical potential in terms of mole fraction, x1, and rewrite the osmotic pressure equation as OV = n2RT, where n2 is the number of moles of the solute and V = 1.00 L.)
Osmotic pressures are often reported in units of atmospheres or mm Hg. The latter impliesthat the height of a column of liquid can be used as a measure of pressure. This is, in fact, thebasis of the torricellian barometer from which the units of “torr” come. The pressure, P, isrelated to the height of the column by:P = ρghwhere ρ is the density of the liquid, g is the acceleration due to gravity and h is the height. Whatwill be the height (in mm) of a column of aqueous solution with a density of 0.9987 g/mL, if theosmotic pressure of the solution at 25 °C is 1.4 mm Hg? The density of mercury at thistemperature is 13.8 g/mL
In addition to filling in the blanks below, show all of your work for this problem on paper for later upload. Calculate the molality of a 25.0% by mass aqueous solution of Ca(NO3)2. Enter your value in the first box and an appropriate unit of measure in the second box.
The osmotic pressure of an unknown substance is measured at 298 K. Determine the molar mass if the concentration of this substance is 28.5 kg m^-3 and the osmotic pressure is 4.00×10^4 Pa.
A semi-permeable membrane separates the contents of cell. The concentration of sodium ions is 2.1 L.atm mol mol K.mol outside of the cell and 2.5 inside of the cell. The ideal gas constant R= 8.206 x 10 -2 L L and room temperature is about 20°C or 293 K. (a) Determine the osmotic pressure (in atm) and the tonicity of the solution surrounding a cell with radius of 0.013 mm at room temperature. П= (b) The solution surrounding the cell is O Hypotonic O Hypertonic O Isotonic atm