A geochemist measures the concentration of salt dissolved in Lake Parsons and finds a concentration of 9.0 g·L *. The geochemist also -1 measures the concentration of salt in several nearby non-isolated lakes, and finds an average concentration of 5.3 g·L *. Assuming the salt concentration in Lake Parsons before it became isolated was equal to the average salt concentration in nearby non-isolated lakes, calculate the percentage of Lake Parsons which has evaporated since it became isolated. Be sure your answer has the correct number of significant digits.

A geochemist measures the concentration of salt dissolved in Lake Parsons and finds a concentration of 9.0 g·L . The geochemist also -1 measures the concentration of salt in several nearby non-isolated lakes, and finds an average concentration of 5.3 g·L . Assuming the salt concentration in Lake Parsons before it became isolated was equal to the average salt concentration in nearby non-isolated lakes, calculate the percentage of Lake Parsons which has evaporated since it became isolated. Be sure your answer has the correct number of significant digits.

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

Balance the following chemical equations.
Consider the reaction 3X + 2Y→ 5C + 4D How many moles of X are needed to produce 24.00 moles of D? If your answer is not a whole number, answer to the hundredths place.
A solution is made by adding 29.1 mL of concentrated potassium hydroxide (34.5 wt%, density 1.46 g/mL) to some water in a volumetric flask, and then adding water to the mark to make exactly 500 mL of solution. Calculate the concentration of this solution in molarity.
A 800.0 mL aqueous solution of 93.0 mM CoCl2 is combined with 399.0 mL of aqueous 54.0 mM K3PO4. If the limiting reagent is completed consumed during this reaction, how many grams of solid precipitate will be produced? Express your answer in units of grams using at least three significant figures.
5) King Krator the Merciless has called on Pogo, a humble goldsmith, to make a crown for theKing. He gives Pogo exactly 14 oz of pure gold to fashion the crown and tells him that if hecheats the King, he will pay with his life ! Pogo leaves with the gold; he and his apprenticesspend two weeks in making the crown; finally he returns to the court. When Pogo returns withthe crown, King Krator finds that the crown weighs 397.25 grams, and has a volume of20.58cm3. King Krator asks the court wizard for the density of gold, and Wizard tells the Kingthat gold has a density of 19.3 times that of an equal volume of spring rain. Krator demands aslate, makes a few calculations, then sternly lifts his head to stare at Pogo. Does Pogo's headroll ?
Aspirin can be prepared from salicylic acid (C7H6O3), which has a molar mass of 138.12 g/mol, and acetic anhydride (C4H6O3), which has a molar mass of 102.04 g/mol. The density of acetic anhydride is 1.082 g/mL. C7H6O3+C4H6O3⟶C9H8O4+C2H4O2 What is the theoretical yield, in grams, of aspirin (C9H8O4), which has a molar mass of 180.15 g/mol, possible when reacting 3.06 g of salicylic acid with 3.54 mL of acetic anhydride?
Aspirin can be prepared from salicylic acid ( C7H6O3 ), which has a molar mass of 138.12 g/mol, and acetic anhydride (C4H,O3 ), which has a molar mass of 102.04 g/mol. The density of acetic anhydride is 1.082 g/mL. C7H6O3 + C4H, O3 → C9H3 O4 + C2H4O2 What is the theoretical yield, in grams, of aspirin ( C9H3O4), which has a molar mass of 180.15 g/mol, possible when reacting 3.25 g of salicylic acid with 3.56 mL of acetic anhydride?
Write a balanced equation for the reaction of nitric acid, HNO3(aq), with magnesium hydroxide, Mg(OH)2(aq). Include physical states.
Part A Constants I Periodic A 0.5880 g sample of impure magnesium hydroxide is dissolved in 102.0 mL of 0.2044 M HCl solution. The excess acid then needs 19.88 mL of 0.1039 M NaOH for neutralization. Calculate the percent by mass of magnesium hydroxide in the sample, assuming that it is the only substance reacting with the HCl solution. Express your answer using four significant figures. ΜΕ ΑΣΦ Submit Request Answer Provide Feedback LG Backspace F12 1 ? % Delete End Down Next >
168 mL of a 1.6 M solution of acetic acid, CH3CO2H, (molar mass 60.05) is diluted to 224 mL. Calculate the molarity of the diluted solution. Use the correct number of significant figures in your answer.
A solution is prepared by dissolving 72.91 g of CdCl2 (MM = 183.317) in enough water to make 158.95 mL of solution. If the density of the solution is 1.556 g/mL, what is the molarity of the chloride ions, Cl-(aq), in solution? Report your answer using two decimal places.
Chilean niter deposits are mostly sodium nitrate, but they also contain 0.3%iodine in the form of calcium iodate, Ca(IO3)2. After the sodium nitrate inthe niter is dissolved and recrystallized, the remaining solution contains 9 g/Lsodium iodate, NaIO3(aq). The NaIO3 is converted to iodine when it reactswith sulfur dioxide and water.2NaIO3 + 5SO2 + 4H2O → Na2SO4 + 4H2SO4 + I2a. How many liters of sodium iodate solution that contains 9 g of NaIO3 perliter would be necessary to form 127.23 kg of iodine, I2?b. What mass, in megagrams, of Chilean niter that is 0.3% I would benecessary to form the volume of sodium iodate solution you calculated inpart (a)