A geochemist measures the concentration of salt dissolved in Lake Parsons and finds a concentration of 4.27 g·L - 1 The geochemist also measures the concentration of salt in several nearby non-isolated lakes, and finds an average concentration of 2.6 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. 0%

A geochemist measures the concentration of salt dissolved in Lake Parsons and finds a concentration of 4.27 g·L - 1 The geochemist also measures the concentration of salt in several nearby non-isolated lakes, and finds an average concentration of 2.6 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. 0%

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

A chemist performs a gravimetric analysis. The chemist combines 1.00 L of 2.00 M AGNO, (ag) with 1.00 L of 4.00M NaCl (ag) in an Erlenmeyer flask. Both the AgNO3 (aq) solution and the NaCl(aq) solution are colorless. After the mixture has been stirred, a cloudy white substance is observed at the bottom of the flask. What is the expected mass of AgCl (s), in grams, assuming that the yield is 100%? In the box, enter the mass to the nearest gram.
The solubility of aluminum sulfate (Al2(SO4)3) in water is 34.22 g per 100.0 mL of solution at a certain temperature. What is the aluminum ion concentration in a saturated solution of aluminum sulfate? Express your answer in units of molarity (M) to at least three significant figures.
An unknown sample of ascorbic acid was titrated with 25.87 mL of 0.8198 M KIO3 (aq). Calculate the mass (in grams) of ascorbic acid in the unknown sample. Use the correct number of significant figures in your answer. F.W. of ascorbic acid = 176.12 g/mol.
A concentrated perchloric acid solution is 69.8% HCIO4 by mass and its density is 1.68 g mL-1. What volume (in litres) of the concentrated perchloric acid solution is needed to make 2.92L of 3.20 mol L-1 HCIO4(aq)? Molar masses, in g mol-1; HCIO4, 100.458 H2O, 18.016 0.447 L 0.0939 L 0.800 L 0.559 L 0.390 L Back: Question Menu
How many grams of oxalic acid, H2C2O4, are required to prepare 750. mL of a 0.250 M oxalic acid solution? Report your result in decimal notation and to the proper number of significant figures.
2. The solubility of KClO, at several temperatures is shown in the accompanying diagram. Solubility, g per 100 g H₂O 50 40 30 20 10 10 20 30 40 50 60 70 80 90 Temperature, °C If a student mixes 10.0 g of KCIO, with 45.0 g of H₂O at 70 ° C. Which statement about the final solution is correct? (A) It is a saturated solution. (B) It is a supersaturated solution. (C) It is an unsaturated solution. (D) It is impossible to determine.
How many millilitres of 0.450 mol L−1 H2SO4(aq) are required to completely neutralize 46.7 mL of 0.930 mol L−1 KOH(aq) ? Hint: Write a balanced chemical equation for the reaction. Give your answer in mL, accurate to three significant figures. Do not include units as part of your answer.
c) Classify the following reactions whether they are homogeneous or heterogeneous: 1- PbCl2 (s) > Pb?+aq) + 2 Cl (ag) 2 N2 (g) + 3H2 (g) > 2NH3 (g) The atomic weight for the metals (g/mole)
One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate. Suppose an EPA chemist tests a 200.mL sample of groundwater known to be contaminated with iron(II) chloride, which would react with silver nitrate solution like this:FeCl2(aq)+2AgNO3(aq)→2AgCl(s)+Fe(NO3)2(aq) The chemist adds 78.0mM silver nitrate solution to the sample until silver chloride stops forming. He then washes, dries, and weighs the precipitate. He finds he has collected 3.4mg of silver chloride.Calculate the concentration of iron(II) chloride contaminant in the original groundwater sample. Round your answer to 2 significant digits. _________________mg/L
As shown in the following Figure, an aqueous solution of Nal is poured into an aqueous solution of Pb(NO3)2 which results in the formation of a yellow precipitate. Assuming stoichiometric amounts of Nal and Pb(NO3)2 are reacted, give the chemical formula of the yellow precipitate and the chemical formula of all molecules and/or ions that are present in the solution (You may use the solubility matrix to answer this question). (b)
(b) Zn(NO3)2(aq) + 2 N2OH(aq) → Zn(OH)2(s) + 2 NaNO3(aq) Write the complete ionic equation. (Include states-of-matter under the given conditions in your answer. Use the lowest possible whole number coefficients.) chemPad О Help Greek List the spectator ions. (Include states-of-matter under the given conditions in your answer. Separate substances in a list with a comma. Use the lowest possible coefficients.) chemPad О Help X.x" →=- Greek Write the net ionic equation. (Include states-of-matter under the given conditions in your answer. Use the lowest possible whole number coefficients.) chemPad О Help Greek Zu2+ Zu+2 Classify the type of reaction given for (b). (Select all that apply.) a combination reaction na combustion reaction O a decomposition reaction V a metathesis reaction V a precipitation reaction
One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate. Suppose an EPA chemist tests a 200. mL sample of groundwater known to be contaminated with copper(II) chloride, which would react with silver nitrate solution like this: CuCl2(aq) + 2 AgNO3(aq) → 2 AgCl(s) + Cu(NO3)2(aq) The chemist adds 75.0 mM silver nitrate solution to the sample until silver chloride stops forming. He then washes, dries, and weighs the precipitate. He finds he has collected 6.3 mg of silver chloride. Calculate the concentration of copper(II) chloride contaminant in the original groundwater sample. Round your answer to 2 significant digits. mg L