Estimate how much the salinity of the surface water of the Arctic Ocean would need to increase before the surface density would equal the potential density at 1000-m depth. how does this compare with the average salinity of the ocean? (Good values might be T=-1.5˚C, S = 32.8, and potential density about 24.5.)

Estimate how much the salinity of the surface water of the Arctic Ocean would need to increase before the surface density would equal the potential density at 1000-m depth. how does this compare with the average salinity of the ocean? (Good values might be T=-1.5˚C, S = 32.8, and potential density about 24.5.)

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter12: Solutions

Section: Chapter Questions

Problem 12.62QE

See similar textbooks

Similar questions

Why do Sedimentation and filtration is important in water treatment? Is a period of time important in water purification?
Specify how the principle of constant proportions can be used to determine seawater salinity by measuring only one dissolved component.
Compare and contrast chlorinity and salinity. What is/are the importance of measuring water salinity?
The ubiquitous single-cell yeast (S. cerevisiae) is roughly spherical with a “typical” diameter of 5 μm. Let’s make a rough approximation of how many water molecules are in a yeast cell.a) What is the molar volume of liquid water? You may assume dH2O = 1.00 g/mlb) What is the volume occupied by a single water molecule?c) Approximately how many molecules of water are in a “typical” yeast cell?Assume the cell is composed completely of pure water with density equal to 1.00 g/mL (a more realistic estimate is ~70% water content by volume, but don’t worry about this).
Seawater consists of many important elements in the form of salts dissolved in the water. At 25°C the mass percentage of salts in seawater will total 3.5% m/m. The density of seawater at this temperature and salt percentage is 1.024 kg/L. Study the chart and answer the questions below: 1. The chart assumes 1000.0 g of seawater. What volume, Vsoln (L), does this correspond to at 25 °C? 2. The diagram claims that chloride ions make up 55% m/m of all salt ions. Confirm this number. if possible, I would like handwritten answers with calculations. Thanks :)
Conductivity measurements of aqueous solutions of MgCl, (strong electrolyte) were done and the following results were obtained. Concentration, mol/L 5.625 x 107 2.250 x 10 6.250 x 10 Specific conductance, 5/cm 7.01 x 10 2.79 x 107 7.54 x 107 Calculate the limiting molar conductivity (S-cm²/mol). Report your answer in 2 decimal places.
A certain liquid X has a normal freezing point of 6.90°C and a freezing point depression constant =Kf 2.27·°C·kgmol−1. Calculate the freezing point of a solution made of 92.g of glycine (C2H5NO2) dissolved in 700. g of X. Round your answer to 2 significant digits.
You are asked to calculate molar conductivity of a NaCl solution with a concentration of 0.03125 mol/L according to the following equation, where χ is the conductivity and is 1.41x10-3 (±0.02) ohm^-1 cm^-1 and C is the concentration of the solution. The uncertainty of the volume measurement in determining concentration is given as ±0.02 and the mole value is given with no significant error. Calculate molar conductivity in ohm^-1 cm2mol^-1 and give your result with necessary significant figures.
You make a calibration curve using dilute concentrations of dye and determine the equation of the line is y = 7.325 x. If the pathlength of the machine you are using is 1 cm, what is ε in Beer’s law for this solute? What are its units?
A certain liquid X has a normal freezing point of 3.30°C and a freezing point depression constant =Kf 5.91·°C·kgmol−1. Calculate the freezing point of a solution made of 9.69 g of benzamide (C7H7NO) dissolved in 400.g of X. Round you answer to 3 significant digits.
Question 5 Which of the following statement/s is/are TRUE? I. The Arrhenius Theory cannot be applied to account for the behavior of the molar conductivity of strong electrolytes, since these solutes are completely dissociated, at least in dilute solutions. II. Debye=Huckel Theory of interionic attraction satisfactorily explains the variation of the molecular conductivity of strong electrolytes with concentration. III. The ions interact with the solvent molecules through dipole-dipole interaction. IV. When an electric potential is applied across the solution, the ions migrate and the ionic atmosphere around these ions is modified. O I, II, II O II, II, IV O ,I O I, II O I, II, IV
A certain liquid X has a normal boiling point of 92.90°C and a boiling point elevation constant Kb=2.15·°C·kgmol−1. Calculate the boiling point of a solution made of 30.g of potassium bromide (KBr) dissolved in 800.g of X. Round your answer to 3 significant digits.