The solubility differs from concentration because concentration is amount of solute per volume of solution and solubility is moles of solute per volume of solution. O solubility is grams of solvent per volume of solution where concentration is amount of solute per volume of solution. concentration is grams of solute per volume of solution and the other is moles of solute per volume of solution. O solubility is grams of solute per volume of solvent and concentration is amount of solute per volume of solution. concentration is moles of solute per volume of solvent and solubility is mass of solute per volume of solution.

The solubility differs from concentration because concentration is amount of solute per volume of solution and solubility is moles of solute per volume of solution. O solubility is grams of solvent per volume of solution where concentration is amount of solute per volume of solution. concentration is grams of solute per volume of solution and the other is moles of solute per volume of solution. O solubility is grams of solute per volume of solvent and concentration is amount of solute per volume of solution. concentration is moles of solute per volume of solvent and solubility is mass of solute per volume of solution.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter6: Types Of Chemical Reactions And Solution Stoichiometry

Section: Chapter Questions

Problem 4RQ

See similar textbooks

Similar questions

A student weighs out a 4.80-g sample of aluminum bromide, transfers it to a 100-mL volumetric flask, adds enough water to dissolve it, and then adds water to the 100-mL mark. What is the molarity of aluminum bromide in the resulting solution?
The units of parts per million (ppm) and parts per billion (ppb) are commonly used by environmental chemists. In general, 1 ppm means 1 part of solute for every 106 parts of solution. Mathematically, by mass: ppm=gsolutegsolution=mgsolutekgsolution In the case of very dilute aqueous solutions, a concentration of 1.0 ppm is equal to 1.0 g of solute per 1.0 mL, which equals 1.0 g solution. Parts per billion is defined in a similar fashion. Calculate the molarity of each of the following aqueous solutions. a. 5.0 ppb Hg in H2O b. 1.0 ppb CHCl3 in H2O c. 10.0 ppm As in H2O d. 0.10 ppm DDT (C14H9Cl5) in H2O
On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
What is the difference between a solute and a solvent?
ssume a highly magnified view of a solution of HCI that allows you to “see” the HCl. Draw this magnified view. If you dropped in a piece of magnesium, the magnesium would disappear, and hydrogen gas would he released. Represent this change using symbols for the elements, and write the balanced equation.
What mass of HCl is contained in 45.0 mL of an aqueous HCl solution that has a density of 1.19 g cm-3 and contains 37.21% HCl by mass?
How do we define the mass percent composition of a solution? Give an example of a solution, and explain the relative amounts of solute and solvent present in the solution in terms of the mass percent composition.
A solution is defined as a homogeneous mixture. Is a small sample of air a solution? Is the atmosphere a solution?
A student was given a 1.6240-g sample of a mixture of sodium nitrate and sodium chloride and was asked to find the percentage of each compound in the mixture. She dissolved the sample and added a solution that contained an excess of silver nitrate. The silver ion precipitated all of the chloride ion in the mixture as silver chloride. It was filtered, dried, and weighed. Its mass was 2.056g. What was the percentage of each compound in the mixture?