Answered: The density of an aqueous solution…

The density of an aqueous solution increases as solutes such as salts are added. What bearing might this have on predicting whether the aqueous solution will be on the top or on the bottom for an

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.3QAP

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Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

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The density of an aqueous solution increases as solutes such as salts are added. What bearing might this have on predicting whether the aqueous solution will be on the top or on the bottom for an extraction?

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Protecting the products of dissolution
Why does the molarity of NaOH usually have to be standardized? When preparing the aqueous NaOH, the exact volume of the NaOH used cannot be measured due to water being hygroscopic. Solid NaOH can react with acid very easily and therefore the initial mass of the base may not be exact. When dissolving the solid NaOH in pure distilled water, the exact volume of the NaOH used cannot be measured due to buret calibration. Solid NaOH can react with water in the air very easily and therefore the initial mass of the base may not be exact.
When a nonvolatile solute such as ammonium sulfate is dissolved in a solvent like water, one of the observed effects is an increase in the vapor pressure of the solute. B scattering of light beams by the solute particles in the solution. an increase in the freezing point of the liquid. a decrease in the vapor pressure of the solvent. a decrease in the boiling point of the liquid.
One way to increase the solubility of an insoluble salt is to increase the ionic strength of the solution. stir the solution vigorously. decrease the ionic strength of the solution. add more of the insoluble salt to the solution.
0.010 mL of 0.1M Fe(II) is mixed with 9.990 mL of 0.1M Fe(III). What is the mole fraction of Fe(II)?
How do we keep relative supersaturation low by controlling solubility? solubility should be higher solubility should be constant solubility should be lower solubility should be fluctuating
2. You have a solution that contains 4.0g of oxalic acid dissolved in 100 mL of water. This solution is placed in a separatory funnel, and then 100 mL of diethyl ether is added to the separatory funnel and an extraction is performed. (Diethyl ether and water are immiscible solvents.) Use the following constants to calculate how much oxalic acid is in each solvent after the extraction. Solubility of oxalic acid in water = 9.5 g / 100 mL Solubility of oxalic acid in ether = 16.9 g/100 mL
This is normally prepared by increasing the temperature of the solvent to allow the dissolution of more solute
What is the molar concentration resulting from mixing 25 mL of 2M and 100 mL of 4M?
The dissolution of solute into a solvent can be dependent on a variety of factors. These include the pH, the ionic strength (amount of salt dissolved), temperature, etc. Other ways to discuss solutions are turbidity, purity, clarity. Pick one of the these factors and discuss.
Predicting the products of dissolution.
Predicting the products of dissolution.