14. Solutions

Solutions: Mass Percent

Mass Percent of a Solution Made Easy: How to Calculate Mass % or Make a Specific Concentration

An aqueous LiNO2 solution is made using 90.3 g LiNO2 and diluting it to a total volume of 1.72 L. If the density of the solution is 1.20 g/mL, what is the mass percent of the solution?

Calculate the amount of water (in kilograms) that must be added to 12.0 g of urea, (NH2)2CO, in the preparation of a 18.3 percent by mass solution. The molar mass of urea, (NH2)2CO, is 60.055 g/mol.

A solution was prepared by dissolving 51.0 g of KBr in 310 mL of water. Calculate the mass percent of KBr in the solution.

A 10.0 M aqueous solution of NaOH has a density of 1.33 g/cm3 at 25 C. Calculate the mass percent of the NaOH in the solution (a) 53.2% (b) 30.1% (c) 40.0% (d) 13.3%

The rate of a first-order reaction is followed by spectroscopy,
monitoring the absorbance of a colored reactant at 520 nm.
The reaction occurs in a 1.00-cm sample cell, and the only
colored species in the reaction has an extinction coefficient
of 5.60 * 103 M-1 cm-1 at 520 nm. (a) Calculate the initial
concentration of the colored reactant if the absorbance is
0.605 at the beginning of the reaction.

Find the percent by mass of sodium chloride in a 1.35 M NaCl
solution. The density of the solution is 1.05 g/mL.

Calculate %m/m (Percent by Mass of a solution)

Expressing Concentration by Mass Percent

Mass Percent & Mole Fraction

Commercial aqueous nitric acid has a density of 1.42 g>mL 
and is 16 M. Calculate the percent HNO3 by mass in the 
solution.

Solutions: Mass Percent Example 2

Solutions: Mass Percent Example 1

How to Calculate Mass Percent of a Solution

How to Calculate Mass Percent of Solute and Solvent of Solution Examples and Practice Problems

Solutions: Mass Percent Concept 1

Ascorbic acid 1vitamin C, C6H8O62 is a water-soluble vitamin. A solution containing 80.5 g of ascorbic acid dissolved
in 210 g of water has a density of 1.22 g>mL at 55 °C. Calculate (a) the mass percentage,

Molarity, Molality, Volume & Mass Percent, Mole Fraction & Density - Solution Concentration Problems

Determine the percent sulfuric acid by mass of a 1.37 m aqueous solution of H2SO4.

Solutions: Mass Percent Concept 2

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Types of Aqueous Solutions

When an ionic solid dissolves, ions leave the solid and become dispersed in the solvent. Three possible aqueous solutions can be formed:saturated, unsaturated and supersaturated.

Boiling Point Elevation

Boiling Point Elevation is the phenomenon when adding a solute to a pure solvent results in increased boiling point of the solvent.

Intro to Henry's Law

According to&nbsp;Henry's Law, at a constant temperature the amount of a gas dissolved in a solvent is directly proportional to its partial pressure when it is in equilibrium with its liquid phase.&nbsp;

Osmotic Pressure

Osmotic Pressure is the force that drives Osmosis from higher concentration to lower concentration.

Mole Fraction

Mole Fraction (X) relates the moles of solute and solvent within a solution.&nbsp;

The Colligative Properties

The&nbsp;Colligative Properties&nbsp;explain what happens to a pure solvent as it transitions to a solution.

Molality

Molality (m)&nbsp;represents the number of moles of solute dissolved per kilogram of solvent.&nbsp;

Freezing Point Depression

Freezing Point Depression is the phenomenon when adding a solute to a pure solvent results in decreased freezing point of the solvent.

Solutions: Solubility and Intermolecular Forces

Solutions are homogeneous mixtures that result from the dissolving of a solute by a solvent.

Vapor Pressure Lowering (Raoult's Law)

Vapor Pressure is the pressure exerted by a gas at equilibrium with its liquid phase at a specific temperature in a closed system.

Henry's Law Calculations

To calculate solubility of a dissolves gas, Henry's Law Constant and partial pressure are used.

Mass Percent represents grams of solute per grams of solution, multiplied by 100.

Osmosis

Osmosis is the net movement of solvent across a semipermeable membrane.

Parts per Million (ppm)

<div dir="auto"><div contenteditable="true"dir="auto"spellcheck="true">Parts per Million (ppm) and Parts per Billion (ppb) are used to express extremely dilute solution concentrations.</div></div>

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