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Hands-on chemistry activities. Course challenge. Test your knowledge of the skills in this course. Start Course challenge. Science; High school chemistry; Unit 5: Stoichiometry and the mole. 800 possible mastery points. Mastered. Proficient. Familiar. Attempted. Not started. Quiz. Unit test.
Molarity, molality, osmolarity, osmolality, and tonicity - what's the difference?
Learn how molarity and molality differ! The molality of a solution is equal to the moles of solute divided by the mass of solvent in kilograms, while the molarity of a solution is equal to the moles of solute divided by the volume of solution in liters.
Molarity is a unit of concentration, with units of moles of solute/ liters of solvent. Concentration being how much of a substance is in a given volume. A solvent being a liquid into which something is dissolved into, which is referred to as the solute.
In this first unit of class 11 chemistry, we learn the significance of scientific notation, rules to calculate significant figures, the laws governing the combination of different atoms, mole concept, stoichiometry that involves the study of amount of substances that are involved in reactions, and modes of expressing concentration of the solution.
The most common way to express solution concentration is molarity (M), which is defined as the amount of solute in moles divided by the volume of solution in liters: M = moles of solute/liters of solution.
To do so, first prepare an ICE (Initial, Change, and Equilibrium) table showing the equilibrium concentrations of the ions in terms of x, the molar solubility of the compound. Then, plug these expressions into the solubility-product expression for the compound and solve for the value of x. Created by Jay.
Rate law and reaction order. Worked example: Determining a rate law using initial rates data. Units of the rate constant. Introduction to rate law.
The molarity or molar concentration of a solute is defined as the number of moles of solute per liter of solution (not per liter of solvent!): What is a mole? To learn more about how moles are used in chemistry, see this video on the mole and Avogadro's number .