Concentrations of Solutions

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Concentration Noun

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[kon-sen-tray-shun]

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Concentration

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A measure of the amount of solute that is dissolved in a given quantity of solvent or a total solution.

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Example: This diagram shows a solution in a beaker, with a magnified view revealing the individual solute particles (pink) evenly mixed among the solvent particles (blue).

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Solute Noun

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[sol-yoot]

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Solute

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The substance that is dissolved in a solvent to form a solution, typically present in a smaller amount.

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Example: This diagram shows a solution, where the solute (white particles) is the substance that gets dissolved into the solvent (blue liquid).

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Solvent Noun

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[sol-vent]

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Solvent

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The substance in which a solute dissolves to produce a solution, typically present in a larger amount.

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Example: This diagram shows how a solvent, like the water molecules, surrounds and pulls apart the particles of a solute (the ions), causing it to dissolve.

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Dilute Solution Noun

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[di-loot suh-loo-shun]

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Dilute Solution

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A solution that contains a relatively small amount of solute compared to the amount of solvent present.

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Example: This diagram shows that adding more solvent (the liquid from the dropper) to a concentrated solution creates a dilute solution, which has less solute per unit of volume.

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Concentrated Solution Noun

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[kon-sen-tray-ted suh-loo-shun]

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Concentrated Solution

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A solution that contains a relatively large amount of solute compared to the amount of solvent present.

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Example: This diagram shows that a concentrated solution has a large amount of solute (salt) dissolved in the solvent, while a dilute solution has less.

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Molarity (M) Noun

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[moh-lar-i-tee]

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Molarity (M)

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A unit of concentration defined as the number of moles of solute dissolved in one liter of total solution.

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Example: This diagram shows that molarity (concentration) depends on two things: the amount of solute (drink mix) and the volume of the solution.

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Mole Noun

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[mohl]

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Mole

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The SI base unit for amount of substance, representing approximately 6.022 x 10^23 elementary entities like atoms or molecules.

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Example: One mole of a substance, like carbon-12, has a mass of 12 grams and contains a specific, very large number of atoms (Avogadro's number).

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Molar Mass Noun

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[moh-ler mas]

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Molar Mass

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The mass of one mole of a chemical substance, which is typically expressed in units of grams per mole (g/mol).

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Example: The molar mass of a water molecule (H₂O) is calculated by adding the mass of two hydrogen atoms and one oxygen atom.

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Volumetric Flask Noun

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[vol-yoo-me-trik flask]

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Volumetric Flask

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Laboratory glassware calibrated to contain a precise volume at a specific temperature, used for preparing standard solutions.

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Example: This diagram shows a volumetric flask used to measure a precise volume. The magnified view shows the liquid's curved surface (meniscus) correctly aligned with the flask's calibration mark.

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Dilution Noun

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[di-loo-shun]

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Dilution

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The process of reducing the concentration of a solute in a solution, which is typically done by adding more solvent.

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Example: This image shows a series of beakers where a colored solution becomes progressively lighter, visually representing how dilution decreases the concentration of a substance.