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| aqueous solution | solution for which water is the solvent
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| Avogadro’s number (NA) | experimentally determined value of the number of entities comprising 1 mole of substance, equal to 6.022 × 1023 mol−1
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| concentrated | qualitative term for a solution containing solute at a relatively high concentration
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| concentration | quantitative measure of the relative amounts of solute and solvent present in a solution
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| dilute | qualitative term for a solution containing solute at a relatively low concentration
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| dilution | process of adding solvent to a solution in order to lower the concentration of solutes
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| dissolved | describes the process by which solute components are dispersed in a solvent
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| empirical formula mass | sum of average atomic masses for all atoms represented in an empirical formula
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| formula mass | sum of the average masses for all atoms represented in a chemical formula; for covalent compounds, this is also the molecular mass
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| mass percentage | ratio of solute-to-solution mass expressed as a percentage
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| mass-volume percent | ratio of solute mass to solution volume, expressed as a percentage
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| molar mass | mass in grams of 1 mole of a substance
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| molarity (M) | unit of concentration, defined as the number of moles of solute dissolved in 1 liter of solution
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| mole | amount of substance containing the same number of atoms, molecules, ions, or other entities as the number of atoms in exactly 12 grams of 12C
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| parts per billion (ppb) | ratio of solute-to-solution mass multiplied by 109
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| parts per million (ppm) | ratio of solute-to-solution mass multiplied by 106
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| percent composition | percentage by mass of the various elements in a compound
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| solute | solution component present in a concentration less than that of the solvent
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| solvent | solution component present in a concentration that is higher relative to other components
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| volume percentage | ratio of solute-to-solution volume expressed as a percentage
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