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Molarity is the number of moles of a solvent contained in 1 liter of the solution.
False
Normality is the number of equivalents of solute contained in 1 liter of solution.
True
Weight percent is a common method used to express the concentration of commercial aqueous reagents.
True
In the calculation of n for base, n represents the number of replaceable H+1 ions.
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The molar concentration of ethanol in an aqueous solution can be calculated using the mass and molar mass of C2H5OH.
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The percent concentration is commonly used to express concentrations in terms of parts per thousand.
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A 70% (w/w) solution of nitric acid means there are 70 g of nitric oxide per 100 g of solution.
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When a solution is described as 5% (v/v) methanol, it means 5.0 g of methanol is diluted with enough water to give 100 mL.
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Weight to volume percent is commonly used to indicate the composition of concentrated aqueous solutions.
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Parts per million (ppm) is a convenient way to express concentration for very concentrated solutions.
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Diluting 20 mL of 10 N HCl with distilled water to make one liter will result in a diluted solution with a normality higher than 10 N.
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In a 5% (w/v) aqueous silver nitrate solution, 5 g of silver nitrate is dissolved in enough water to make 100 mL of solution.
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