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Hydrochloric acid is usually purchased in a concentrated form that is 37.0 $%$ $H C l$ by mass and has a density of 1.20 $g / m L$ . How much concentrated solution would it take to prepare 2.95 L of 0.480 M HCl upon dilution with water?

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champagnemammoth903

Concentrated hydrochloric acid is 37.0% HCL by weight and has aspecific gravity of 1.19 (density = 1.19 g/mL). What volume of thisacid must be diluted to 500 mL to produce a 0.300 M solution ofthis acid?

(Mol. wt HCL = 36.5 g/mole)

How much concentrated solution would you take to prepare 2.85 of0.570 by mixing with water? HCl is purchased in 37% mass and has adensity of 1.20 g/mL.

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Hydrochloric acid is usually purchased in a concentrated form that is 37.0 $%$ $H C l$ by mass and has a density of 1.20 $g / m L$ . How much concentrated solution would it take to prepare 2.95 L of 0.480 M HCl upon dilution with water?

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Hydrochloric acid is usually purchased in a concentrated form that is 37.0% HCl by mass and has a density of 1.20 g/mL. How much concentrated solution would it take to prepare 2.95 L of 0.480 M HCl upon dilution with water?

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Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Principles of Chemistry Molecular Approach

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

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Hydrochloric acid is usually purchased in a concentrated form that is 37.0 $%$ $H C l$ by mass and has a density of 1.20 $g / m L$ . How much concentrated solution would it take to prepare 2.95 L of 0.480 M HCl upon dilution with water?