How many grams of solute would you use to prepare each of...

How many grams of solute would you use to prepare each of the following solutions? (a) 250.0 $\mathrm{mL}$ of 0.600 $\mathrm{M}$ ethyl alcohol ( $\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O} )$ (b) 167 $\mathrm{mL}$ of 0.200 $\mathrm{M}$ boric acid $\left(\mathrm{H}_{3} \mathrm{BO}_{3}\right)$

How many grams of solute would you use to prepare each of the following solutions?
(a) 250.0 $\mathrm{mL}$ of 0.600 $\mathrm{M}$ ethyl alcohol ( $\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O} )$
(b) 167 $\mathrm{mL}$ of 0.200 $\mathrm{M}$ boric acid $\left(\mathrm{H}_{3} \mathrm{BO}_{3}\right)$

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Key Concepts

Molarity

Molarity is defined as the number of moles of solute per liter of solution. This concept is crucial in solution preparation as it provides the relationship necessary to determine how many moles of a substance are needed based on the desired concentration and volume of the solution.

Volume Conversion

Volume conversion involves changing the units of volume, typically from milliliters to liters, since molarity is expressed as moles per liter. Ensuring the volume is in the correct unit is essential for accurate calculations when preparing solutions.

Mole Concept

The mole is a fundamental unit in chemistry that quantifies the amount of substance based on a fixed number of particles. Understanding this concept allows for the practical use of molar relationships to calculate the amount of solute required in chemical solutions.

Molar Mass

Molar mass is the mass of one mole of a substance, expressed in grams per mole. This property enables the conversion of moles to grams, an essential step when measuring out a specific mass of solute to prepare a solution with a desired molarity.

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