A prescription order calls for 1500 mL solution of potassium sulfate to be made so that it will

Step 1: Calculate the molecular weight of potassium ion (K+) The molecular weight of potassium i

A prescription order calls for 1500 mL solution of...

A prescription order calls for $1500 \mathrm{~mL}$ solution of potassium sulfate to be made so that it will contain $15 \mathrm{mEq}$ of $\mathrm{K}^{+}$ion. How many milligrams of potassium sulfate $\left(\mathrm{K}_2 \mathrm{SO}_4\right.$, molecular weight $\left.=174 \mathrm{~g} / \mathrm{mol}\right)$ are needed?

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Key Concepts

Milliequivalents (mEq)

A milliequivalent is a unit used to express the chemical activity of ions in solution, taking into account both the concentration and the charge of the ion. It is particularly useful in medical and chemical calculations to ensure the precise dosage of ionic compounds, where 1 mEq corresponds to one-thousandth of an equivalent, reflecting the amount of substance that can react in a manner determined by its charge.

Molecular Weight and Mass Conversion

Molecular weight represents the mass of one mole of a substance, calculated as the sum of the atomic weights of its constituent atoms. This concept is critical when converting between the number of moles and the mass (in grams or milligrams) of a compound, facilitating the preparation of solutions with an accurate concentration of the compound or its ions.

Ionic Stoichiometry

Ionic stoichiometry involves understanding the ratio of ions produced by a compound when it dissolves. For ionic compounds, such as salts, knowing the number of ions (and their respective charges) released per formula unit allows one to relate the measured quantity of a specific ion (given in mEq) to the amount of the whole compound needed. This ensures that the solution contains the exact required concentration of the ion.

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