How many milligrams of calcium chloride (CaCl2., molecular weight = 111 g / mol ) are needed to

Step 1: Calculate the molar mass of calcium chloride (CaCl2). The molar mass of CaCl2 is 40.08 g

How many milligrams of calcium chloride (CaCl2., molecular...

How many milligrams of calcium chloride $\left(\mathrm{CaCl}_2\right.$, molecular weight $=$ $111 \mathrm{~g} / \mathrm{mol}$ ) are needed to prepare $750 \mathrm{~mL}$ of solution containing $10 \mathrm{mEq} / \mathrm{L}$ of $\mathrm{Ca}^{+2}$ ?

Key Concepts

Milliequivalent Concept

Milliequivalents (mEq) represent a measure of the chemical activity of ions in a solution based on their charge. It allows for the conversion between the amount in moles and the effective concentration of ions, which is particularly useful when the ion in question has a charge other than one. This concept is essential in ensuring that the amount of an ionic species in a solution is correctly calculated, especially when dealing with electrolytes that dissociate in solution.

Molarity and Concentration Units

Molarity, defined as moles of solute per liter of solution, is a key concentration unit used in preparing chemical solutions. Converting between different volume units (such as milliliters to liters) is an important step in these calculations. Understanding how to adjust molarity or related concentration values to different volumes is critical in preparing solutions with precise concentrations.

Molecular Weight and Mass-Mole Relations

The molecular weight of a compound, expressed in grams per mole, is used as a conversion factor between the mass of a substance and the number of moles present. This concept is crucial for translating a chemical requirement given in equivalents or moles into a measurable mass, such as grams or milligrams, when preparing solutions.

Stoichiometric Relationships in Dissociation

Stoichiometry involves using the balanced relationship between reactants and products to determine the quantities needed in a chemical reaction or solution. In the context of ionic compounds that dissociate, understanding how the compound breaks apart into its constituent ions allows for the correct calculation of the amount of compound required to provide a specific amount of an ion in the final solution.

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