Answer
a. 1.1 mEq/L
b. Below the normal range.
Work Step by Step
a.
1. Identify the conversion factors.
Molar mass of magnesium: $24.31 \space g/mole$
$1 \space L = 10 \space dL$
Magnesium has a charge of +2: 1 mole $Mg^{2+}$ = 2 Eq $Mg^{2+}$
$1 \space Eq = 1000 \space mEq$
2. Convert the concentration to mEq/L:
$$\frac{0.0026 \space g}{dL} \times \frac{10 \space dL}{1 \space L} \times \frac{1 \space mole}{24.31 \space g} \times \frac{1 \space Eq}{1 \space mole} \times \frac{1000 \space mEq}{1 \space Eq}= \frac{1.1 \space mEq}{L} $$
b. According to the Table 9.6, the normal concentration of $Mg^{2+}$ in blood plasma is between 1.5 and 3.0 mEq/L. Since 1.1 mEq/L is less than 1.5 mEq/L, this value is below the normal range.