Answer
a. 2 Eq $Mg^{2+}$
b. 0.5 Eq $H^+$
c. 4 Eq $Cl^-$
d. 6 Eq $Fe^{3+}$
Work Step by Step
1. Identify the absolute value of the charge of each ion.
a. 2
b. 1
c. 1
d. 3
2.
1 mole of each compound is equal to "x" Eq of the same compound. In this case, for ions, x is equal to the absolute value of the charge in each ion.
a. $1 \space mole \space Mg^{2+} = 2 \space Eq \space Mg^{2+}$
b. $1 \space mole \space H^+ = 1 \space Eq \space H^+$
c. $1 \space mole \space Cl^- = 1 \space Eq \space Cl^-$
d. $1 \space mole \space Fe^{3+} = 3 \space Eq \space Fe^{3+}$
3. Use these as conversion factors:
a. $$1 \space mole \space Mg^{2+} \times \frac{2 \space Eq \space Mg^{2+}}{1 \space mole \space Mg^{2+}} = 2 \space Eq \space Mg^{2+}$$
b. $$0.5 \space mole \space H^+ \times \frac{1 \space Eq \space H^+}{1 \space mole \space H^+} = 0.5 \space Eq \space H^+$$
c. $$4 \space moles \space Cl^- \times \frac{1 \space Eq \space Cl^-}{1 \space mole \space Cl^-} = 4 \space Eq \space Cl^-$$
d. $$2 \space moles \space Fe^{3+} \times \frac{3 \space Eq \space Fe^{3+}}{1 \space mole \space Fe^{3+}} = 6 \space Eq \space Fe^{3+}$$
