QuestionExample Write chemical equations showing the dissociation of $\mathrm{MgSO}_{4}(\mathrm{aq})$ and $\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})$ .

Studdy Solution

STEP 1

1. We are dealing with aqueous solutions of magnesium sulfate ( $\mathrm{MgSO}_{4}(\mathrm{aq})$ ) and lead(II) nitrate ( $\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})$ ).
2. The compounds will dissociate into their respective ions in water.
3. We need to write the balanced chemical equations for the dissociation.

STEP 2

1. Identify the ions formed from the dissociation of each compound.
2. Write the balanced chemical equation for the dissociation of $\mathrm{MgSO}_{4}(\mathrm{aq})$ .
3. Write the balanced chemical equation for the dissociation of $\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})$ .

STEP 3

Identify the ions formed from the dissociation of each compound.
For $\mathrm{MgSO}_{4}(\mathrm{aq})$ , the ions are $\mathrm{Mg}^{2+}(\mathrm{aq})$ and $\mathrm{SO}_{4}^{2-}(\mathrm{aq})$ .
For $\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})$ , the ions are $\mathrm{Pb}^{2+}(\mathrm{aq})$ and $\mathrm{NO}_{3}^{-}(\mathrm{aq})$ .

STEP 4

Write the balanced chemical equation for the dissociation of $\mathrm{MgSO}_{4}(\mathrm{aq})$ .
$\mathrm{MgSO}_{4}(\mathrm{aq}) \rightarrow \mathrm{Mg}^{2+}(\mathrm{aq}) + \mathrm{SO}_{4}^{2-}(\mathrm{aq})$

STEP 5

Write the balanced chemical equation for the dissociation of $\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq})$ .
$\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq}) \rightarrow \mathrm{Pb}^{2+}(\mathrm{aq}) + 2\mathrm{NO}_{3}^{-}(\mathrm{aq})$

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