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# When $25.0 \mathrm{~mL}$ of $0.500 \mathrm{M}$ iron(II) sulfate is combined with $35.0 \mathrm{~mL}$ of $0.332 \mathrm{M}$ barium hydroxide, two different precipitates are formed. (a) Write a net ionic equation for the reaction that takes place. (b) Estimate the mass of the precipitates formed. (c) What are the equilibrium concentrations of the ions in solution?

Solution

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We are mixing two solutions :

$V\mathrm{(FeSO_4)=25.0~mL}$

$c\mathrm{(FeSO_4)=0.5~M}$

$V\mathrm{(Ba(OH)_2)=35~mL}$

$c\mathrm{(Ba(OH)_2)=0.332~M}$

$\textcolor{#4257b2}{\text{Subtask A}}$

• we need to write the net ionic equation for this reaction

$\textcolor{#4257b2}{\text{Subtask B}}$

• we need to determine the masses of the products

$\textcolor{#4257b2}{\text{Subtask C}}$

• we need to calculate the equilibrium concentrations of the ions

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