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Question

When 25.0 mL25.0 \mathrm{~mL} of 0.500M0.500 \mathrm{M} iron(II) sulfate is combined with 35.0 mL35.0 \mathrm{~mL} of 0.332M0.332 \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?

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The task

We are mixing two solutions :

V(FeSO4)=25.0 mLV\mathrm{(FeSO_4)=25.0~mL}

c(FeSO4)=0.5 Mc\mathrm{(FeSO_4)=0.5~M}

V(Ba(OH)2)=35 mLV\mathrm{(Ba(OH)_2)=35~mL}

c(Ba(OH)2)=0.332 Mc\mathrm{(Ba(OH)_2)=0.332~M}

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

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

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

  • we need to determine the masses of the products

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

  • we need to calculate the equilibrium concentrations of the ions

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