Answer:
A precipitate will form, BaCO₃
Explanation:
When Ba²⁺ and CO₃²⁻ ions are in an aqueous media, BaCO₃(s), a precipitate, is produced following its Ksp expression:
Ksp = 5.1x10⁻⁹ = [Ba²⁺] [CO₃²⁻]
<em>Where the concentrations of the ions are the concentrations in equilibrium</em>
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For actual concentrations of a solution, you can define Q, <em>reaction quotient, </em>as:
Q = [Ba²⁺] [CO₃²⁻]
<em>If Q > Ksp, the ions will react producing BaCO₃, if not, no precipitate will form</em>.
Actual concentrations of Ba²⁺ and CO₃²⁻ are:
[Ba²⁺] = [Ba(NO₃)₂] = 1.1x10⁻³ × (20.0mL / 100.0mL) = 2.2x10⁻⁴M
[CO₃²⁻] = [Na₂CO₃] = 8.4x10⁻⁴ × (80.0mL / 100.0mL) = 6.72x10⁻⁴M
<em>100.0mL is the volume of the mixture of the solutions</em>
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Replacing in Q expression:
Q = [Ba²⁺] [CO₃²⁻]
Q = [2.2x10⁻⁴M] [6.72x10⁻⁴M]
Q = 1.5x10⁻⁷
As Q > Ksp
<h3>A precipitate will form, BaCO₃</h3>
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