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Barium hydroxide has a solubility of $0.108 \textrm{ M}$ at $25 °C$ in water.

What is true about the solubility of barium hydroxide in a $0.200 \textrm{ M}$ aqueous solution of barium nitrate at $25 °C$?

A

The solubility would be decreased because the presence of nitrate ions increases the viscosity of the water.

B

The solubility would be decreased because the presence of barium ions shifts the equilibrium position of the solubility reaction towards the solid.

C

The solubility would be increased because the presence of barium ions increases the $K_{sp}$.

D

The solubility would be increased because the presence of nitrate ions surround the dissolving barium ions and push the equilibrium towards the dissolved ions.

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