A solution of potassium hydroxide is in equilibrium with undissolved solute at 4

Question

A solution of potassium hydroxide is in equilibrium with undissolved solute at 45°C. What will happen if the temperature is raised to 50°C? (Hsoln = -57.6 kJ/mol)

A.  

The mass of dissolved KOH will increase.

B.  

The mass of dissolved KOH will decrease.

C.  

The mass of dissolved KOH will be unchanged.

D.  

The mass of water in the solution will increase.

E.  

More information is needed in order to make a reliable prediction.

Please explain.

A solution of potassium hydroxide is in equilibrium with undissolved solute at 45°C. What will happen if the temperature is raised to 50°C? (Hsoln = -57.6 kJ/mol)

Explanation / Answer

Ans : B

KOH(s) <=======> KOH(aq) ; (Hsoln = -57.6 kJ/mol)

Hsoln = -57.6 kJ/mol => The process is exothermic

According to LeChatlier's principle, If temperature is increased then the equilibrium is shifted in the direction where temperayure in decreasing. Here it is backward direction. Therefore, the mass of dissolved KOH will decrease.

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