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A 0.075 molal solution of monobasic acid...

A 0.075 molal solution of monobasic acid has a freezing point of `-0.18^(@)C`. Calculate `K_(a)` for the acid , `(k_(f)=1.86)`

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To calculate the acid dissociation constant \( K_a \) for the monobasic acid from the given data, we will follow these steps: ### Step 1: Calculate the Depression in Freezing Point The depression in freezing point (\( \Delta T_f \)) can be calculated using the formula: \[ \Delta T_f = T_f^{\text{solvent}} - T_f^{\text{solution}} \] Given that the freezing point of pure water (solvent) is \( 0^\circ C \) and the freezing point of the solution is \( -0.18^\circ C \): ...
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