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If a solution containing 6 g of tripheny...

If a solution containing `6 g` of triphenyl methane, `(C_(6)H_(5))_(3)CH ("molecular weight" =244)`,in `1000 g` of benzene is cooled to `0.22^(@)C`.below the freezing point of benzene, how much solvent will crystallize out and what will be the molality of residual solution? `(K_(f)=5.1 K m^(-1))`

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To solve the problem step by step, we will follow these calculations: ### Step 1: Calculate the change in freezing point (ΔTf) We know that the freezing point depression is given by the formula: \[ \Delta T_f = K_f \times m \] where \(K_f\) is the cryoscopic constant and \(m\) is the molality of the solution. ...
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