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kupik [55]
3 years ago
15

The freezing-point depression of a 0.100 m MgSO4 solution is 0.225°C. Determine the experimental van't Hoff factor of MgSO4 at t

his concentration. (Kf of water is 1.86°C/m)
Chemistry
1 answer:
Andrews [41]3 years ago
7 0

<u>Answer:</u> The experimental van't Hoff factor is 1.21

<u>Explanation:</u>

The expression for the depression in freezing point is given as:

\Delta T_f=iK_f\times m

where,

i = van't Hoff factor = ?

\Delta T_f = depression in freezing point  = 0.225°C

K_f = Cryoscopic constant  = 1.86°C/m

m = molality of the solution = 0.100 m

Putting values in above equation, we get:

0.225^oC=i\times 1.86^oC/m\times 0.100m\\\\i=\frac{0.225}{1.86\times 0.100}=1.21

Hence, the experimental van't Hoff factor is 1.21

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Answer:

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1. From the equation,

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Therefore, 74g of HCl will produce = (74 x 2)/73 = 2.03g

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4 0
4 years ago
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In-s [12.5K]
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                                     1.  Sodium Stearate C₁₇H₃₅COONa
                                   
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When Soap is treated with MgCl₂ or CaCl₂ it forms insoluble precipitate called S.C.U.M. The reactions with MgCl₂ are as follow,

                2C₁₇H₃₅COONa + MgCl₂  -------->  2C₁₇H₃₅COOMg  + 2 NaCl

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3 years ago
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