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Darya [45]
2 years ago
9

What is the expected freezing-point depression for a solution that contains 2.0 mol of KCI

Chemistry
1 answer:
larisa86 [58]2 years ago
8 0

Answer:

a. -7.44 °C

Explanation:

Hello there!

In this case, since the freezing point depression formula is:

\Delta T_f=-i*m*Kf

Thus, since the Van't Hoff's factor is 2 for KCl as it ionizes in K⁺ and Cl⁻, the molarity is 2.0 m (2.0mol/1.0kg) and the freezing point depression constant is 1.86 °C/m, we calculate the freezing point depression as follows:

\Delta T_f=-2*2.0m*1.86\°C /m\\\\\Delta T_f=-7.44\°C

Therefore, the answer is a. -7.44 °C.

Regards!

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Muriatic acid, HCl, is often used to remove rust. A solution of muriatic acid, HCl, reacts with Fe2O3 deposits on industrial equ
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Step 1:

The balanced equation for the reaction.

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Step 2 :

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From the balanced equation above,

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Step 3:

Determination of the mass of HCl needed to react with 439g of Fe2O3. This is illustrated below:

From the balanced equation above,

159.70g of Fe2O3 reacted with 218.76g of HCl.

Therefore, 439g of Fe2O3 will react with = (439 x 218.76) /159.70 = 601.35g of HCl.

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Conversion of 601.35g of HCl to mole. This is illustrated below:

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