22. Which of the following does have an impact on the amount of a solid that wil

Question

22. Which of the following does have an impact on the amount of a solid that will dissolve in liquid solvent?

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Question 231 pts

23. The partial pressure of oxygen gas, O2, over a 25.0 mL sample of water at a constant temperature of 25°C is increased. What effect does it have on the solubility of the gas in water?

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Question 241 pts

24. What are the units of the concentration term best used when temperature changes are occurring?

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Question 251 pts

25. Which of the following is not a solution property that depends upon the number of particles dissolved?

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Question 261 pts

26. What is the concentration in molality of a homogeneous saturated solution of aluminum sulfate, Al2(SO4)3 at 20°C. The solubility limit is 75.4 g per 100 g of water at 20°C.

Explanation / Answer

Answer)

Temperature.

When the temperature of a substance is raised, the kinetic energy of the molecule increases, which help the molecules to overcome the attractive forces among themselves. The solute particles tend to leave the surface of the solid and dissolve into the liquid phase. Thus, increasing the temperature usually increases the solubility of substances. For example, sugar is more soluble in water at higher temperatures. Stirring only increases the speed of the dissolving.

Answer:

Increase

The solubility of gas shall increase if the pressure increases, whereas a decrease in pressure decreases solubility. This is in accordance with Henry's Law, which states that the solubility of a gas in a liquid is directly proportional to the pressure of that gas above the surface of the solution.

Answer:

(moles of solute)/(kg of solvent)

At higher temperatures, volumes of liquids increase, while at lower temperatures, volumes of liquids decrease. Therefore, molarities (moles of solute/L of solution) also vary at different temperatures. Because volume is not a part of its equation, it makes molality independent of temperature and hence best suited.

Answer:

Molar mass of the solute

Colligative properties of solutions are properties that depend upon the concentration of solute molecules or ions. Colligative properties include freezing point depression, boiling point elevation, vapour pressure lowering, and osmotic pressure.

Answer:

2.20 m

Molar mass of Al2(SO4)3*18H2O is 342.2 g/mol

we have 75.4 g of Al2(SO4)3

number of moles = 75.4 / 342.2 = 0.22034 or 2.20 * 10 ^ -1 moles

Molality is (moles of solute)/(kg of solvent)

This implies, 0.22 mol is present in 100 g,

So for molality, 1000g is concerned

=0.22 *1000/100 = 2.20 m

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