Which of the following is true for the solubility of KBr (s) and CH 3 (CH 2 ) 3 CH 3 (g) in water?

Which of the following is true for the solubility of solid potassium bromide and gaseous pentane in water? Alright, so decreasing the temperature will decrease the solubility of gaseous pentane. So, remember we said that if you increase the temperature you're going to decrease the solubility of your gas. Here we're doing the opposite, here we are decreasing our temperature, so we should expect some increasing in the solubility of our gas, not a decrease, so this is not true. Next, increasing the pressure will decrease the solubility of potassium bromide. Remember we said that increasing, decreasing, playing around the pressure has little to no effect on solids and liquids. So here, increasing the pressure shouldn't necessarily decrease the solubility. This is not true. Both potassium bromide and pentane are completely soluble in water. Well, potassium bromide is an ionic compound and a soluble ionic compound, and because of that it would be soluble in polar water. Pentene on the other hand is a hydrocarbon. It possesses only carbons and hydrogens, so it is non polar. Which would mean that it is not very soluble in polar water. So this is not true for both. Both are insoluble in water. Well, we just said that potassium bromide is soluble in water since it's a soluble ionic solid. So as a result, none of the above are true. So here the final answer would be option e.

14. Solutions

Intro to Henry's Law

General Chemistry

14. Solutions

Intro to Henry's Law

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Multiple Choice

Which of the following is true for the solubility of KBr (s) and CH₃(CH₂)₃CH₃ (g) in water?

Decreasing the temperature will decrease the solubility of CH₃(CH₂)₃CH₃.

Increasing the pressure will decrease the solubility of KBr.

Both KBr and CH₃(CH₂)₃CH₃ are completely soluble in water.

Both are insoluble in water.

None of the above.

Verified step by step guidance

Understand the solubility principles for ionic compounds and gases in water. KBr is an ionic compound, and its solubility is generally not affected by pressure but can be affected by temperature. CH3(CH2)3CH3 is a nonpolar gas, and its solubility in water is affected by both temperature and pressure.

Consider the effect of temperature on the solubility of gases. For most gases, solubility decreases with an increase in temperature. Therefore, decreasing the temperature would typically increase the solubility of a gas like CH3(CH2)3CH3 in water, not decrease it.

Consider the effect of pressure on the solubility of gases. According to Henry's Law, the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid. Therefore, increasing the pressure would increase the solubility of CH3(CH2)3CH3, not decrease it.

Evaluate the solubility of KBr in water. KBr is an ionic compound and is generally soluble in water due to the polar nature of water molecules, which can stabilize the ions in solution. Pressure changes have little effect on the solubility of solids like KBr.

Assess the statement that both KBr and CH3(CH2)3CH3 are completely soluble in water. While KBr is soluble, CH3(CH2)3CH3 is a nonpolar hydrocarbon and is not soluble in water, which is polar. Therefore, the statement is incorrect, and the correct answer is 'None of the above.'

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Which of the following is true for the solubility of KBr (s) and CH3(CH2)3CH3 (g) in water?

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Which of the following is true for the solubility of KBr (s) and CH₃(CH₂)₃CH₃ (g) in water?