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Chapter 11: Q11.3-20E (page 647)

Which of the following gases is expected to be most soluble in water? Explain your reasoning.

(a) \({\bf{CH}}_4\)

(b) \({\bf{CCl}}_4\)

(c)\({\bf{CHCl}}_3\)

Short Answer

Expert verified

\({\rm{CHCl_3}}\) is expected to be most soluble in water. In this, the only polar molecule which dissolves in a polar solvent like water is \({\rm{CHCl_3}}\).

Step by step solution

01

Solubility

Solubility is the amount of a solute that can dissolve into solvent and form a solution that could or could not conduct electricity.

As we all know, 鈥渓ike dissolves like鈥�. According to this statement, the polar substances dissolve with polar and non-polar substances dissolve with non-polar.

02

(a) Explanation on polarity for \({\bf{CH_4}}\)

\({\rm{CH_4}}\) (methane) is an organic compound, which is less polar than \({\rm{CHCl_3}}\) as their dipole moment is zero.

03

(b) Explanation on polarity for \({\bf{CCl_4}}\)

Carbon tetrachloride is non-polar in nature. That鈥檚 why it will have less solubility in water as compared to \({\rm{CHCl_3}}\).

04

(c) Explanation on polarity for \({\bf{CHCl_3}}\)

\({\rm{CHCl_3}}\) is expected to be most soluble in water because of the formation of dipole-dipole interaction as both \({\rm{CHCl_3}}\) and water are polar in nature. Of the three gases, only \({\rm{CHCl_3}}\)is polar.

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Most popular questions from this chapter

The Henry鈥檚 law constant for \({\bf{O}}_2\)is \({\bf{1}}{\bf{.3 \times 1}}{{\bf{0}}^{{\bf{ - 3}}}}{\bf{ M at}}{{\bf{m}}^{{\bf{ - 1}}}}\)at 25 掳C. What mass of oxygen would be dissolved in a 40 L aquarium at 25 掳C, assuming an atmospheric pressure of 1.00 atm, and that the partial pressure of \({\bf{O}}_2\)is 0.21 atm?

Calculate the mole fraction of each solute and solvent:

  1. 583 g of\({{\bf{H}}_2}{\bf{S}}{{\bf{O}}_4}\)in 1.50 kg of water鈥攖he acid solution used in an automobile battery
  2. 0.86 g of NaCl in 1.00 脳 102 g of water鈥攁 solution of sodium chloride for intravenous injection
  3. 46.85 g of codeine, \({{\bf{C}}_{{\bf{18}}}}{{\bf{H}}_{{\bf{21}}}}{\bf{N}}{{\bf{O}}_{\bf{3}}}\), in 125.5 g of ethanol, \({{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{5}}}{\bf{OH}}\)
  4. 25 g of I2 in 125 g of ethanol, \({{\bf{C}}_{\bf{2}}}{{\bf{H}}_{\bf{5}}}{\bf{OH}}\).

Compare the processes that occur when methanol (\({\bf{CH}}_3{\bf{OH}}\)), hydrogen chloride (\({\bf{HCl}}\)), and sodium hydroxide (\({\bf{NaOH}}\)) dissolve in water. Write equations and prepare sketches showing the form in which each of these compounds is present in its respective solution.

Heat is released when some solutions form; heat is absorbed when other solutions form. Provide a molecular explanation for the difference between these two types of spontaneous processes.

An organic compound has a mass composition of 93.46% C and 6.54% H. A solution of 0.090 g of this compound in 1.10 g of camphor melts at 158.4 掳C. The melting point of pure camphor is 178.4 掳C.\({\bf{Kf}}\)for camphor is 37.7 掳C/m. What is the molecular formula of the solute? Show your calculations.
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