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In Morrison & Boyd, I found this question:

Butan-1-ol (b.p. $118~\mathrm{^\circ C}$) has a much higher boiling point than its isomer diethyl ether (b.p. $35~\mathrm{^\circ C}$), yet both compounds show the same solubility ($8~\mathrm{g}$ per $100~\mathrm{g}$) in water.

 

Molecules

 

How do you account for these facts?

Now, as far as I know, the boiling point depends on the inter molecular forces. Since in the alcohol, there is hydrogen bonding in the O-H group, it has a higher boiling point than the ether. But in an aqueous solution, the solubility is also related to hydrogen bonding. Since there is more hydrogen bonding in the alcohol, I would expect it to have a higher solubility in water, but that is not the case. So how do we explain it? I am completely confused by this question. What is the answer?

In Morrison & Boyd, I found this question:

Butan-1-ol (b.p. $118~\mathrm{^\circ C}$) has a much higher boiling point than its isomer diethyl ether (b.p. $35~\mathrm{^\circ C}$), yet both compounds show the same solubility ($8~\mathrm{g}$ per $100~\mathrm{g}$) in water.

 

Molecules

 

How do you account for these facts?

Now, as far as I know, the boiling point depends on the inter molecular forces. Since in the alcohol, there is hydrogen bonding in the O-H group, it has a higher boiling point than the ether. But in an aqueous solution, the solubility is also related to hydrogen bonding. Since there is more hydrogen bonding in the alcohol, I would expect it to have a higher solubility in water, but that is not the case. So how do we explain it? I am completely confused by this question. What is the answer?

In Morrison & Boyd, I found this question:

Butan-1-ol (b.p. $118~\mathrm{^\circ C}$) has a much higher boiling point than its isomer diethyl ether (b.p. $35~\mathrm{^\circ C}$), yet both compounds show the same solubility ($8~\mathrm{g}$ per $100~\mathrm{g}$) in water.

Molecules

How do you account for these facts?

Now, as far as I know, the boiling point depends on the inter molecular forces. Since in the alcohol, there is hydrogen bonding in the O-H group, it has a higher boiling point than the ether. But in an aqueous solution, the solubility is also related to hydrogen bonding. Since there is more hydrogen bonding in the alcohol, I would expect it to have a higher solubility in water, but that is not the case. So how do we explain it? I am completely confused by this question. What is the answer?

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orthocresol
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In Morrison & Boyd, I found this question:

[![enter image description here][1]][1]

Butan-1-ol (b.p. $118~\mathrm{^\circ C}$) has a much higher boiling point than its isomer diethyl ether (b.p. $35~\mathrm{^\circ C}$), yet both compounds show the same solubility ($8~\mathrm{g}$ per $100~\mathrm{g}$) in water.

Molecules

How do you account for these facts?

Now, as far as I know, the boiling point depends on the inter molecular forces. Since in butylthe alcohol, there is hydrogen bonding in the O-H group, it has a higher boiling point than diethylthe ether. But in an aqueous solution, the solubility is also related to hydrogen bonding. Since there is more hydrogen bonding in butylthe alcohol, I would expect it to have a higher solubility in waterwater, but that is not the case. So how do we explain it? I am completely confused by this question. What is the answer? [1]: https://i.sstatic.net/FriSx.png

In Morrison & Boyd, I found this question:

[![enter image description here][1]][1]

Now, as far as I know, the boiling point depends on the inter molecular forces. Since in butyl alcohol, there is hydrogen bonding in the O-H group, it has a higher boiling point than diethyl ether. But in an aqueous solution, the solubility is also related to hydrogen bonding. Since there is more hydrogen bonding in butyl alcohol, I would expect it to have a higher solubility in water, but that is not the case. So how do we explain it? I am completely confused by this question. What is the answer? [1]: https://i.sstatic.net/FriSx.png

In Morrison & Boyd, I found this question:

Butan-1-ol (b.p. $118~\mathrm{^\circ C}$) has a much higher boiling point than its isomer diethyl ether (b.p. $35~\mathrm{^\circ C}$), yet both compounds show the same solubility ($8~\mathrm{g}$ per $100~\mathrm{g}$) in water.

Molecules

How do you account for these facts?

Now, as far as I know, the boiling point depends on the inter molecular forces. Since in the alcohol, there is hydrogen bonding in the O-H group, it has a higher boiling point than the ether. But in an aqueous solution, the solubility is also related to hydrogen bonding. Since there is more hydrogen bonding in the alcohol, I would expect it to have a higher solubility in water, but that is not the case. So how do we explain it? I am completely confused by this question. What is the answer?

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orthocresol
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n-Butyl Alcohol has much higher boiling point than Diethyl Ether yet it has Why do alcohols and ethers have approximately the same solubilty, Whysolubility in water but different boiling points?

inIn Morrison & Boyd, I found this question:

[![enter image description here][1]][1]

Now, as far as I know, the boiling point depends on the inter molecular forces. Since in Butyl Alcoholbutyl alcohol, there is hydrogen bonding in the O-H group, it has a higher boiling point than Diethyl Etherdiethyl ether. But in an aqueous solution, the solubility is also related to hydrogen bonding. Since there is more hydrogen bonding in Butylbutyl alcohol, I would expect it to have a higher solubility in water, but that is not the case. So how do we explain it? I am completely confused by this question. What is the answer? [1]: https://i.sstatic.net/FriSx.png

n-Butyl Alcohol has much higher boiling point than Diethyl Ether yet it has the same solubilty, Why?

in Morrison & Boyd, I found this question:

[![enter image description here][1]][1]

Now, as far as I know, the boiling point depends on the inter molecular forces. Since in Butyl Alcohol, there is hydrogen bonding in the O-H group, it has a higher boiling point than Diethyl Ether. But in an aqueous solution, the solubility is also related to hydrogen bonding. Since there is more hydrogen bonding in Butyl alcohol, I would expect it to have a higher solubility in water, but that is not the case. So how do we explain it? I am completely confused by this question. What is the answer? [1]: https://i.sstatic.net/FriSx.png

Why do alcohols and ethers have approximately the same solubility in water but different boiling points?

In Morrison & Boyd, I found this question:

[![enter image description here][1]][1]

Now, as far as I know, the boiling point depends on the inter molecular forces. Since in butyl alcohol, there is hydrogen bonding in the O-H group, it has a higher boiling point than diethyl ether. But in an aqueous solution, the solubility is also related to hydrogen bonding. Since there is more hydrogen bonding in butyl alcohol, I would expect it to have a higher solubility in water, but that is not the case. So how do we explain it? I am completely confused by this question. What is the answer? [1]: https://i.sstatic.net/FriSx.png

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Kartik
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