Why are methanol and ethanol completely soluble in water while octanol is not very little soluble....
Why are methanol and ethanol completely soluble in water while octanol is not very little soluble. Show the structures.
Homework Answers
methanol is CH3OH which has a small hydrophobic group CH3 and a polar group OH.
ethanol is C2H5OH which has a small hydrophobic group C2H5 abd polar grup Oh.
Thus in these two cases , the attraction of polar OH group with water is stronger than the repulsions of non-polar alkyl groups.
However in octanol C8H17OH , the hydrophobic group is quite larger than the polar OH group, such that it repels water more strongly than the attractions of OH with water.
Methanol CH3OH
Ethanol CH3CH2OH
OCtanol CH3CH2CH2CH2CH2CH2CH2CH2OH
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Why are methanol and ethanol completely soluble in water while
octanol is not very little soluble....
Student ID/No. 2. Alcohols and Phenols (11 points) 04/1618 A. Why are some alcohols (methanol, ethanol)...
Student ID/No. 2. Alcohols and Phenols (11 points) 04/1618 A. Why are some alcohols (methanol, ethanol) soluble in water, but others (cyclohexanol. octanol etc.) are not? (3 points) B. Classify the alcohols below as primary, secondary, or tertiary (1 point each -3 points) Alcohol Classification (1°.2°.3) CH3 CH2 ?? CH2 H3C ?? ??? CH CH2 ??
2. While caffeine is very soluble in water, aspirin is only minimally soluble. a. Clearly explain...
2. While caffeine is very soluble in water, aspirin is only minimally soluble. a. Clearly explain why you think caffeine is soluble in water. b. In order to dissolve the aspirin, I had to use a sodium hydroxide solution (this is why you had to add HCl to the separatory funnel.) Clearly explain how the use of a sodium hydroxide solution allowed the aspirin to dissolve. Structures/reaction(s) will likely help your answer.
Is NaBr more soluble in ethanol or propanol? Why is dimethyl acetamide soluble in water?
Is NaBr more soluble in ethanol or propanol? Why is dimethyl acetamide soluble in water?
4. Now draw Lewis structures of a single ethanol molecule completely surrounded by water molecules. Be...
4. Now draw Lewis structures of a single ethanol molecule completely surrounded by water molecules. Be sure to show hydrogen bonding (where possible) between ethanol and nearby water molecules, plus hydrogen bonding between water molecules themselves.
Question 8 (1 point) Select all that would apply for 1-octanol OH Soluble in water Soluble...
Question 8 (1 point) Select all that would apply for 1-octanol OH Soluble in water Soluble in alkaline water (aq. NaOH) Positive acidic chromate test (color turns from orange to green) Positive Tollens' test (mirror formation) pH <6 pH 7 pH >8
Question 8 (1 point) Select all that would apply for 1-octanol OH Soluble in water Soluble...
Question 8 (1 point) Select all that would apply for 1-octanol OH Soluble in water Soluble in alkaline water (aq. NaOH) Positive acidic chromate test (color turns from orange to green) Positive Tollens' test (mirror formation) OpH<6 Орн 7 pH>8
Suggest an explanation for the observations that ethanol, C2H5OH, is completely miscible with water and that ethanethiol...
Suggest an explanation for the observations that ethanol, C2H5OH, is completely miscible with water and that ethanethiol, C2H5SH, is soluble only to the extent of 1.5 g per 100 mL of water.
Is p-methoxybenzoic acid soluble in methanol? why or why not?
Is p-methoxybenzoic acid soluble in methanol? why or why not?
Based on the molecular polarity of water, which of the following molecules would be soluble in...
Based on the molecular polarity of water, which of the following molecules would be soluble in water? glucose, methanol, and ethanol glucose, ethane, and ethanol carbon dioxide, methane, and methanol O carbon dioxide, glucose, and methanol glucose, carbon dioxide, and ethanol
6. Methanoic acid (formic acid) is infinitely soluble in water, while decanoic acid (capric acid) is...
6. Methanoic acid (formic acid) is infinitely soluble in water, while decanoic acid (capric acid) is almost completely insoluble. Based on a comparison of structures, explain the large difference in water solubility. (2 marks)
Student ID/No. 2. Alcohols and Phenols (11 points) 04/1618 A. Why are some alcohols (methanol, ethanol) soluble in water, but others (cyclohexanol. octanol etc.) are not? (3 points) B. Classify the alcohols below as primary, secondary, or tertiary (1 point each -3 points) Alcohol Classification (1°.2°.3) CH3 CH2 ?? CH2 H3C ?? ??? CH CH2 ??
2. While caffeine is very soluble in water, aspirin is only minimally soluble. a. Clearly explain why you think caffeine is soluble in water. b. In order to dissolve the aspirin, I had to use a sodium hydroxide solution (this is why you had to add HCl to the separatory funnel.) Clearly explain how the use of a sodium hydroxide solution allowed the aspirin to dissolve. Structures/reaction(s) will likely help your answer.
4. Now draw Lewis structures of a single ethanol molecule completely surrounded by water molecules. Be sure to show hydrogen bonding (where possible) between ethanol and nearby water molecules, plus hydrogen bonding between water molecules themselves.
Question 8 (1 point) Select all that would apply for 1-octanol OH Soluble in water Soluble in alkaline water (aq. NaOH) Positive acidic chromate test (color turns from orange to green) Positive Tollens' test (mirror formation) pH <6 pH 7 pH >8
Question 8 (1 point) Select all that would apply for 1-octanol OH Soluble in water Soluble in alkaline water (aq. NaOH) Positive acidic chromate test (color turns from orange to green) Positive Tollens' test (mirror formation) OpH<6 Орн 7 pH>8
Based on the molecular polarity of water, which of the following molecules would be soluble in water? glucose, methanol, and ethanol glucose, ethane, and ethanol carbon dioxide, methane, and methanol O carbon dioxide, glucose, and methanol glucose, carbon dioxide, and ethanol
6. Methanoic acid (formic acid) is infinitely soluble in water, while decanoic acid (capric acid) is almost completely insoluble. Based on a comparison of structures, explain the large difference in water solubility. (2 marks)
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