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Would you expect cyclohexane, C6H12, to be miscible with water? Explain why or why not
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- Can a covalent compound like ethanol, CH3OH dissolve in water? Explain Edit View InsertUse molecular structures and noncovalent interactions to explain why dimethyl ether, (CH3)2O, is completely miscible in water, but dimethylsulfide, (CH3)2S, is only slightly water soluble.Which would you expect to be more soluble in water, cyclohexane or dioxane?
- Part A Which of the following likely to be more soluble in hexane, C6H14? Explain your answer in each case. Match the items in the left column to the appropriate blanks in the sentences on the right. hydrogen bonding dispersion forces acetic acid ionic bonds octanoic acid benzene glycerol CaCl₂ CC14 is more soluble, because Among CCl4 and CaCl2, are less likely to be overcome by solute-solvent interactions. Among benzene (C6H6) and glycerol (CH₂(OH) CH(OH)CH₂ OH), soluble, because interaction. in in Among octanoic acid (CH3 (CH₂)6 COOH) and acetic acid (CH3 COOH), more soluble, because it has similar to those in hexane. Reset is more is less likely to be overcome by solute-solvent will be HelpSolubility- hexachlorobenzene Q1)Using the Lewis structures of the molecule and water, identify and label areas of intermolecular attraction. ▪More than one water molecule should be shown ▪Label the type of IM forces present b)Using the Lewis structures of the molecule and a nonpolar solvent (e.g., hexane), identify and label areas of intermolecular attraction. c)explain the solubility (or lack thereof) of your molecule in water. When available, use solubility data (at the same temperature) to support your explanation. d)explain the solubility (or lack thereof) of your molecule in nonpolar solvents. When available, use solubility data (at the same temperature) to support your explanation. e)when dissolved in water, qualitatively discuss whether the molecule is a strong electrolyte, weak electrolyte, or nonelectrolyte. Please answer very soon will give rating surely All questions answers neededYou come across a bottle in the stock room labeled CHCl3 Do you expect this molecule to interact more with water (H2O) or methane (CH4)?Explain why.
- 26) Based off molecular polarity determined by VSEPR theory, which of the following would be insoluble in CCI4 ? A) octane CH,CH,CH,CH,CH,CH,CH,CH3 B) methanol CH;OH C) hexane CH;CH;CH;CH;CH;CH3 27) Which of the following naming is incorrect? iron(III) sulfate B) Fe2(SO3)3 iron(III) sulfite C) Feg(SO4)3 iron(III) sulfate iron (II) sulfide iron(II) sulfite A) FESO, D) Fes E) FeSO,Arrange the following acids in the increasing order of their solubility in water: p-ClC6H4COOH, CH3COOH, CH3(CH2)3COOHWater’s highly polar character is responsible for its exceptional ability to dissolve a wide range of ionic and polar-covalent substances?
- Chemistry 1. Glycerol, CH2(OH)CH(OH)CH2OH, has a 3 carbon chain with -OH groups coming off of each carbon. This thick, syrup like liquid is used in anti-freeze and as a food additive. Hexaoctane, C18H38, is a greasy wax-like solid at room temperature. Using this information rank molecules in order of increasing boiling point and justify your answer: PCl2F, H2O, SeS3, MgS, Glycerol, CH4, CaS, PF2Cl, Hexaoctane, NeAcetone [(CH3)2CO] is widely used as an industrial solvent.(a) Draw the Lewis structure for the acetone molecule andpredict the geometry around each carbon atom. (b) Is theacetone molecule polar or nonpolar? (c) What kinds ofintermolecular attractive forces exist between acetone molecules?(d) 1-Propanol (CH3CH2CH2OH) has a molecularweight that is very similar to that of acetone, yet acetoneboils at 56.5 °C and 1-propanol boils at 97.2 °C. Explain thedifference.Aspirin has a higher molar mass compared to salicylic acid, however aspirin melts at a lower temperature than salicylic acid. Provide a brief explanation for this observation. Table 1 Compound: Formula: Salicylic Acid C;H6O3 Aspirin C9H3O4 Molar Mass: 138.12 Melting point: Ka 158-160°C 1.08 x 10³ 180.15 140-142°C 2.72 x 10$ pKa Solubility (g/100ML) 2.99 4.57 0.18 0.25