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Interpretation:
The given solvent capable of dissolving ionic compounds is to be identified.
Concept Introduction:
▸ A general rule of solubility is: like dissolves like.
▸ Polar and ionic solids are dissolved in polar solvents.
▸ Nonpolar solids are dissolved in nonpolar solvents.
▸ If a molecule has dipole moment, it is termed as polar molecule. The symmetrical molecules are non-polar because the dipole moment cancel each other.
▸ The species resistant to water or the species that are incompatible with water are termed as hydrophobic.
▸ The water loving species or the species compatible with water are termed as hydrophilic species.
▸ If the compound contains one hydrophilic group and more than six carbon atoms, then the compound is insoluble in water.
▸ Alkyl chains with high molecular weight are hydrophobic in nature.
▸ The hydroxyl group is hydrophilic in nature because it forms hydrogen bonding with water molecules.
▸ The carbonyl oxygen and hydroxyl group of
▸ A hydrogen bond is a partially electrostatic force of attraction between a hydrogen atom which is bound to more electronegative atom such as nitrogen, oxygen or fluorine and another atom bearing a lone pair of electron.
▸ The liquid
▸ The liquid
▸ In benzene, the bonds are polar due to the presence of electronegativity difference between carbon and hydrogen but the dipole moment cancel out due to the symmetrical structure of benzene. The net dipole moment is zero which makes the molecule non-polar.
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Chapter 2 Solutions
Organic Chemistry, 12e Study Guide/Student Solutions Manual
- (a) What is the molarity of a solution made by dissolving 10 moles of sucrose, C12H22O11, in 10L of water? (b) How much boric acid (H3BO3), in grams, is needed to be dissolves in 300.g of water to make a 1.50m aqueous H3BO3 solution? The molar mass of H3BO3 is 61.83g/mol. (c) How much aluminum sulfate (Al2(SO4)3) in moles, is needed to be dissolved in 500g of water to make a 1.0m aqueous Al2(SO4)3 solution?arrow_forwardChoose which waste disposal container you should dispose of the unused 0.1 M FeClz solution. (A) organic waste B acid waste inorganic waste (D) alkali wastearrow_forward4.(a) Aqueous 50.5 % (w/w) sodium hydroxide has a density of 1.53 g cm–3. Calculate the concentration of this solution in mol dm–3. (b) What volume of 50.5 % (w/w) aqueous sodium hydroxide is required to prepare 500 cm3 of 0.100 mol dm–3 stock NaOH? [Start with your answer to 4(a)]arrow_forward
- 11.8. (a) Explain why the concentration of dissolved oxygen in fresh water is an important indicator of the quality of the water. (b) How is the solubility of oxygen in water affected by increasing temperature?arrow_forwardThe Henry’s law constant at 25°C for nitrogen dissolved inwater is 8.57 × 104 atm, that for oxygen is 4.34 × 104 atm,and that for helium is 1.7 × 105 atm.(a) Calculate the number of moles of nitrogen and oxy-gen dissolved per liter of water in equilibrium with air at 25°C.(b) Air is dissolved in blood and other bodily luids. As adeep-sea diver descends, the pressure increases and the concentration of dissolved air in the blood increases. If the diver returns to the surface too quickly, gas bubbles out of solution within the body so rapidly that it can cause a dangerous condition called “the bends.” Use Henry’s law to show why divers some- times use a combination of helium and oxygen in their breathing tanks in place of compressed air.arrow_forward(a) Solubility of CO2 at 20 C and 1 atm is equivalent to 87.8 mL/ 100 mL water.Suppose the partial pressure of CO2 before opening a can of coke was 2.5 atm, calculate the molarity of CO2 in a coke saturated with CO2 at 20 C.(b) The 250-mL coke was then opened. Given the atmospheric pressure is 1 atm and volume percent of CO2 in air is 0.036%, what is the solubility of CO2 in the coke at 20 C after exposed to air? And what volume of CO2, measured at 20 C and 1 atm, has expelled after the coke has opened for a prolonged time?arrow_forward
- What is the concentration of potassium nitrate (in molarity) at saturation if the mass solubility at 50 oC is 88 g KNO3 per 100 g water?arrow_forwardWhich of these compounds is most soluble in water and why? (A) CH4; it forms hydrogen bonding with water molecules. (B) NH3; it forms hydrogen bonding with water molecules. (C) PH3: it forms hydrogen bonding with water molecules. (D) All of them; they form hydrogen bonds with water molecules.arrow_forwardWhat is the osmotic pressure of a 300 mL aqueous solution containing 4 g of Ca(NO3)2 at 25 °C?arrow_forward
- Phosphorus pentachloride reacts violently with water togive a mixture of phosphoric acid and hydrochloric acid.(a) Write a balanced chemical equation for this reaction.(b) Determine the concentration (in moles per liter) of each of the acids that result from the complete reaction of 1.22 L of phosphorus pentachloride (measured at 215°C and 0.962 atm pressure) with enough water to give a solution volume of 697 mL.arrow_forward(b) How do the structures of these molecules account for these differences in solubility? Provide a full account of the structures and their influence on intermolecular forces that might account for the differences in this physical property. ( Name Solubility 20 1-butanol 73 g/L butanal 7.6 g/100 mL butanone 27.5 g/100 mL 1-chlorobutane 0.5 g/Larrow_forwardTo obtain a precipitate which is useful for gravimetric analysis, the analyst tries to obtain conditions to encourage crystal growth, as opposed to the formation of a colloid. Which of the following statements aids in the formation of a crystalline precipitate and the formation of a colloidal precipitate? Drag your answers to the appropriate markers. (a) The solutions are made as dilute as practical to allow crystals to form slowly. (b) The addition of strong electrolytes (e.g. NaCl or HCl) in the analyte solution, prior to the precipitation reaction. (c) After the digestion of the precipitate, the hot solution is cooled down to room temperature gradually and kept undisturbed overnight. (d) The analyst selects the precipitate of the analyte with the Ksp less than 1 x 10 -15 (e) The Relative Supersaturation value of the analyte solution should be greater than 1 million upon the addition of the precipitating reagent. formation of colloidal precipitate favored formation of crystalline…arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
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