Guided course 01:03Solutions: Solubility and Intermolecular Forces Concept 1Jules Bruno3273views79rank
Guided course 01:44Solutions: Solubility and Intermolecular Forces Example 1Jules Bruno2570views49rank2comments
Guided course 02:42Solutions: Solubility and Intermolecular Forces Concept 2Jules Bruno2461views45rank1comments
Guided course 01:52Solutions: Solubility and Intermolecular Forces Example 2Jules Bruno2079views35rank
11:26Ion Dipole Forces & Ion Induced Dipole Interactions - ChemistryThe Organic Chemistry Tutor776views
03:58When do two substances form a solution (part 1) | Solutions | Chemistry | Don't MemoriseDon't Memorise285views
05:17How does a Solute Dissolve in a Solvent? | Solutions | Chemistry | Don't MemoriseDon't Memorise727views
Multiple ChoiceIndicate the most important type of intermolecular attraction responsible for solvation in the following solution:Methanol, CH3OH, dissolved in ethanol, CH3CH2OH1553views11rank
Multiple ChoiceWhich of the following solutes will most readily dissolve in H2O?1752views18rank2comments
Multiple ChoiceTwo pure chemical substance are likely to mix and form a solution if:1109views5rank1comments
Multiple ChoiceWhich of the following statements is/are true?I. The hydrocarbon methane (CH4) will dissolve completely in acetone (CH3COCH3).II. Ammonia (NH3) will form a heterogeneous mixture with carbon tetrachloride (CCl4).III. Pentane (C5H12) will form a homogeneous mixture with carbon tetrabromide (CBr4).IV. Methanethiol (CH3SH) is miscible in fluoromethane (CH3F).1194views16rank1comments
Multiple ChoiceAccording to Hess's law which of the following terms for the formation of a solution is always exothermic?228views
Multiple ChoiceConsider a solution that is saturated with a gas and a solid at room temperature. Which of the following will occur when the solution is heated by 50°C?237views
Textbook QuestionWhen lithium chloride dissolves in water, the temperature of the solution increases. Which diagram represents the enthalpy changes of the steps in the solution-making process? (LO 13.2)1496views
Textbook QuestionThis figure shows the interaction of a cation with surrounding water molecules. (b) Which of the following explanations accounts for the fact that the ion–solvent interaction is greater for Li+ than for K+? a. Li+ is of lower mass than K+. b. The ionization energy of Li is higher than that for K. c. Li+ has a smaller ionic radius than K+. d. Li has a lower density than K. e. Li reacts with water more slowly than K. [Section 13.1]456views
Textbook QuestionIn which solvent does sodium acetate 1CH COONa2 have the highest solubility (a) Acetone CH3OCH3 (b) Methanol (CH3OH) (c) Ethanol (CH3CH2OH) (d) Pentane (CH3CH2CH2CH2CH3)921views
Textbook QuestionConsider two ionic solids, both composed of singly charged ions, that have different lattice energies. (b) If not, which solid will be more soluble in water, the one with the larger lattice energy or the one with the smaller lattice energy? Assume that solute–solvent interactions are the same for both solids. [Section 13.1]565views
Textbook QuestionWhich diagram best represents a liquid–liquid emulsion such as milk? The colored balls represent different liquid molecules. [Section 13.6] 996views
Textbook QuestionIndicate the type of solute–solvent interaction (Section 11.2) that should be most important in each of the following solutions: (d) HCl in acetonitrile 1CH3CN2757views
Textbook QuestionIndicate the type of solute–solvent interaction (Section 11.2) that should be most important in each of the following solutions: (c) KBr in water548views
Textbook QuestionIndicate the type of solute–solvent interaction (Section 11.2) that should be most important in each of the following solutions: (b) methanol 1CH3OH2 in water965views
Textbook QuestionIndicate the type of solute–solvent interaction (Section 11.2) that should be most important in each of the following solutions: (a) CCl4 in benzene882views
Textbook QuestionIndicate the principal type of solute–solvent interaction in each of the following solutions and rank the solutions from weakest to strongest solute–solvent interaction: (c) methanol 1CH3OH2 in water549views
Textbook QuestionIndicate the principal type of solute–solvent interaction in each of the following solutions and rank the solutions from weakest to strongest solute–solvent interaction: (b) CH2Cl2 in benzene 1C6H62588views
Textbook QuestionIndicate the principal type of solute–solvent interaction in each of the following solutions and rank the solutions from weakest to strongest solute–solvent interaction: (a) KCl in water1508views
Textbook QuestionAn ionic compound has a very negative ∆Hsoln in water (b) Which term would you expect to be the largest negative number: ∆Hsolvent, ∆Hsolute, or ∆Hmix675views
Textbook QuestionWhen ammonium chloride dissolves in water, the solution becomes colder. (b) Why does the solution form?1587views
Textbook QuestionWhen ammonium chloride dissolves in water, the solution becomes colder. (a) Is the solution process exothermic or endothermic?1259views
Textbook QuestionTwo nonpolar organic liquids, hexane 1C6H142 and heptane 1C7H162, are mixed. (b) Hexane and heptane are miscible with each other in all proportions. In making a solution of them, is the entropy of the system increased, decreased, or close to zero, compared to the separate pure liquids?438views
Textbook QuestionTwo nonpolar organic liquids, hexane 1C6H142 and heptane 1C7H162, are mixed (b) Hexane and heptane are miscible with each other in all proportions. In making a solution of them, is the entropy of the system increased, decreased, or close to zero, compared to the separate pure liquids?620views
Textbook QuestionTwo nonpolar organic liquids, hexane 1C6H142 and heptane 1C7H162, are mixed. (a) Do you expect ∆Hsoln to be a large positive number, a large negative number, or close to zero? Explain.1159views
Textbook QuestionKBr is relatively soluble in water, yet its enthalpy of solution is + 19.8 kJ/mol. Which of the following statements provides the best explanation for this behavior? (a) Potassium salts are always soluble in water. (b) The entropy of mixing must be unfavorable. (c) The enthalpy of mixing must be small compared to the enthalpies for breaking up water–water interactions and K–Br ionic interactions. (d) KBr has a high molar mass compared to other salts like NaCl.2712views1rank
Textbook QuestionOil and water are immiscible. Which is the most likely reason? (a) Oil molecules are denser than water. (b) Oil molecules are composed mostly of carbon and hydrogen. (c) Oil molecules have higher molar masses than water. (d) Oil molecules have higher vapor pressures than water. (e) Oil molecules have higher boiling points than water.1605views
Textbook QuestionPick an appropriate solvent from Table 13.3 to dissolve each substance. State the kind of intermolecular forces that would occur between the solute and solvent in each case. b. sodium chloride (ionic)865views
Textbook QuestionWhich molecule would you expect to be more soluble in water: CH3CH2CH2OH or HOCH2CH2CH2OH?3970views
Textbook QuestionWhich of the following in each pair is likely to be more soluble in hexane, C6H14:(b) benzene 1C6H62 or glycerol, CH21OH2CH1OH2CH2OH,2189views
Textbook QuestionFor each compound, would you expect greater solubility in water or in hexane? Indicate the kinds of intermolecular forces that occur between the solute and the solvent in which the molecule is most soluble. a. glucose598views
Textbook QuestionWhich of the following in each pair is likely to be more soluble in water: (c) HCl or ethyl chloride 1CH3CH2Cl2? Explain in each case.501views
Textbook QuestionWhich of the following in each pair is likely to be more soluble in water: (a) cyclohexane 1C6H122 or glucose 1C6H12O62,1027views
Textbook QuestionFor each compound, would you expect greater solubility in water or in hexane? Indicate the kinds of intermolecular forces that would occur between the solute and the solvent in which the molecule is most soluble. d. ethylene glycol711views
Textbook QuestionIf a single 5-g block of NaCl is placed in water, it dissolves slowly, but if 5 g of powdered NaCl is placed in water, it dis- solves rapidly. Explain.400views
Textbook QuestionWhen lithium iodide (LiI) is dissolved in water, the solution becomes hotter. d. Why does the solution form? What drives the process?460views
Textbook QuestionWhen lithium iodide (LiI) is dissolved in water, the solution becomes hotter. c. Sketch a qualitative energy diagram similar to Figure 13.7 for the dissolution of LiI.966views
Textbook QuestionIndicate whether each statement is true or false: (c) The solubility of most gases in water decreases as the temperature increases because water is breaking its hydrogen bonding to the gas molecules as the temperature is raised.1028views
Textbook QuestionWhen lithium iodide (LiI) is dissolved in water, the solution becomes hotter. b. What can you conclude about the relative magnitudes of the lattice energy of lithium iodide and its heat of hydration?1502views
Textbook QuestionWhen lithium iodide (LiI) is dissolved in water, the solution becomes hotter. a. Is the dissolution of lithium iodide endothermic or exothermic?888views
Textbook QuestionWhich would you expect to have the larger hydration energy, SO42- or ClO4-? Explain.501views
Textbook QuestionClassify the strongest type of intermolecular force in the follow- ing interactions: solvent–solvent, solvent–solute, and solute– solute when solid iodine 1I22 is placed in the water. Based on these interactions, predict whether I2 is soluble in water.879views1rank
Textbook QuestionDetermine whether each pair of compounds forms a homogeneous solution when combined. For those that form homogeneous solutions, indicate the type of forces that are involved. d. CH3CH2OH and H2O1906views
Textbook QuestionDetermine whether each pair of compounds forms a homogeneous solution when combined. For those that form homogeneous solutions, indicate the type of forces that are involved. a. CCl4 and H2O1626views
Textbook QuestionPredict whether the solubility of butane, C4H10, is greater in water or benzene, C6H6.938views
Textbook QuestionArrange the following compounds in order of their expected increasing solubility in water: Br2, KBr, toluene (C7H8, a constituent of gasoline).843views
Textbook QuestionLook at the solubility graph in Figure 13.7, and estimate which member of each of the following pairs has the higher molar solubility at the given temperature. (b) CH3CO2Na or glucose at 20 °C1140views
Textbook QuestionWater is a good solvent for many substances. What is the molecular basis for this property, and why is it significant?649views
Textbook QuestionAerosols are important components of the atmosphere. Does the presence of aerosols in the atmosphere increase or decrease the amount of sunlight that arrives at the Earth's surface, compared to an 'aerosol-free' atmosphere? Explain your reasoning.506views
Textbook QuestionWater does not easily remove grease from dishes or hands because grease is nonpolar and water is polar. The addition of soap to water, however, allows the grease to dissolve. Study the structure of sodium stearate (a soap) and describe how it works. 1243views
Textbook QuestionThe 'free-base' form of cocaine (C17H21NO4) and its protonated hydrochloride form (C17H22ClNO4) are shown below; the free-base form can be converted to the hydrochloride form with one equivalent of HCl. For clarity, not all the carbon and hydrogen atoms are shown; each vertex represents a carbon atom with the appropriate number of hydrogen atoms so that each carbon makes four bonds to other atoms (a) One of these forms of cocaine is relatively water-soluble: which form, the free base or the hydrochloride?1403views
Textbook QuestionA supersaturated solution of sucrose (C12H22O11) is made by dissolving sucrose in hot water and slowly letting the solution cool to room temperature. After a long time, the excess sucrose crystallizes out of the solution. Indicate whether each of the following statements is true or false: (b) After the excess sucrose has crystallized out, the system is now unstable and is not in equilibrium.1355views
Textbook QuestionThe solubility of carbon tetrachloride (CCl4) in water at 25 °C is 1.2 g>L. The solubility of chloroform (CHCl3) at the same temperature is 10.1 g>L. Why is chloroform almost ten times more soluble in water than carbon tetrachloride?2770views1rank
Textbook QuestionA series of anions is shown below: The anion on the far right is called 'BARF' by chemists, as its common abbreviation sounds similar to this word. (d) Tetrabutylammonium, (CH3CH2CH2CH2)4N + is a bulky cation. Which anion, when paired with the tetrabutylammonium cation, would lead to a salt that will be most soluble in nonpolar solvents?585views
Textbook QuestionCompounds like sodium stearate, called 'surfactants' in general, can form structures known as micelles in water, once the solution concentration reaches the value known as the critical micelle concentration (cmc). Micelles contain dozens to hundreds of molecules. The cmc depends on the substance, the solvent, and the temperature. (a) The turbidity (the amount of light scattering) of solutions increases dramatically at the cmc. Suggest an explanation. .709views
Open QuestionWhich lists mixtures, in order, from the smallest particles to the largest particles?199views
Open QuestionWhich interactions and processes contribute to the dissolution of ionic compounds in water?176views
Open QuestionWhich statement accurately describes part of the dissolving process of a polar solute in water?166views
Open QuestionChoose the pair of substances that are most likely to form a homogeneous solution.448views
Open QuestionFor each of the following molecules, would you expect greater solubility in water or in hexane?272views
Open QuestionWhich statement explains why sugar dissolves easily in water, but sand does not?251views
Open Questionbased only on intermolecular forces, which of the following would be the least soluble in CH3CH2OH?186views
Open QuestionA substance, usually liquid, that dissolves another substance to form a solution is a(n) _____.179views
Open QuestionWhich bond or interaction would be difficult to disrupt when compounds are put into water?156views
Open QuestionBased only on intermolecular forces, which of the following would be the most soluble in CH3OH?156views
Open QuestionWhich of the following is most directly responsible for water's unique properties?158views
Open QuestionBased only on intermolecular forces, which of the following would be the least soluble in CH3OH?165views
Open QuestionWhen sodium chloride dissolves in water, the sodium and chloride ions are pulled into solution by:139views
Open QuestionWhy can salt and sugar both dissolve in water, even though one is ionic and the other is covalent?244views