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introductory chemistry concepts
Introductory Chemistry Concepts And Critical Thinking 7th Edition Charles Corwin - Solutions
Label the polar Ge—Cl bond using delta notation (δ+ and δ–).
Label the polar As—Cl bond using delta notation (δ+ and δ–).
Write the electron dot formula and draw the structural formula for silane, SiH4 , whose central atom is a semimetal.
Write the electron dot formula and draw the structural formula for stibine, SbH3, whose central atom is a semimetal.
Write the electron dot formula and draw the structural formula for the arsenate ion, AsO3 3–, whose central atom is a semimetal.
Write the electron dot formula and draw the structural formula for the silicate ion, SiO3 2–, whose central atom is a semimetal.
Predict the electron pair geometry, the molecular shape, and the bond angle for a carbon disulfide molecule, CS2, using VSEPR theory
Predict the electron pair geometry, the molecular shape, and the bond angle for a silicon dioxide molecule, SiO2, using VSEPR theory.
Predict the electron pair geometry, the molecular shape, and the bond angle for a phosgene molecule, CCl2O, using VSEPR theory.
Predict the electron pair geometry, the molecular shape, and the bond angle for a carbonate ion, CO3 2–, using VSEPR theory.
Xenon dioxide is a slightly stable molecule that contains a noble gas. Write the electron dot formula and draw the structural formula for XeO2.
Xenon trioxide is a slightly stable molecule that contains a noble gas. Write the electron dot formula and draw the structural formula for XeO3.
Calculate the solubility of carbon dioxide in water at 0 °C and a pressure of 3.00 atm. The solubility of carbon dioxide is 0.348 g/100 mL water at 0 °C and 1.00 atm.
The elevation of Lake Havasu is 400 feet, and Lake Tahoe is 6200 feet. If the water temperatures are the same, which lake has a lower concentration of oxygen gas?
Yeast and sugar are added to champagne to give the sparkle of carbonation. Under what conditions is carbon dioxide gas most soluble?(a) Low temperature, high pressure(b) Low temperature, low pressure(c) High temperature, low pressure(d) High temperature, high pressure(e) None of the above.
Indicate whether the solubility of carbon dioxide gas in soda increases or decreases for each of the following changes.(a) The temperature of the soda decreases from 20 °C to 10 °C.(b) The partial pressure of CO2 decreases from 3 atm to 2 atm.
Oxygen is much less soluble in water than carbon dioxide, 0.00412 g/100 mL at 20 °C and 760 mm Hg. Calculate the solubility of oxygen gas in water at 20 °C and a pressure of 1150 mm Hg.
Predict whether each of the following solvents is miscible or immiscible with water:(a) Methanol, CH3OH(b) Toluene, C7H8.
The like dissolves like rule states that two liquids are miscible if what property of the two liquids is alike?
Apply the like dissolves like rule to predict which of the following liquids is miscible with water.(a) Benzene, C6H6(b) Chloroform, CHCl3(c) Methanol, CH3OH(d) All of the above(e) None of the above.
Indicate whether the solubility of carbon dioxide gas in soda increases or decreases for each of the following changes.(a) The temperature of the soda increases from 10 °C to 20 °C.(b) The partial pressure of CO2 increases from 1 atm to 2 atm.
Predict whether each of the following solvents is miscible or immiscible with water:(a) Methylene chloride, CH2Cl2(b) Glycerin, C3H5(OH)3.
The like dissolves like rule states that a solid is soluble in a liquid if what property is alike?
Predict whether each of the following solid compounds is soluble or insoluble in water.(a) Fructose, C6H12O6(b) Lithium carbonate, Li2CO3(c) Naphthalene, C10H8.
Apply the like dissolves like rule to predict which of the following is a water-soluble vitamin.(a) Vitamin A, C20H30O(b) Vitamin C, C6H8O6(c) Vitamin D, C27H44O(d) Vitamin E, C29H50O2(e) None of the above.
The solubility of nitrogen gas is 1.90 mL/dL of blood at 1.00 atm. What is the solubility of nitrogen gas in a deep-sea diver’s blood at a depth of 200 feet and a pressure of 7.00 atm?
Predict whether each of the following solid compounds is soluble or insoluble in water.(a) Anthracene, C14H10(b) Cupric sulfate, CuSO4(c) Lactic acid, HC3H5O3.
When an ionic compound dissolves in water, is the oxygen atom in a water molecule attracted to the cation or anion in the compound?
When potassium iodide, KI, dissolves in water, why does the oxygen atom of the water molecule attack the potassium ion, K+?
When glucose, C6H12O6, dissolves in water, which of the following is formed in the solution?(a) Hydrated clusters of H2O(b) Hydrated clusters of CO2(c) Hydrated clusters of H2CO3(d) Hydrated clusters of C6H12O6(e) None of the above.
The solubility of nitrogen gas is 1.90 mL/dL of blood at 1.00 atm. What is the solubility of nitrogen gas in a deep-sea diver’s blood at a depth of 125 feet and a pressure of 4.50 atm?
When potassium iodide, KI, dissolves in water, why do the hydrogen atoms of the water molecule attack the iodide ion, I–?
Why does grinding solid crystals increase the rate of dissolving of a solid solute in water?
Why does heating a solution increase the rate of dissolving of a solid solute in water?
Which of the following increases the rate of dissolving for a solid solute in a solvent? (a) Heating the solution(b) Stirring the solution(c) Grinding the solute(d) All of the above(e) None of the above.
The solubility of nitrous oxide is 0.12 g/100 g water at 20 °C and 1.00 atm. What is the partial pressure required to dissolve 0.25 g of the gas in 100 g of water at 20 °C?
Why does stirring a solution increase the rate of dissolving of a solid solute in water?
Determine the solubility of each of the following solid compounds at 50 °C as shown in Figure 13.5.(a) NaCl(b) KCl(c) LiCl(d) C12H22O11.Figure 13.5 Solubility (g/100 g H₂O) 150 100 50 C12H22O11 25 50 Temperature (°C) LiCl KCI. NaCl 75 100
Given a hot cup of coffee, and a warm cup of coffee, which can dissolve more sugar?
What is the solubility of C12H22O11 at 20 °C? (Refer to Figure 13.5)(a) 20 g/100 g water(b) 55 g/100 g water(c) 100 g/100 g water(d) 140 g/100 g water(e) 150 g/100 g water.Figure 13.5 Solubility (g/100 g H₂O) 150 100 50 C12H22O11 25 50 Temperature (°C) LiCl KCI NaCl 75 100
Refer to the solubility behavior shown in Figure 13.5 and determine the minimum temperature required to obtain the following solutions.(a) 35 g NaCl per 100 g of water(b) 45 g KCl per 100 g of water(c) 120 g LiCl per 100 g of water(d) 109 g C12H22O11 per 100 g of water. Solubility (g/100 g
The solubility of nitrous oxide is 0.12 g/100 g water at 20 °C and 1.00 atm. What is the partial pressure required to dissolve 0.55 g of the gas in 100 g of water at 20 °C?
A sodium acetate solution contains 110 g of NaC2H3O2 per 100 g of water. Refer to Figure 13.6 and determine whether the solution is unsaturated, saturated, or supersaturated at each of the following temperatures.(a) 50 °C(b) 70 °C(c) 90 °C.Figure 13.6 Solubility (g/100 g
How is it possible to exceed the saturation of a solution and produce a supersaturated solution?
How concentrated is a solution containing 130 g of NaC2H3O2 in 100 g water at 90 °C? (a) Unsaturated(b) Saturated(c) Supersaturated(d) Superunsaturated(e) None of the above.
A sodium acetate solution contains 80 g of NaC2H3O2 per 100 g water. Refer to Figure 13.6 and determine whether the solution is unsaturated, saturated, or supersaturated at each of the following temperatures.(a) 0 °C(b) 15 °C(c) 45 °C.Figure 13.6 Solubility (g/100 g
State whether the solutes and solvents in each of the following combinations are miscible or immiscible.(a) Polar solute + polar solvent(b) Polar solute + nonpolar solvent.
Intravenous dextrose injections are given to restore sugar levels in patients. What is the mass of sugar dissolved in 25.0 g of a 10.0% dextrose solution? We will solve this problem using the unit analysis method of problem solving; that is, given value unit factor unit in answer
Explain how dextrose and fructose can have the same molecular formula, C6H12O6, but different physical and chemical properties?
What mass of solute is dissolved in 5.00 kg of 40.0% antifreeze solution? (a) 1.25 kg(b) 2.00 kg(c) 7.50 kg(d) 12.5 kg(e) 200 kg.
State whether the solutes and solvents in each of the following combinations are miscible or immiscible.(a) Nonpolar solute + polar solvent(b) Nonpolar solute + nonpolar solvent.
Fructose is referred to as fruit sugar and accounts for the sweet taste of fruit. What is the mass of sugar dissolved in 10.0 g of a 5.00% fructose solution?
Given the mass percent concentration of a solution, how many unit factors can we write?
What is the volume of 3.00 M sulfuric acid that contains 9.809 g of H2SO4 solute (98.09 g/mol)? (a) 0.300 mL(b) 30.0 mL(c) 33.3 mL(d) 333 mL(e) 3330 mL.
Predict whether each of the following solvents is polar or nonpolar.(a) Water, H2O(b) Hexane, C6H14(c) Acetone, C3H6O(d) Chloroform, CHCl3.
A 7.50% potassium chloride solution is prepared by dissolving enough of the salt to give 100.0 g of solution. What is the mass of water required?
What volume of 6.00 M hydrochloric acid contains 10.0 g of HCl solute (36.46 g/mol)?
How many milliliters of 12.0 M hydrochloric acid contain 7.30 g of HCl solute (36.46 g/mol)? In molarity calculations, we relate the given value to moles and then convert to the unit asked for in the answer. given value unit factor unit factor unit in answer
Given the molar concentration of a solution, how many unit factors can we write?
What volume of 16 M nitric acid must be diluted with distilled water to prepare 500.0 mL of 0.50 M HNO3?(a) 0.016 mL(b) 0.16 mL(c) 1.6 mL(d) 16 mL(e) 160 mL.
Predict whether each of the following solvents is polar or nonpolar.(a) Isopropyl alcohol, C3H7OH(b) Pentane, C5H12(c) Xylene, C6H4(CH3)2(d) Trichloroethane, C2H3Cl3.
Battery acid is 18 M sulfuric acid. What volume of battery acid must be diluted with distilled water to prepare 1.00 L of 0.50 M H2SO4?
If equal volumes of 6 M sulfuric acid and distilled water are added together, what is the concentration of the diluted acid?
Concentrated hydrochloric acid is available commercially as a 12 M solution. What is the molarity of an HCl solution prepared by diluting 50.0 mL of concentrated acid with distilled water to give a total volume of 2.50 L?
What volume of 0.115 M hydrochloric acid reacts completely with 0.125 g of sodium carbonate, Na2CO3 (105.99 g/mol)? Na2CO3(s) + 2 HCl(aq) → Na2SO4(aq) + 2 H2O(l) + 2 CO2(g) (a) 9.75 mL(b) 10.3 mL(c) 20.5 mL(d) 41.0 mL(e) 97.5 mL.
Predict whether each of the following solvents is miscible or immiscible with hexane, C6H14.(a) Heptane, C7H16(b) Methanol, CH3OH(c) Methyl ethyl ketone, C4H8O(d) Chloroform, CHCl3.
Given that 27.5 mL of 0.210 M lithium iodide solution reacts with 0.133 M lead(II) nitrate solution, what volume of Pb(NO3)2 solution is required for complete precipitation? Pb(NO3)2(aq) + 2 LiI(aq) → PbI2(s) + 2 LiNO3(aq)
Before applying unit analysis and solving a solution stoichiometry problem, what must always be done first?
Given that 37.5 mL of 0.100 M aluminum bromide solution reacts with a silver nitrate solution, what is the mass of AgBr (187.77 g/mol) produced? The balanced equation is AlBr3(aq) + 3 AgNO3(aq) S 3 AgBr(s) + Al(NO3)3(aq)
Explain why bubbles form on the inside surface of a pan when water is heated.
Predict whether each of the following solvents is miscible or immiscible with water.(a) Toluene, C7H8(b) Ethanol, C2H5OH(c) Acetic acid, CH3COOH(d) Trichloroethylene, C2HCl3.
Explain why peanut butter can be used to remove grease from clothing.
In the laboratory, how could you quickly determine whether an unknown liquid is polar or nonpolar?
Explain why powdered sugar dissolves more rapidly in water than granulated sugar.
Oil and water separate into two layers. Explain why the two liquids are immiscible using the like dissolves like rule.
Lake Nuclear and Lake Green are adjoining at the same elevation. If water from Lake Nuclear cools a nuclear power plant and Lake Green does not, which lake has more dissolved oxygen gas?
State whether the following combinations of solute and solvent are generally soluble or insoluble.(a) Polar solute + nonpolar solvent(b) Nonpolar solute + nonpolar solvent(c) Ionic solute + nonpolar solvent.
Examine the following illustrations of NaCl and AgCl dissolving in water. At the molecular level, explain why NaCl is more soluble than AgCl.
State whether the following combinations of solute and solvent are generally soluble or insoluble.(a) Polar solute + polar solvent(b) Nonpolar solute + polar solvent(c) Ionic solute + polar solvent.
Predict whether each of the following compounds is soluble or insoluble in water.(a) Naphthalene, C10H8(b) Potassium hydroxide, KOH(c) Calcium acetate, Ca(C2H3O2)2(d) Trichlorotoluene, C7H5Cl3.
Predict whether each of the following compounds is soluble or insoluble in hexane, C6H14.(a) Trichloroethylene, C2HCl3(b) Iron(III) nitrate, Fe(NO3)3(c) Tartaric acid, H2C4H4O6(d) Dodecane, C12H26.
Predict whether each of the following compounds is water soluble or fat soluble.(a) Oleic acid, C18H34O2(b) Citric acid, C6H8O7(c) Lactic acid, CH3CH(OH)COOH(d) Stearic acid, CH3(CH2)16COOH.
Predict whether each of the following vitamins is water soluble or fat soluble.(a) Vitamin B3, C6H6N2O(b) Vitamin C, C6H8O6(c) Vitamin D, C27H44O(d) Vitamin K, C31H46O2.
Diagram a molecule of fructose, C6H12O6, dissolved in water.
Diagram a crystal of sucrose, C12H22O11, dissolving in water.
Diagram a formula unit of each of the following substances dissolved in water.(a) Lithium bromide, LiBr(b) Calcium chloride, CaCl2.
Diagram a formula unit of each of the following substances dissolved in water.(a) Cobalt(II) sulfate, CoSO4(b) Nickel(II) nitrate, Ni(NO3)2.
What three factors increase the rate of dissolving of a solid substance in solution?
Indicate whether each of the following increases, decreases, or has no effect on the rate at which 10.0 g of sugar dissolves in a liter of water.(a) Using water from the refrigerator(b) Shaking the sugar and water(c) Using powdered sugar rather than crystals(d) Using tap water rather than
How many grams of each of the following solutes can dissolve in 100 g of water at 20 °C?(a) NaCl(b) KCl.
How many grams of each of the following solutes can dissolve in 100 g of water at 30 °C? (a) LiCl(b) C12H22O11.
Determine the maximum solubility of each of the following solid compounds at 40 °C. (a) NaCl(b) KCl.
Determine the maximum solubility of each of the following solid compounds at 50 °C. (a) LiCl(b) C12H22O11.
What is the minimum temperature required to dissolve each of the following?(a) 34 g NaCl in 100 g of water(b) 50 g KCl in 100 g of water.
What is the minimum temperature required to dissolve each of the following? (a) 90 g LiCl in 100 g of water(b) 120 g C12H22O11 in 100 g of water.
At what temperature is each of the following solutions saturated? (a) 40 g NaCl/100 g water(b) 40 g KCl/100 g water.
At what temperature is each of the following solutions saturated? (a) 105 g LiCl/100 g water(b) 140 g C12H22O11/100 g water.
State whether each of the following solutions is saturated, unsaturated, or supersaturated. (a) 110 g LiCl/100 g H2O at 50 °C(b) 110 g LiCl/100 g H2O at 70 °C(c) 110 g LiCl/100 g H2O at 90 °C.
State whether each of the following solutions is saturated, unsaturated, or supersaturated.(a) 130 g C12H22O11/100 g H2O at 40 °C(b) 130 g C12H22O11/100 g H2O at 50 °C(c) 130 g C12H22O11/100 g H2O at 60 °C.
Assume that 100 g of LiCl is dissolved in 100 g of water at 100 °C and the solution is allowed to cool to 20 °C.(a) How much LiCl remains in solution?(b) How much LiCl crystallizes from the solution?
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