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engineering
chemical engineering

Chemistry The Central Science 12th edition Theodore Brown, Eugene LeMay, Bruce Bursten, Catherine Murphy, Patrick Woodward - Solutions

How many milliliters of 0.0850 M NaOH are required to titrate each of the following solutions to the equivalence point: (a) 40.0 mL of 0.0900 M HNO3, (b) 35.0 mL of 0.0850 M CH3COOH, (c) 50.0 mL of a solution that contains 1.85 g of HCl per liter?
How many milliliters of 0.105 M HCl are needed to titrate each of the following solutions to the equivalence point: (a) 45.0 mL of 0.0950 M NaOH, (b) 22.5 mL of 0.118 M NH3, (c) 125.0 mL of a solution that contains 1.35 g of NaOH perliter?
A 20.0-mL sample of 0.200 M HBr solution is titrated with 0.200MNaOH solution. Calculate the pH of the solution after the following volumes of base have been added: (a) 15.0 mL, (b) 19.9 mL, (c) 20.0 mL, (d) 20.1 mL, (e) 35.0 mL.
A 20.0-mL sample of 0.150 M KOH is titrated with 0.125 M HClO4 solution. Calculate the pH after the following volumes of acid have been added: (a) 20.0 mL, (b) 23.0 mL, (c) 24.0 mL, (d) 25.0 mL, (e) 30.0 mL.
A 35.0-mL sample of 0.150 M acetic acid (CH3 COOH) is titrated with 0.150 M NaOH solution. Calculate the pH after the following volumes of base have been added: (a) 0 mL, (b) 17.5 mL, (c) 34.5 mL, (d) 35.0 mL, (e) 35.5 mL, (f) 50.0 mL.
Consider the titration of 30.0 mL of 0.050 MNH3 with 0.025 M HCl. Calculate the pH after the following volumes of titrant have been added: (a) 0 mL, (b) 20.0 mL, (c) 59.0 mL, (d) 60.0 mL, (e) 61.0 mL, (f) 65.0 mL.
Calculate the pH at the equivalence point for titrating 0.200 M solutions of each of the following bases with 0.200 M HBr: (a) Sodium hydroxide (NaOH), (b) Hydroxylamine (NH2OH), (c) Aniline (C6H5NH2).
Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.080 MNaOH: (a) hydrobromic acid (HBr), (b) chlorous acid (HClO2), (c) benzoic acid (C6H5COOH).
(a) Why is the concentration of undissolved solid not explicitly included in the expression for the solubility-product constant? (b) Write the expression for the solubility-product constant for each of the following strong electrolytes: AgI, SrSO4, Fe(OH)2, and Hg2Br2.
The following drawings represent solutions at various stages of the titration of a weak acid, HA, with NaOH. (The Na+ ions and water molecules have been omitted for clarity.) To which of the following regions of the titration curve does each drawing correspond:(a) Before addition of NaOH,(b) After
(a) Explain the difference between solubility and solubilityproduct constant. (b) Write the expression for the solubility-product constant for each of the following ionic compounds:MnCO3, Hg(OH)2, and Cu3(PO4)2.
(a) If the molar solubility of CaF2 at 35°C is 1.24 x 10-3 mol/L what is ksp at this temperacture?
(a) The molar solubility of PbBr2 at 25°C is1.0 x 10-2 mol / L, Calculate Ksp.
A 1.00-L solution saturated at 25°C with calcium oxalate (CaC2O4) contains 0.0061 g of CaC2O4. Calculate the solubility product constant for this salt at 25°C.
A 1.00-L solution saturated at 25°C with lead (II) iodide contains 0.54 g of PbI2. Calculate the solubility-product constant for this salt at 25°C.
Using Appendix D, calculate the molar solubility of AgBr in (a) Pure water,
Calculate the solubility of LaF3 in grams per liter in (a) Pure water,
Consider a beaker containing a saturated solution of CaF2 in equilibrium with undissolved CaF2 (s). (a) If solid CaCl2 is added to this solution, will the amount of solid CaF2 at the bottom of the beaker increase, decrease, or remain the same? (b) Will the concentration of ions in solution
Consider a beaker containing a saturated solution of Pbl2 in equilibrium with undissolved Pbl2(s). (a) If solid KI is added to this solution, will the amount of solid PbI2 at the bottom of the beaker increase, decrease, or remain the same? (b) Will the concentration of ions in solution increase
Calculate the solubility of Mn(OH)2 in grams per liter when buffered at pH (a) 7.0, (b) 9.5, (c) 11.8.
Match the following descriptions of titration curves with the diagrams:(a) Strong acid added to strong base,(b) Strong base added to weak acid,(c) Strong base added to strong acid,(d) Strong base added to polyprotic acid. [Section 17.3]
Calculate the molar solubility of Ni(OH)2 when buffered at pH (a) 8.0, (b) 10.0, (c) 12.0.
Which of the following salts will be substantially more soluble in acidic solution than in pure water: (a) ZnCO3, (b) ZnS, (c) BiI3, (d) AgCN, (e) Ba3(PO4)2?
For each of the following slightly soluble salts, write the net ionic equation, if any, for reaction with acid: (a) MnS, (b) PbF2, (c) AuCl3, (d) Hg2C2O4, (e) CuBr.
From the value of Kf listed in Table 17.1, calculate the concentration of Ni2+ n 1.0 L of a solution that contains a total of mol 1 x 10-3 of nickel (II) ion and that is 0.20 M in NH3.
To what final concentration of NH3 must a solution be adjusted to just dissolve 0.020 mol of NiC2O4 in 1.0 L of solution? (Hint: You can neglect the hydrolysis of C2O42-because the solution will be quite basic.)
Use values of ksp for AgI and kf for Ag(CN)2 - to(a) Calculate the molar solubility of agi in pure water,(b) Calculate the equilibrium constant for the reaction
Using the value of Ksp for Ag2S, Ka2 and Ka1 for H2S, and Kf = 1.1 x 105 for AgCI2-, calculate the equilibrium constant for the following reaction:
(a) Will Ca(OH)2 precipitate from solution if the pH of a 0.050 M solution of CaCl2 is adjusted to 8.0? (b) Will Ag2SO4 precipitate when 100 mL of 0.050 M AgNO3 is mixed with 10 mL of 5.0 x 10-2 M Na2SO4 solution?
(a) Will Co(OH)2 precipitate from solution if the pH of a 0.020 M solution of Co(NO3)2 is adjusted to 8.5? (b) Will AgIO3 precipitate when 20 mL of 0.010 M AgNO3 is mixed with 10 mL of 0.015 M NaIO3? (Ksp of AgIO3 is 3.1 x10-8.)
Calculate the minimum pH needed to precipitate Mn(OH)2 so completely that the concentration of is less than 1 per liter [1 part per billion (ppb)].
Equal volumes of two acids are titrated with 0.10 MNaOH resulting in the two titration curves shown in the following figure.
Suppose that a 10-mL sample of a solution is to be tested for I-ion by addition of 1 drop (0.2mL) of 0.10 M Pb(NO3)2. What is the minimum number of 1- grams of that must be present for Pbl2 (s) to form?
A solution contains 2.0 x 10-4 M Ag+ and 1.5 x 10 -3 M Pb2+ .If NaI is added, will AgI (Ksp = 8.3 x 10-17) or PbI2 (Ksp = 7.9 x 10 -9) precipitate first? Specify the concentration of 1-needed to begin precipitation.
A solution of Na2SO4 is added drop wise to a solution that is 0.010 M in Ba2+ and 0.010 M in Sr2+. (a) What concentration of SO42- is necessary to begin precipitation? (Neglect volume changes. BaSO4 ksp = 1.1 x 10 -10 SrSO4:) (b) Which cation precipitates first? (c) What is the concentration of
A solution contains three anions with the following concentrations: 0.20 MCrO42-, 0.10 M CO32-, and 0.010. MCI- If a dilute AgNO3 solution is slowly added to the solution, what is the first compound to precipitate: Ag2CrO4, (Ksp = 1.2 x 10-12)Ag2CO3, (Ksp = 8.1 x 10-12) or AgCl(Ksp = 1.8 x 10-12)?
A 1.0 M Na2SO4 solution is slowly added to 10.0 mL of a solution that is 0.20 M in Ca2+ and 0.30 M in Ag+. (a) Which compound will precipitate first: CaSO4 (Ksp = 2.4 x 10-5) or Ag2SO4(Ksp = 1.5 x 10-5) ? (b) How much Na2SO4 solution must be added to initiate the precipitation?
A solution containing an unknown number of metal ions is treated with dilute HCl; no precipitate forms. The pH is adjusted to about 1, and H2S is bubbled through. Again, no precipitate forms. The pH of the solution is then adjusted to about 8. Again, H2S is bubbled through. This time a precipitate
An unknown solid is entirely soluble in water. On addition of dilute HCl, a precipitate forms. After the precipitate is filtered off, the pH is adjusted to about 1 and H2S is bubbled in; a precipitate again forms. After filtering off this precipitate, the pH is adjusted to 8 and H2S is again added;
In the course of various qualitative analysis procedures, the following mixtures are encountered: (a) Zn2+ and, Cd2+ (b) Cr (OH)3 and Fe (OH)3, (c) Mg2+ and K+, (d) Ag+ andMn2+. Suggest how each mixture might be separated.
Suggest how the cations in each of the following solution mixtures can be separated: (a) Na+ and, Cd2+ (b) Cd2+ and, Mg2+ (c) Pb2+andAI3+ , (d) Ag+ andHg2+ .
(a) Precipitation of the group 4 cations of Figure 17.23 requires a basic medium. Why is this so? (b) What is the most significant difference between the sulfides precipitated in group 2 and those precipitated in group 3? (c) Suggest a procedure that would serve to redissolve the group 3 cations
A saturated solution of Cd(OH)2 is shown in the middle beaker. If hydrochloric acid solution is added, the solubility of Cd(OH)2 will increase, causing additional solid to dissolve. Which of the two choices, Beaker A or Beaker B, accurately represents the solution after equilibrium is
A student who is in a great hurry to finish his laboratory work decides that his qualitative analysis unknown contains a metal ion from group 4 of Figure 17.23.He therefore tests his sample directly with (NH4) 2HPO4, skipping earlier tests for the metal ions in groups 1, 2, and 3. He observes a
Derive an equation similar to the Henderson-Hasselbalch equation relating the pOH of a buffer to the of its base component.
Benzenesulfonic acid is a monoprotic acid with pKa = 2.25. Calculate the pH of a buffer composed of 0.150 Mbenzenesulfonic acid and 0.125 M sodium benzenesulfonate.
The following graphs represent the behavior of BaCO3 under different circumstances. In each case the vertical axis indicates the solubility of the BaCO3 and the horizontal axis represents the concentration of some other reagent. (a) Which graph represents what happens to the solubility of BaCO3 as
At 273 K and 1 atm pressure, one mole of an ideal gas occupies(a) Looking back at Figure 18.1, do you predict that 1 mole of an ideal gas in the middle of the stratosphere would occupy a greater or smaller volume than 22.4 L?(b) Looking at Figure 18.1, we see that the temperature is lower at 85 km
One mystery in environmental science is the imbalance in the "carbon dioxide budget." Considering only human activities, scientists have estimated that 1.6 billion metric tons of CO2 is added to the atmosphere every year because of deforestation (plants use CO2, and fewer plants will leave more CO2
(a) What is the primary basis for the division of the atmosphere into different regions? (b) Name the regions of the atmosphere, indicating the altitude interval for each one.
(a) How are the boundaries between the regions of the atmosphere determined? (b) Explain why the stratosphere, which is more than 20 miles thick, has a smaller total mass than the troposphere, which is less than 10 miles thick.
Air pollution in the Mexico City metropolitan area is among the worst in the world. The concentration of ozone in Mexico City has been measured at 441 ppb (0.441 ppm).Mexico City sits at an altitude of 7400 feet, which means its atmospheric pressure is only 0.67 atm. (a) Calculate the partial
From the data in Table 18.1, calculate the partial pressures of carbon dioxide and argon when the total atmospheric pressure is 1.05 bar.
The average concentration of carbon monoxide in air in an Ohio city in 2006 was 3.5 ppm. Calculate the number of CO molecules in 1.0 L of this air at a pressure of 759 torr and a temperature of 22oC.
(a) From the data in Table 18.1, what is the concentration of neon in the atmosphere in ppm?In Table 18.1(b) What is the concentration of neon in the atmosphere in molecules per L, assuming an atmospheric pressure of 730 torr and a temperature of 296 K?
The dissociation energy of a carbon-bromine bond is typically about 210 kJ / mol. (a) What is the maximum wavelength of photons that can cause C-Br bond dissociation? (b) Which kind of electromagnetic radiation-ultraviolet, visible, or infrared-does the wavelength you calculated in part (a)
In CF3Cl the C-Cl bond-dissociation energy is 339 kJ / mol. In CCl4 the bond-dissociation energy is 293 kJ / mol. What is the range of wavelengths of photons that can cause C-Cl bond rupture in one molecule but not in the other?
(a) Distinguish between photodissociation and photoionization. (b) Use the energy requirements of these two processes to explain why photodissociation of oxygen is more important than photoionization of oxygen at altitudes below about 90 km.
Molecules in the upper atmosphere tend to contain double and triple bonds rather than single bonds. Suggest an explanation.
Why is the photodissociation of N2 in the atmosphere relatively unimportant compared with the photodissociation of O2?
Do the reactions involved in ozone depletion involve changes in oxidation state of the O atoms? Explain.
Explain how the reactions of ozone in the stratosphere are responsible for the relatively warm temperatures of the stratosphere.
(a) What is the difference between chlorofluorocarbons and hydrofluorocarbons? (b) Why are hydrofluorocarbons potentially less harmful to the ozone layer than CFCs?
Draw the Lewis structure for the chlorofluorocarbon CFC-11, CFCl3.What chemical characteristics of this substance allow it to effectively deplete stratospheric ozone?
(a) Why is the fluorine present in chlorofluorocarbons not a major contributor to depletion of the ozone layer? (b) What are the chemical forms in which chlorine exists in the stratosphere following cleavage of the carbon-chlorine bond?
Would you expect the substance CFBr3 to be effective in depleting the ozone layer, assuming that it is present in the stratosphere? Explain.
For each of the following gases, make a list of known or possible naturally occurring sources: (a) CH4, (b) SO2, (c) NO.
Why is rainwater naturally acidic, even in the absence of polluting gases such as SO2?
(a)Write a chemical equation that describes the attack of acid rain on limestone, CaCO3. (b) If a limestone sculpture were treated to form a surface layer of calcium sulfate, would this help to slow down the effects of acid rain? Explain.
The figure shows the three lowest regions of Earth's atmosphere.(a) Name each and indicate the approximate elevations at which the boundaries occur.(b) In which region is ozone a pollutant? In which region does it filter UV solar radiation?(c) In which region is infrared radiation from Earth's
The first stage in corrosion of iron upon exposure to air is oxidation to Fe2+. (a) Write a balanced chemical equation to show the reaction of iron with oxygen and protons from acid rain. (b) Would you expect the same sort of reaction to occur with a silver surface? Explain.
Alcohol-based fuels for automobiles lead to the production of formaldehyde (CH2O) in exhaust gases. Formaldehyde undergoes photodissociation, which contributes to photochemical smog: CH2O + hv → CHO + H The maximum wavelength of light that can cause this reaction is 335 nm. (a) In what part of
An important reaction in the formation of photochemical smog is the photodissociation of NO2:NO2 + hv → NO(g) + O(g)The maximum wavelength of light that can cause this reaction is 420 nm.(a) In what part of the electromagnetic spectrum is light with this wavelength found?(b) What is the maximum
Explain why increasing concentrations of CO2 in the atmosphere affect the quantity of energy leaving Earth but do not affect the quantity of energy entering from the Sun.
(a) With respect to absorption of radiant energy, what distinguishes a greenhouse gas from a nongreenhouse gas? (b) CH4 is a greenhouse gas, but N2 is not. How might the molecular structure of CH4 explain why it is a greenhouse gas?
What is the molarity of Na+ in a solution of NaCl whose salinity is 5.6 if the solution has a density of 1.03 g/mol?
Phosphorus is present in seawater to the extent of 0.07 ppm by mass. If the phosphorus is present as phosphate, PO43-calculate the corresponding molar concentration of phosphate in seawater.
The enthalpy of evaporation of water is 40.67 kJ/mol. Sunlight striking Earth's surface supplies 168 W per square meter (1 W = 1 watt = 1 j/s). (a) Assuming that evaporation of water is only due to energy input from the Sun, calculate how many grams of water could be evaporated from a 1.00 square
The enthalpy of fusion of water is 6.01 kJ/mol. Sunlight striking Earth's surface supplies 168 W per square meter (1 W = 1 watt = 1 J/s). (a) Assuming that melting of ice is only due to energy input from the Sun, calculate how many grams of ice could be melted from a 1.00 square meter patch of ice
A first-stage recovery of magnesium from seawater is precipitation of Mg(OH)2 with CaO:What mass of CaO, in grams, is needed to precipitate 1000 lb of Mg(OH)2?
You are working with an artist who has been commissioned to make a sculpture for a big city in the eastern United States. The artist is wondering what material to use to make her sculpture because she has heard that acid rain in the eastern United States might destroy it over time. You take samples
Gold is found in seawater at very low levels, about 0.05 ppb by mass. Assuming that gold is worth about $800 per troy ounce, how many liters of seawater would you have to process to obtain $1,000,000 worth of gold? Assume the density of seawater is 1.03 g/mL and that your gold recovery process is
(a)What is groundwater? (b)What is an aquifer?
The Ogallala aquifer is the largest in the United States, covering 450,000 km2 across eight states, from South Dakota to Texas. This aquifer provides 82% of the drinking water for the people who live in this region, although most (> 75%) of the water that is pumped from it is for irrigation.
Suppose that one wishes to use reverse osmosis to reduce the salt content of brackish water containing 0.22 M total salt concentration to a value of 0.01 M, thus rendering it usable for human consumption. What is the minimum pressure that needs to be applied in the permeators (Figure 18.19) to
Assume that a portable reverse-osmosis apparatus operates on seawater, whose concentrations of constituent ions are listed in Table 18.5, and that the desalinated water output has an effective molarity of about 0.02 M. What minimum pressure must be applied by hand pumping at 297 K to cause reverse
List the common products formed when an organic material containing the elements carbon, hydrogen, oxygen, sulfur, and nitrogen decomposes (a) Under aerobic conditions, (b) Under anaerobic conditions.
(a) Explain why the concentration of dissolved oxygen in freshwater is an important indicator of the quality of the water. (b) How is the solubility of oxygen in water affected by increasing temperature?
The organic anionis found in most detergents. Assume that the anion undergoes aerobic decomposition in the following manner: What is the total mass of O2 required to biodegrade 10.0 g of this substance?
The average daily mass of O2 taken up by sewage discharged in the United States is 59 g per person. How many liters of water at 9 ppm O2 are totally depleted of oxygen in 1 day by a population of 1,200,000 people?
Write a balanced chemical equation to describe how magnesium ions are removed in water treatment by the addition of slaked lime, Ca(OH)2.
(a) Which of the following ionic species could be responsible for hardness in a water supply: Ca2+, K+, Mg2+, Fe2+, Na+? (b) What properties of an ion determine whether it will contribute to water hardness?
How many moles of Ca(OH)2 and Na2CO3 should be added to soften 1200 L of water in which [Ca2+] = 5.0 × 10-4 M and [HCO3-] = 7.0 × 10-4 M?
The concentration of Ca2+ in a particular water supply is 5.7 × 10-3. The concentration of bicarbonate ion, HCO3-, in the same water is 1.7 ×10-3. What masses of Ca(OH)2 and Na2CO3 must be added to 5.0 ×107L of this water to reduce the level of Ca2+ to 20% of its original level?
Ferrous sulfate (FeSO4) is often used as a coagulant in water purification. The iron (II) salt is dissolved in the water to be purified, then oxidized to the iron (III) state by dissolved oxygen, at which time gelatinous Fe(OH)3 forms, assuming the pH is above approximately 6. Write balanced
What properties make a substance a good coagulant for water purification?
(a) What are trihalomethanes (THMs)? (b) Draw the Lewis structures of two example THMs.
If trihalomethanes are easily removed from water by aeration (bubbling with air), what does this imply about the vapor pressure of THMs compared to water?
One of the principles of green chemistry is that it is better to use as few steps as possible in making new chemicals. How does this principle relate to energy efficiency?
Discuss how catalysts can make processes more energy efficient.

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