All Matches

Solution Library

Expert Answer

Textbooks

Search Textbook questions, tutors and Books

Oops, something went wrong!

Change your search query and then try again

Result Not Found

Books FREE
Tutors
Study Help
Hire a Tutor
AI Study Help New

Search
Sign In
Register

study help
engineering
chemical engineering

Questions and Answers of Chemical Engineering

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
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
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)
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,
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,
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
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
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
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
(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,
(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
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
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
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
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
(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?
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
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
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
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
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
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
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
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
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
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
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
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
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
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
(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
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
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
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
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
(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
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
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
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
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
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 →
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
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
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
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
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
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
(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
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
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
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
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
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
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
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
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
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.

Showing 4200 - 4300 of 6780

First
36
37
38
39
40
41
42
43
44
45
46
47
48
49
50
Last

Services

Sitemap
Fun
Definitions
Become Tutor
Study Help Categories
Recent Questions
Expert Questions

Company Info

Security
Copyrights
Privacy Policy
Terms & Conditions
SolutionInn Fee
Scholarship

Get In Touch

About Us
Contact Us
Career
Jobs
FAQ
Campus Ambassador

Secure Payment

Download Our App

© 2024 SolutionInn. All Rights Reserved