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
Ask a Question

Search
Sign In
Register

study help
sciences
general chemistry principles

Questions and Answers of General Chemistry Principles

(A) What is the molar solubility of PbI2 in 0.10 M Pb(NO3)2(aq)? To which ion concentration should the solubility be related?(B) What is the molar solubility of Fe(OH)3 in a buffered solution with pH
Three drops of 0.20 M KI are added to 100.0 mL of 0.010 M Pb(NO3)2. Will a precipitate of lead(II) iodide form? (Assume 1 drop = 0.05 mL.) Pbl₂(s) — Pb²+ (aq) + 21¯(aq) Ksp = 7.1 × 10-⁹
Determine [Mg2+] in a saturated solution of Mg(OH)2 at (a) pH = 10.00 and (b) pH = 5.00. Is each of these a plausible quantity? Explain.
(A) Three drops of 0.20 M KI are added to 100.0 mL of a 0.010 M solution of AgNO3. Will a precipitate of silver iodide form?(B) We saw in Example 18-5 that a 3-drop volume of 0.20 M KI is
The first step in a commercial process in which magnesium is obtained from seawater involves precipitating Mg2+ as Mg(OH)2(s). The magnesium ion concentration in seawater is about 0.059 M. If a
The measured molar solubility of AgCl in water is 1.3 x 10-5 M. In the presence of Cl-(aq) as a common ion at different concentrations, the measured solubilities of AgCl are as listed below.[Cl-], M:
(A) A typical Ca2+ concentration in seawater is 0.010 M. Will the precipitation of Ca(OH)2 be complete from a seawater sample in which [OH-] is maintained at 0.040 M?(B) What [OH-] should be
AgNO3(aq) is slowly added to a solution that has [CrO42-] = 0.010 M and [Br-] = 0.010 M.(a) Show that AgBr(s) should precipitate before Ag2CrO4(s) does.(b) When Ag2CrO4(s) begins to precipitate, what
(A) AgNO3(aq) is slowly added to a solution with [CI-] = 0.115 M and [Br-] = 0.264 M. What percent of the Br- remains unprecipitated at the point at which AgCl(s) begins to precipitate?(B) A solution
An unknown contains one or more of Pb2+, Hg22+, and Ag+. It forms a white precipitate with HCl(aq). The precipitate is treated with hot water, yielding a solution that gives a yellow precipitate with
Should Mg(OH)2(s) precipitate from a solution that is 0.010 M MgCl2 and also 0.10 M NH3?
The dissolution of PbS(s) in water is given byIn an apparent violation of Le Châtelier’s principle, the addition of NaOH to the solution leads more PbS to dissolve. Explain. PbS(s) + H₂O(1)
(A) Should Mg(OH)2(s) precipitate from a solution that is 0.010 M MgCl2(aq) and also 0.10 M NaCH3COO? Ksp[Mg(OH)2] = 1.8 x 10-11; Ka(CH3COOH) = 1.8 x 10-5. What equilibrium expression establishes
What [NH4+] must be maintained to prevent precipitation of Mg(OH)2(s) from a solution that is 0.010 M MgCl2 and 0.10 M NH3?
Both Cu2+ and Ag+ are present in the same aqueous solution. Explain which of the following reagents would work best in separating these ions, precipitating one and leaving the other in solution:
(A) What minimum [NH4+] must be present to prevent precipitation of Mn(OH)2(s) from a solution that is 0.0050 M MnCl2 and 0.025 M NH3? For Mn(OH)2, Ksp = 1.9 x 10-13.(B) What is the molar solubility
Predict what will happen if nitric acid is added to a solution of [Ag(NH3)2]Cl in NH3(aq).
(A) Copper(II) ion forms both an insoluble hydroxide and the complex ion [Cu(NH3)4]2+. Write equations to represent the expected reaction when (a) CuSO4(aq) and NaOH(aq) are mixed; (b) An excess of
A 0.10 mol sample of AgNO3 is dissolved in 1.00 L of 1.00 M NH3. If 0.010 mol NaCl is added to this solution, will AgCl(s) precipitate?
(A) Will AgCl(s) precipitate from 1.50 L of a solution that is 0.100 M AgNO3 and 0.225 M NH3 if 1.00 mL of 3.50 M NaCl is added? What are [Ag+] and [Cl-] immediately after the addition of the 1.00 mL
What is the minimum concentration of NH3 needed to prevent AgCl(s) from precipitating from 1.00 L of a solution containing 0.10 mol AgNO3 and 0.010 mol NaCl?
(A) What [NH3]tot is necessary to keep AgCl from precipitating from a solution that is 0.13 M AgNO3 and 0.0075 M NaCl?(B) What minimum concentration of thiosulfate ion, S2O32-, should be present in
What is the molar solubility of AgCl in 0.100 M NH3(aq)?
(A) What is the molar solubility of Fe(OH)3 in a solution containing 0.100 M C2O42-? For [Fe(C2O4)3]3-, Kf = 2 x 1020.(B) Without doing detailed calculations, show that the order of decreasing
Show that PbS(s) will precipitate but FeS(s) will not precipitate from a solution that is 0.010 M in Pb2+, 0.010 M in Fe2+, saturated in H2S (0.10 M H2S), and maintained with [H3O+] = 0.30 M. For
(A) Show that Ag2S(s) (Kspa = 6 x 10-30) should precipitate and that FeS(s) Kspa = 6 x 102) should not precipitate from a solution that is 0.010 M Ag+ and 0.020 M Fe2+, but otherwise under the same
(A) Heavy fertilizer use can lead to phosphate pollution in lakes, causing an explosion of plant growth, particularly algae. Excess algae deplete the lake of the oxygen necessary for other plant
The standard electrode potential for the reduction of Eu3+(aq) to Eu2+(aq) is -0.43 V. Use the data in Appendix D to determine which of the following is capable of reducing Eu3+(aq) to Eu2+(aq) under
Write the half-cell reactions and the balanced chemical equation for the electrochemical cells diagrammed here. Use data from Table 19.1 and Appendix D to calculate E°cell for each reaction.Table
Dichromate ion (Cr2O72-) in acidic solution is a good oxidizing agent. Which of the following oxidations can be accomplished with dichromate ion in acidic solution? Explain. 2+ (a) Sn²+ (aq) to Sn++
Consider the reaction Co(s) + Ni2+(aq) → Co2+(aq) + Ni(s), with E°cell = 0.02 V. If Co(s) is added to a solution with [Ni2+] = 1 M, should the reaction go to completion? Explain.
Write cell reactions for the electrochemical cells diagrammed here, and use data from Table 19.1 to calculate E°cell for each reaction.Table 19.1 2+ (a) Al(s) Al³+ (aq)||Sn²+ (aq)|Sn(s) (b) Pt(s)
Use the data in Appendix D to calculate the standard cell potential for each of the following reactions. Which reactions will occur spontaneously? (a) H₂(g) + F2 (g) (b) Cu(s) + Ba²+ (aq) 2 H(aq)
Predict whether the following metals will react with the acid indicated. If a reaction does occur, write the net ionic equation for the reaction. Assume that reactants and products are in their
Use the data in Appendix D to calculate the standard cell potential for each of the following reactions. Which reactions will occur spontaneously? 2+ Fe2+ ²+ (aq) + Ag+ (aq) 2 Sn²+ (aq) Hg2 (a)
Predict whether, to any significant extent, (a) Fe(s) will displace Zn2+(aq);(b) MnO4-(aq) will oxidize Cl-(aq) to Cl2(g) in acidic solution;(c) Ag(s) will react with 1 M HCl(aq);(d) O2(g) will
In each of the following examples, sketch a voltaic cell that uses the given reaction. Label the anode and cathode; indicate the direction of electron flow; write a balanced equation for the cell
Write the equilibrium constant expression for each of the following reactions, and determine the value of K at 25 °C. Use data from Table 19.1.Table 19.1 2 V² (a) 2 V³+ (aq) + Ni(s) — > (b)
Write a cell diagram and calculate the value of E°cell for a voltaic cell in which (a) Cl₂(g) is reduced to Cl(aq) and Fe(s) is oxidized to Fe²+ (aq); (b) Ag (aq) is displaced from solution by
Use thermodynamic data from Appendix D to calculate a theoretical voltage of the silver–zinc button cell described on page 893. TABLE D.1 Ground-State Electron Configurations Element Configuration
Determine the values of ΔrG° for the following reactions carried out in voltaic cells. (a) 2 Al(s) + 3 Cu²+ (aq) (b) O₂(g) +41 (aq) + 4 H*(aq) 2 A1³+ (aq) + 3 Cu(s) 2 H₂O(1) +2 12(s) (c)
Consider the voltaic cell below.Use data from Appendix D to determine (a) The equation for the cell reaction; (b) E°cell; (c) ΔrG°; (d) K; (e) Whether the reaction goes essentially to
The theoretical voltage of the aluminum–air battery is E°cell = 2.71 V. Use data from Appendix D and equation (19.28) to determine ΔfG° for Al[(OH)4]-.Eq. 19.28 4 Al(s) + 3 O₂(g) + 6 H₂O(1)
For the reaction answer the following questions:(a) Can a solution be prepared at 298 K that has(b) If not, in which direction will a reaction occur? 2 H+ (aq) + BrO4 (aq) + 2 Ce³+ (aq) BrO3(aq) +
For the reaction 2 Cu+(aq) + Sn4+(aq) → 2 Cu2+(aq) + Sn2+(aq), E°cell = -0.0050 V, (a) Can a solution be prepared at 298 K that is 0.500 M in each of the four ions?(b) If not, in which direction
By the method of combining reduction half-cell reactions illustrated, determine E°lrO2/Ir , given that E°lr3+/Ir = 1.156 V and E°IrO2/Ir3+ = 0.223 V.
Consider the reduction half-cell reactions listed in Appendix D, and give plausible explanations for the following observations:(a) For some half-cell reactions E depends on pH; for others, it does
Use the Nernst equation and Table 19.1 to calculate Ecell for each of the following cells.Table 19.1 (a) Al(s) Al³+ (0.18 M)||Fe2+ (0.85 M) Fe(s) (b) Ag(s) Ag (0.34 M)||CI (0.098 M), Cl₂(g, 0.55
A voltaic cell represented by the following cell diagram has Ecell = 1.250 V. What must be [Ag+] in the cell? 2+ Zn(s) Zn²+ (1.00 M)||Ag+ (x M) Ag(s)
Use the Nernst equation and data from Appendix D to calculate Ecell for each of the following cells. (a) Mn(s) Mn²+ (0.40 M)||Cr³+ (0.35 M), Cr²+ (0.25 M) Pt(s) (b) Mg(s) Mg2+ (0.016
Determine E°MoO2/Mo3+, given that E°H2MoO4/MoO2 = 0.646 V and E°H2MoO4/Mo3+ = 0.428 V.
For the cell pictured in Figure 19-11, what is Ecell if the unknown solution in the half-cell on the left (a) Has pH = 5.25;(b) Is 0.0103 M HCl; (c) Is 0.158 M CH3COOH (Ka = 1.8 x 10-5)?Figure
If [Zn2+] is maintained at 1.0 M, (a) What is the minimum [Cu2+] for which reaction (19.3) is spontaneous in the forward direction?(b) Should the displacement of Cu2+(aq) by Zn(s) go to completion?
Write an equation to represent the oxidation of Cl-(aq) to Cl2(g) by PbO2(s) in an acidic solution. Will this reaction occur spontaneously in the forward direction if all other reactants and products
Can the displacement of Pb(s) from 1.0 M Pb(NO3)2 be carried to completion by tin metal? Explain.
A voltaic cell, with Ecell = 0.180 V, is constructed as follows:What is the Ksp of Ag3PO4? Ag(s) Ag (satd Ag3PO4)||Ag (0.140 M) Ag(s)
A concentration cell is constructed of two hydrogen electrodes: one immersed in a solution with [H+] = 1.0 M and the other in 0.65 M KOH.(a) Determine Ecell for the reaction that occurs.(b) Compare
For the voltaic cell,(a) What is Ecell initially?(b) If the cell is allowed to operate spontaneously, will Ecell increase, decrease, or remain constant with time? Explain.(c) What will be Ecell
Refer to the discussion of the Leclanché cell.(a) Combine the several equations written for the operation of the Leclanché cell into a single overall equation.(b) Given that the voltage of the
For the voltaic cell,(a) what is Ecell initially?(b) As the cell operates, will Ecell increase, decrease, or remain constant with time? Explain.(c) What will be Ecell when [Ag+] has increased to
Derive a balanced equation for the reaction occurring in the cell: (a) If E°cell = 1.21 V, calculate ΔrG° and the equilibrium constant for the reaction.(b) Use the Nernst equation to determine
For the alkaline Leclanché cell.(a) write the overall cell reaction.(b) Determine E°cell for that cell reaction.Figure 19.14 The Leclanché (Dry) Cell The most common form of voltaic cell is the
Show that the oxidation of Cl-(aq) to Cl2(g) by Cr2O72-(aq) in acidic solution, with reactants and products in their standard states, does not occur spontaneously. Explain why it is still possible to
The iron–chromium redox battery makes use of the reactionoccurring at a chromium anode and an iron cathode.(a) Write a cell diagram for this battery.(b) Calculate the theoretical voltage of the
What is the theoretical standard cell voltage, E°cell, of each of the following voltaic cells? (a) The hydrogen–oxygen fuel cell described by equation (19.26); (b) The zinc–air battery; (c) A
One of the advantages of the aluminum-air battery over the iron–air and zinc–air batteries is the greater quantity of charge transferred per unit mass of metal consumed. Show that this is indeed
Refer to Figure 19-20, and describe in words or with a sketch what you would expect to happen in each of the following cases.(a) Several turns of copper wire are wrapped around the head and tip of an
Describe how you might construct batteries with each of the following voltages: (a) 0.10 V; (b) 2.5 V; (c) 10.0 V.Be as specific as you can about the electrodes and solution concentrations you
When an iron pipe is partly submerged in water, the iron dissolves more readily below the waterline than at the waterline. Explain this observation by relating it to the description of corrosion
Natural gas transmission pipes are sometimes protected against corrosion by the maintenance of a small potential difference between the pipe and an inert electrode buried in the ground. Describe how
In the construction of the Statue of Liberty, a framework of iron ribs was covered with thin sheets of copper less than 2.5 mm thick. A layer of asbestos separated the copper skin and iron framework.
How many grams of metal are deposited at the cathode by the passage of 2.15 A of current for 75 min in the electrolysis of an aqueous solution containing (a) Zn2+;(b) Al3+;(c) Ag+;(d) Ni2+?
Which of the following reactions occur spontaneously, and which can be brought about only through electrolysis, assuming that all reactants and products are in their standard states? For those
A quantity of electric charge brings about the deposition of 3.28 g Cu at a cathode during the electrolysis of a solution containing Cu2+(aq). What volume of H2(g), measured at 28.2 °C and 763
An aqueous solution of K2SO4 is electrolyzed by means of Pt electrodes.(a) Which of the following gases should form at the anode: O2, H2, SO2, SO3? Explain.(b) What product should form at the
A dilute aqueous solution of Na2SO4 is electrolyzed between Pt electrodes for 3.75 h with a current of 2.83 A. What volume of gas, saturated with water vapor at 25 °C and at a total pressure of 742
If a lead storage battery is charged at too high a voltage, gases are produced at each electrode. (It is possible to recharge a lead-storage battery only because of the high overpotential for gas
Calculate the quantity indicated for each of the following electrolyses.(a) The mass of Zn deposited at the cathode in 42.5 min when 1.87 A of current is passed through an aqueous solution of
Calculate the quantity indicated for each of the following electrolyses.(a) [Cu2+] remaining in 425 mL of a solution that was originally 0.366 M CuSO4, after passage of 2.68 A for 282 s and the
Electrolysis is carried out for 2.00 h in the following cell. The platinum cathode, which has a mass of 25.0782 g, weighs 25.8639 g after the electrolysis. The platinum anode weighs the same before
A coulometer is a device for measuring a quantity of electric charge. In a silver coulometer, Ag+(aq) is reduced to Ag(s) at a Pt cathode. If 1.206 g Ag is deposited in 1412 s by a certain quantity
A solution containing both Ag+ and Cu2+ ions is subjected to electrolysis. (a) Which metal should plate out first? (b) Plating out is finished after a current of 0.75 A is passed through the
Two voltaic cells are assembled in which the following reactions occur. V²+ (aq) + VO²+ (aq) + 2 H+ (aq) 2 V3+ (aq) + H₂O(1) Ecell = 0.616 V V³+ (aq) + Ag (aq) + H₂O(1) VO2+ (aq) + 2 H+ (aq) +
A solution containing a mixture of a platinum(II) salt contaminated by approximately 10 mole % of another oxidation state is electrolyzed at 1.20 A for 32.0 minutes, at which point no more platinum
Suppose that a fully charged lead–acid battery contains 1.50 L of 5.00 M H2SO4. What will be the concentration of H2SO4 in the battery after 2.50 A of current is drawn from the battery for 6.0 h?
For the half-cell reaction V3+(aq) + e- → V2+(aq), E° = -0.255 V. If excess Ni(s) is added to a solution in which [V3+(aq)] = 0.500 M, what will be the concentration of Ni2+(aq) when the
The energy consumption in electrolysis depends on the product of the charge and the voltage [volt x coulomb = V · C = J(joules)]. Determine the theoretical energy consumption per 1000 kg Cl2
A voltaic cell is constructed based on the following reaction and initial concentrations:Calculate [Fe2+] when the cell reaction reaches equilibrium. Fe²+ (0.0050 M) + Ag+ (2.0 M) = Fe³+ (0.0050 M)
Use data from Table 19.1 to predict whether, to any significant extent, (a) Mg(s) will displace Pb2+ from aqueous solution;(b) Sn(s) will react with and dissolve in 1 M HCl;(c) SO42- will oxidize
To construct a voltaic cell with Ecell = 0.0860 V, what [Cl-] must be present in the cathode half-cell to achieve this result? Ag(s) Ag (satd AgI)||Ag¹(satd AgCl, x M CI) Ag(s)
The hydrazine fuel cell is based on the reactionThe theoretical E°cell of this fuel cell is 1.559 V. Use this information and data from Appendix D to calculate a value of ΔfG° for [N2H4(aq)].
Describe a laboratory experiment that you could perform to evaluate the Faraday constant, F, and then show how you could use this value to determine the Avogadro constant.
Use the following data and data from Appendix D to determine the quantity of heat needed to convert 15.0 g of solid mercury at -50.0 °C to mercury vapor at 25 °C. Specific heats: Hg(s), 24.3 J
In the manufacture of ammonia, the chief source of hydrogen gas is the following reaction for the reforming of methane at high temperatures.The following data are also given.At 1000 K, 1.00 mol each
At 1.00 atm, the solubility of O2 in water is 2.18 x 10-3 M at 0 °C and 1.26 x 10-3 M at 25 °C. What volume of O2(g) measured at 25 °C and 1.00 atm, is expelled when 515 mL of water saturated with
A saturated solution prepared at 70 °C contains 32.0 g CuSO4 per 100.0 g solution. A 335 g sample of this solution is then cooled to 0 °C and CuSO4 · 5 H2O crystallizes out. If the concentration
How would you write the reaction quotient expression for Cu(s) + 2 H+(aq) → Cu2+(aq) + H2(g) ? Write this first in terms of activities and then convert to pressures and concentrations.
Based on these descriptions, write a balanced equation and the corresponding expression for each reversible reaction.(a) Carbonyl fluoride, COF2(g), decomposes into gaseous carbon dioxide and gaseous
These equilibrium concentrations are measured at 298 K: [Cu+]eq = 0.148 M, [Sn2+]eq = 0.124 M, and [Sn4+]eq = 0.176 M. What is the equilibrium concentration of Cu2+(aq)?
(A) In another experiment also carried out at 298 K, equal concentrations of [Cu+], [Sn4+], and [Sn2+] are found to be in equilibrium. What must be the equilibrium concentration of [Cu2+]?(B) At 25

Showing 1200 - 1300 of 4009

First
6
7
8
9
10
11
12
13
14
15
16
17
18
19
20
Last

Get In Touch

About Us
Contact Us
Career
Jobs
FAQ
Campus Ambassador

Company Info

Security
Copyrights
Privacy Policy
Terms & Condition
SolutionInn Fee
Scholarship

Services

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

Copyright © 2024 SolutionInn All Rights Reserved.

Get the SolutionInn - Study Help App