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general chemistry principles

Questions and Answers of General Chemistry Principles

To 0.350 L of 0.150 M NH3 is added 0.150 L of 0.100 M MgCl2. How many grams of (NH4)2SO4 should be present to prevent precipitation of Mg(OH)2(s)?
Will the following precipitates form under the given conditions? (a) Pbl₂(s), from a solution that is 1.05 × 10-³ MHI, 1.05 × 10-3 M Nal, and 1.1 x 10-3 M Pb(NO3)2. (b) Mg(OH)2(s), from 2.50 L
PbCl2(s) is considerably more soluble in HCl(aq) than in pure water, but its solubility in HNO3(aq) is not much different from what it is in water. Explain this difference in behavior.
Thymol blue in its acid range is not a suitable indicator for the titration of HCl by NaOH. Suppose that a student uses thymol blue by mistake in the titration of Figure 17-8 and that the indicator
Solution (a) Is 100.0 mL of 0.100 M HCl and solution; (b) Is 150.0 mL of 0.100 M NaCH3COO. A few drops of thymol blue indicator are added to each solution. What is the color of each solution? What
You are asked to prepare a buffer solution with a pH of 3.50. The following solutions, all 0.100 M, are available to you: HCOOH, CH3COOH, H3PO4, NaHCOO, NaCH3COO, and NaH2PO4. Describe how you would
If 0.35 mL of 15 M NH3 is added to 0.750 L of the buffer solution in Exercise 16(a), what will be the pH of the resulting solution?Exercise 16(a)You prepare a buffer solution by dissolving 2.00 g
Calculate the change in pH that results from adding (a) 0.100 mol NaNO2 to 1.00 L of 0.100 M HNO2(aq);(b) 0.100 mol NaNO3 to 1.00 L of 0.100 M HNO3(aq).Why are the changes not the same?
3.00 mol of calcium chlorite is dissolved in enough water to produce 2.50 L of solution. Ka = 2.9 x 10-8 for HClO, and Ka = 1.1 x 10-2 for HClO2. Compute the pH of the solution.
Propionic acid, CH3CH2COOH, is 0.42% ionized in 0.80 M solution. The Ka for this acid is (a) 1.42 x 10-5;(b) 1.42 x 10-7;(c) 1.77 x 10-5;(d) 6.15 x 104;(e) None of these.
For H2SO3(aq), Ka1 = 1.3 x 10-2 and Ka2 = 6.3 x 10-8 . In 0.10 M H2SO3(aq), (a) [HSO3] = 0.013 M; (b) [SO3²] = 6.3 × 108 M; (c) [H3O¹] = 0.10 M; (d) [H3O¹] = 0.013 M; (e) [SO3²-] = 0.036 M.
It is possible to write simple equations to relate pH, pK, and concentrations (c) of various solutions. Three such equations are shown here.(a) Derive these three equations, and point out the
For the ionization of phenylacetic acid, C₂H₂CH₂CO₂H + H₂O — H3O+ + C²H5CH₂CO₂¯¯ Ka 4.9 x 10-5 = (a) What is [C6H5CH₂CO2¯] in 0.186 M C6H5CH₂CO₂H? (b) What is the pH of
What are the [H3O+] and pH of 0.085 M C2H5NH2?
25.00 mL of a HNO3(aq) solution with a pH of 2.12 is mixed with 25.00 mL of a KOH(aq) solution with a pH of 12.65. What is the pH of the final solution?
50.00 mL of 0.0155 M HI(aq) is mixed with 75.00 mL of 0.0106 M KOH(aq). What is the pH of the final solution?
In a manner similar to equation (16.3), represent the self-ionization of the following liquid solvents:(a) NH3;(b) HF; (c) CH3OH;(d) CH3COOH;(e) H2SO4.Eq. 16.3 2 H₂O(1) H₂O (aq) + OH(aq) (16.3)
Use your knowledge of electronegativities, but do not refer to tables or figures in the text, to arrange the following bonds in terms of increasing ionic character: C—H, F—H, Na—Cl, Br—H,
In the equilibrium described in Example 15-12, the percent dissociation of N2O4 can be expressed asWhat must be the total pressure of the gaseous mixture if N2O4(g) is to be 10.0% dissociated at 298
Refer to Example 15-13. Suppose that 0.100 L of the equilibrium mixture is diluted to 0.250 L with water. What will be the new concentrations when equilibrium is re-established?Example 15-13Solid
Explain why the percent of molecules that dissociate into atoms in reactions of the type I2(g) ⇌ 2 I(g) always increases with an increase in temperature.
1.00 g each of CO, H2O, and H2 are sealed in a 1.41 L vessel and brought to equilibrium at 600 K. How many grams of CO2 will be present in the equilibrium mixture? CO(g) + H₂O(g) =
1.10 g of an unknown compound reduces the freezing point of 75.22 g benzene from 5.53 to 4.92°C. What is the molar mass of the compound?
6.00 M sulfuric acid, H2SO4(aq), has a density of 1.338 g/mL. What is the percent by mass of sulfuric acid in this solution?
Based on data presented in the text, would you expect diamond or graphite to have the greater density? Explain.
In one type of Breathalyzer (alcohol meter), the quantity of ethanol in a sample is related to the amount of electric current produced by an ethanol–oxygen fuel cell. Use data from Table 19.1 and
Show that for some fuel cells the efficiency value, e = ΔrG°/ΔrH°,can have a value greater than 1.00. Can you identify one such reaction? Use data from Appendix d. TABLE D.1 Ground-State Electron
It is sometimes possible to separate two metal ions through electrolysis. One ion is reduced to the free metal at the cathode, and the other remains in solution. In which of these cases would you
Assume that the volume of each solution in Figure 19-22 is 100.0 mL. The cell is operated as an electrolytic cell, using a current of 0.500 A. Electrolysis is stopped after 10.00 h, and the cell is
You prepare 1.00 L of a buffer solution that is 1.00 M NaH2PO4 and 1.00 M Na2HPO4. The solution is divided in half between the two compartments of an electrolytic cell. Both electrodes used are Pt.
A common reference electrode consists of a silver wire coated with AgCl(s) and immersed in 1 M KCl. (a) What is E°cell when this electrode is a cathode in combination with a standard zinc electrode
The electrodes in the following electrochemical cell are connected to a voltmeter as shown. The half-cell on the right contains a standard silver–silver chloride electrode (see Exercise 88). The
Use data from Table 19.1, as necessary, to predict the probable products when Pt electrodes are used in the electrolysis of (a) CuCl2(aq);(b) Na2SO4(aq);(c) BaCl2(l);(d) KOH(aq).Table 19.1 TABLE
An important source of Ag is recovery as a by-product in the metallurgy of lead. The percentage of Ag in lead was determined as follows. A 1.050-g sample was dissolved in nitric acid to produce
The following voltaic cell registers an Ecell = 0.108 V. What is the pH of the unknown solution? Pt H₂(g, 1 bar) H¹ (x M)||H* (1.00 M)|H₂(g, 1 bar) Pt
For each of the following combinations of electrodes (A and B) and solutions, indicate • The overall cell reaction • The direction in which electrons flow spontaneously (from A to B, or from B
For the reaction Zn(s) + H+(aq) + NO3-(aq) → Zn2+(aq) + H2O(l) + NO(g), describe the voltaic cell in which it occurs, label the anode and cathode, use a table of standard electrode potentials to
Construct a concept map illustrating the relationship between batteries and electrochemical ideas.
Construct a concept map illustrating the principles of electrolysis and its industrial applications.
What is the value of Ecell for the voltaic cell pictured in Figure 19-10 and diagrammed as follows? Pt Fe²+ (0.10 M), Fe³+ (0.20 M)|| Agt (1.0M) Ag(s) Pt wire Anode Fe2+ (0.10 M) Fe3+ (0.20
Add appropriate arrows to Figure 19-4 to show the direction of migration of ions through the electrochemical cell.Figure 19-4 Flow of electrons Anode Zn 1.103 Voltmeter Salt bridge KNO3(aq) 1.00 M
Aluminum metal displaces zinc(II) ion from aqueous solution.(a) Write oxidation and reduction half-cell equations and an overall equation for this redox reaction.(b) Write a cell diagram for a
(A) Write the overall equation for the redox reaction that occurs in the voltaic cell(B) Draw a voltaic cell in which silver ion is displaced from solution by aluminum metal. Label the cathode, the
Two electrochemical cells are connected as shown.(a) Do electrons flow in the direction of the red arrows or the blue arrows?(b) What are the ion concentrations in the half-cells at the point at
The cell diagram for an electrochemical cell is written asWrite the equations for the half-cell reactions that occur at the electrodes. Balance the overall cell reaction. Ni(s)
For Figure 19-6, describe any changes in mass that might be detected at the Pt, Cu, and Zn electrodes as electric current passes through the electrochemical cells.Figure 19-6 H₂(g) 1 bar Pt H+
(A) The cell diagram for an electrochemical cell is written asWrite the equations for the half-cell reactions that occur at the electrodes. Balance the overall cell reaction.(B) The cell diagram for
(A) What is E°cell for the reaction in which Cl2(g) oxidizes Fe2+(aq) to Fe3+(aq)?(B) Use data from Table 19.1 to determine E°cell for the redox reaction in which Fe2+(aq) is oxidized to Fe3+(aq)
A new battery system currently under study for possible use in electric vehicles is the zinc–chlorine battery. The overall reaction producing electricity in this cell is Zn(s) + Cl2(g) →
For the half-cell reaction ClO4-(aq) + 8 H+(aq) + 7 e- → 1/2 Cl2(g) + 4 H2O(l), what are the standard-state conditions for the reactants and products?
Cadmium is found in small quantities wherever zinc is found. Unlike zinc, which in trace amounts is an essential element, cadmium is an environmental poison. To determine cadmium ion concentrations
(A) In acidic solution, dichromate ion oxidizes oxalic acid, H2C2O4(aq), to CO2(g) in a reaction with E°cell = 1.81 V.Use the value of E°cell for this reaction, together with appropriate data from
When two cell reactions with reactants and products in their standard states are compared, one is found to have a negative value of E°cell and the other a positive value. Which cell reaction will
(A) Use electrode potential data to determine ΔG° for the reaction(B) The hydrogen–oxygen fuel cell is a voltaic cell with a cell reaction of 2 H2(g) + O2(g) → 2 H2O(l). Calculate E°cell for
Given that E° = 2.121 V, determine ΔrG° for the reaction Zn(s) + Cl2(g, 1 bar) → ZnCl2(aq, 1 M).
Describe two sets of conditions under which the measured Ecell for a reaction is equal to E°cell.
Will aluminum metal displace Cu2+ ion from aqueous solution? That is, will a spontaneous reaction occur in the forward direction for the following reaction? 2 Al(s) + 3 Cu²+ (1 M) 3 Cu(s) + 2 A1³+
The following cell is set up under standard-state conditions.When sodium sulfate is added to the anode half-cell, formation of a white precipitate is observed, accompanied by a change in the value of
(A) Name one metal ion that Cu(s) will displace from aqueous solution, and determine E°cell for the reaction.(B) When sodium metal is added to seawater, which has [Mg2+] = 0.0512 M, no magnesium
Peroxodisulfate salts, such as Na2S2O8, are oxidizing agents used in bleaching. Dichromates such as K2Cr2O7 have been used as laboratory oxidizing agents. Which is the better oxidizing agent in
Write a cell diagram for a possible voltaic cell in which the cell reaction is Cl-(0.50 M) → Cl-(0.10 M). What would be Ecell for this reaction?
(A) An inexpensive way to produce peroxodisulfates would be to pass O2(g) through an acidic solution containing sulfate ion. Is this method feasible under standard conditions?(B) Consider the
What is the value of the equilibrium constant K for the reaction between copper metal and iron(III) ions in aqueous solution at 25 °C? 3+ Cu(s) + 2 Fe³+ (aq) Cu²+ (aq) + 2 Fe²+ (aq) K = ?
Why do the calomel standard reduction potential and the saturated calomel electrode have different potentials?
(A) Should the displacement of Cu2+ from aqueous solution by Al(s) go to completion? Base your assessment on the value of K for the displacement reaction. We determined E°cell for this reaction in
(A) Calculate Ecell for the following voltaic cell.(B) Calculate Ecell for the following voltaic cell. 2+ Al(s) A1³+ (0.36 M)||Sn4+ (0.086 M), Sn²+ (0.54 M) Pt
Why do dry cells and lead-acid cells “run down” during use? Do you think a fuel cell runs down? Explain.
Will the cell reaction proceed spontaneously as written for the following cell? Ag(s) Ag+ (0.075 M)||Hg2+ (0.85 M) Hg(1)
Of the metals Al, Cu, Ni, and Zn, which could act as a sacrificial anode for iron?
(A) Will the cell reaction proceed spontaneously as written for the following cell?(B) For what ratio of [Ag+]2/[Hg2+] will the cell reaction in Example 19-10 not be spontaneous in either
With the data given for reaction (19.23), calculate Ksp for AgI.Reaction (19.23) AgI(s) Ag+ (aq) + (aq) Ksp = ?
(A) Use data from Table 19.1 to predict the probable products when Pt electrodes are used in the electrolysis of KI(aq).Table 19.1(B) In the electrolysis of AgNO3(aq), what are the expected
(A) Ksp for AgCl = 1.8 x 10-10. What would be the measured Ecell for the voltaic cell in Example 19-11 if the contents of the anode half-cell were saturated AgCl(aq) and AgCl(s)?Example 19-11With the
Refer to Figure 19-23. Predict the electrode reactions and the overall reaction when the anode is made of (a) Copper and (b) Platinum.Figure 19-23 (?)- Battery cass Cu2+ Cu CuSO4(aq) Anode (+)
The electrodeposition of copper can be used to determine the copper content of a sample. The sample is dissolved to produce Cu2+(aq), which is electrolyzed. At the cathode, the reduction half-cell
(A) If 12.3 g of Cu is deposited at the cathode of an electrolytic cell after 5.50 h, what was the current used?(B) For how long would the electrolysis in Example 19-13 have to be carried out, using
For the reaction 2 NO(g) + Cl2(g) ⇌ 2 NOCl(g), the equilibrium constant is Kc = 3.7 x 108 at 25 °C. What are the equilibrium amounts of all gases, at 25 °C, if 0.100 mol each of NO and Cl2 are
Bromoacetic acid, BrCH2COOH, has pKa = 2.902. Calculate the expected values of (a) The freezing point of 0.0500 M BrCH2COOH(aq) and (b) The osmotic pressure at 25 °C of 0.00500 M BrCH2COOH(aq).
Calculate the equilibrium concentration and the percent ionization of HA in 1.00 M HA(aq) at 25 °C, assuming Ka is equal to (a) 1.00 x 105; (b) 1.00 x 10-5.
(A) Sodium fluoride, NaF, is found in some toothpaste formulations as an anticavity agent. What is the pH of 0.10 M NaF(aq)?(B) The pH of an aqueous solution of NaCN is 10.38. What is [CN-] in this
According to the Lewis theory, each of the following is an acid–base reaction. Which species is the acid and which is the base? BF4 (a) BF3 + F- (b) OH(aq) + CO₂(aq) HCO3(aq)
(A) The solubility of CO2(g) in H2O at 25 °C and under a CO2(g) pressure of 1 atm is 1.45 g CO2/L. Air contains 0.037% CO2 by volume. Use this information, together with data from Table 16.5, to
The structural formula shown is para-hydroxybenzoic acid, a weak diprotic acid used as a food preservative. Titration of 25.00 mL of a dilute aqueous solution of this acid requires 16.24 mL of 0.0200
(1) Given that an indicator is itself a weak acid or base, why does adding it to a solution not change the nature of the equilibrium?(2) Starting with about 10 mL of dilute NaCl(aq) containing a
What are the effects on the pH of adding (a) 0.0060 mol HCl and (b) 0.0060 mol NaOH to 0.300 L of a buffer solution that is 0.250 M CH3COOH and 0.560 M NaCH3COO?
What is the pH at each of the following points in the titration of 25.00 mL of 0.100 M HCl with 0.100 M NaOH?(a) Before the addition of any NaOH (initial pH)(b) After the addition of 24.00 mL 0.100 M
What is the pH at each of the following points in the titration of 25.00 mL of 0.100 M CH3COOH with 0.100 M NaOH?(a) Before the addition of any NaOH (initial pH)(b) After the addition of 10.00 mL
Sodium phosphate, Na3PO4, is an ingredient of some preparations used to clean painted walls before they are repainted. What is the pH of 0.025 M Na3PO4(aq)?
A large excess of MgF2(s) is maintained in contact with 1.00 L of pure water to produce a saturated solution of MgF2. When an additional 1.00 L of pure water is added to the mixture and equilibrium
Write the solubility product constant expression for the solubility equilibrium of (a) Calcium fluoride, CaF2 (one of the substances used when a fluoride treatment is applied to teeth).(b) Copper
Lime (quicklime), CaO, is obtained from the high-temperature decomposition of limestone (CaCO3). Quicklime is the cheapest source of basic substances, but it is water insoluble. It does react with
(A) Write the solubility product constant expression for (a) MgCO3 (one of the components of dolomite, a form of limestone) and (b) Ag3PO4 (used in photographic emulsions).(B) A handbook lists Ksp
Of the compounds CaF2, CaCl2, AgF, and AgCl, which would be considered insoluble? Explain.
A handbook lists the aqueous solubility of CaSO4 at 25 °C as 0.20 g CaSO4/100 mL. What is the Ksp of CaSO4 at 25 °C? CaSO4(s) = Ca²+ (aq) + SO4² (aq) Ksp ?
(A) A handbook lists the aqueous solubility of AgOCN as 7 mg/100 mL at 20 °C. What is the Ksp of AgOCN at 20 °C?(B) A handbook lists the aqueous solubility of lithium phosphate at 18 °C as 0.034
In the fractional precipitation pictured in Figure 18-4 and described in Example 18-7, no mention was made of the concentration of the AgNO3(aq) used. Is this concentration immaterial? Explain.Figure
Lead(II) iodide, PbI2, is a dense, golden yellow, “insoluble” solid used in bronzing and in ornamental work requiring a golden color (such as mosaic gold). Calculate the molar solubility of
(A) The Ksp of Cu3(AsO4)2 at 25 °C is 7.6 x 10-36. What is the molar solubility of Cu3(AsO4)2 in H2O at 25 °C?(B) How many milligrams of BaSO4 are dissolved in a 225 mL sample of saturated
Which will be affected more by the addition of a strong acid or a strong base: the solubility of CaF2 or the solubility of CaCl2? Explain.
What is the molar solubility of PbI2 in 0.10 M KI(aq)?

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