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Questions and Answers of Chemical Principles

Write balanced half-reactions and devise a galvanic cell (write a cell diagram) to study each of the following reactions: (a) Pb(NO3)2(aq) + K₂SO4(aq) → PbSO4(s) + 2 KNO3(aq), a precipitation
Calculate the molar solubility of each substance in its respective solution:(a) Silver iodide in 0.020 m NaI(aq);(b) Calcium carbonate in 2.3 * 10–4 m Na2CO3(aq);(c) Lead(II) fluoride in 0.21 m
Use data from Tables 6C.1 and 6C.2 to place the following acids in order of increasing strength: HCOOH, (CH3)3NH+, N2H5+, HF. TABLE 6C.1 Acidity Constants at 25 C* K 3.0 X 10-1 2.0 X 10- 1.7 X 10-1
The pH of several solutions was measured in a hospital laboratory; convert each of the following pH values into the molar concentration of H3O+ ions:(a) 4.8 (the pH of a urine sample);(b) 0.7 (the
Many reactions that take place in water have analogous reactions in liquid ammonia (normal boiling point, –33°C).(a) Write the chemical equation for the autoprotolysis of NH3.(b) Write the
Below are molecular models of two oxoacids. Write the name of each acid and then draw the model of its conjugate base.(Red = O, white = H, green = Cl, and blue = N.) (a) (b)
Arrange the following species in order of increasing strength as oxidizing agents for species in aqueous solution:(a) Co2+, Cl2, Ce4+, In3+;(b) NO3 –, ClO4 –, HBrO, Cr2O7 2–, all in acidic
Like sulfuric acid, a certain diprotic acid, H2A, is a strong acid in its first deprotonation and a weak acid in its second deprotonation. A solution that is 0.015 m H2A(aq) has a pH of 1.72. What is
Suppose that 1.773 g of impure barium hydroxide is dissolved in enough water to produce 200. mL of solution and that 25.0 mL of this solution is titrated to the stoichiometric point with 13.1 mL of
Calculate the unknown concentration of the ion in each of the following cells: 2+ (a) Pb(s) Pb²+ (aq, ?)||Pb²+ (aq, 0.10 mol-L-¹) Pb(s), Ecell = +0.083 V. (b) Pt(s)| Fe³+ (aq, 0.10 mol-L-¹),
Calculate the pH and pOH of(a) A solution that is 0.23 m Na2HPO4(aq) and 0.18 m Na3PO4(aq);(b) A solution that is 0.45 m Na2HPO4(aq) and 0.62 m Na3PO4(aq);(c) A solution that is 0.16 m Na2HPO4(aq)
For the exercise in this topic, base your answers on the potentials listed in Table 6M.1 or Appendix 2B, with the exception of the reduction and oxidation of water at pH = 7:(a) What current is
Find the initial concentration of the weak acid or base in each of the following aqueous solutions:(a) A solution of HClO with pH = 5.4;(b) A solution of pyridine, C5H5N, with pH = 8.8.
(a) Calculate the pH of 8.50 * 10–5 m and 7.37 * 10–6 m HCN(aq), ignoring the effect of the autoprotolysis of water.(b) Repeat the calculations, taking into account the autoprotolysis of water.
You wish to separate magnesium ions and barium ions by selective precipitation. Which anion, fluoride or carbonate, would be the better choice for achieving this precipitation? Why?
(a) Write balanced half-reactions for the redox reaction of an acidified solution of potassium permanganate and iron(II) chloride.(b) Write the balanced equation for the cell reaction and devise a
(a) Complete the following table.(b) Rank the four solutions in order of increasing acidity. [H3O+] (i) 1.50 mol-L-¹ (ii) (iii) (iv) [OH-] 1.50 mol-L-¹ PH 0.75 POH 0.75
Calculate the molar solubility of each of the following sparingly soluble substances in its respective solution: aluminum hydroxide at(a) pH = 7.0;(b) pH = 4.5; zinc hydroxide at(c) pH =
You continue exploring different combinations of electrodes in pursuit of better batteries. You know that the Ce4+/Ce3+ couple has been used in combination with Zn2+/Zn to develop new power sources
Which of the following can be classified as reactions between Brønsted acids and bases? For those that can be so classified, identify the acid and the base. (a) NHI(aq) + H,O(l)→NH,(aq) + HgO*(aq)
You are an environmental chemist studying a local waterway and need to know the amounts of all forms of phosphate in the stream. You might begin by making up some solutions of phosphoric acid to use
Acetic acid is used as a solvent for some reactions between acids and bases.(a) Nitrous acid and carbonic acids are both weak acids in water. Will either of them act as a strong acid in acetic acid?
The images below represent the solutes in the solutions of three salts (water molecules are not shown, hydrogen atoms and hydronium ions are represented by small gray spheres, hydroxide ions by red
If you are working in a research laboratory preparing a series of compounds, you might be faced with having to make a choice between acids based on their strengths. Can you decide which to use based
You continue to use the buffer that you prepared in Example 6G.1 but are worried about how adding sodium hydroxide to the buffer solution will affect the pH, which could upset your experiment.
A student was given a standard Fe(s)|Fe2+(aq) half-cell and another half-cell containing an unknown metal M in 1.00 m MNO3(aq) and formed the cell M(s)|M+(aq)||Fe2+(aq)|Fe(s). At 25°C, Ecell = 11.24
Although there are extensive tables available for the pKa of weak acids, you might be dealing with an unknown acid or a known acid at an unlisted temperature. You could then use a procedure like this
Write the formulas of the conjugate acids of(a) C2O4 2–, the oxalate ion;(b) C6H5NH2, aniline;(c) NH2OH, hydroxylamine; and the conjugate bases of(d) H2O2, hydrogen
Calculate the pH of 0.010 m H2SeO4(aq), given that Ka1 is very large and Ka2 = 1.2 * 10–2.
As in Example 6L.1, you are planning to use a Daniell cell to power a model electric car. However, you find that you do not have standard solutions available. You have only dilute solutions, and you
Explain what happens to(a) The pH of a solution of phosphoric acid after the addition of solid sodium dihydrogen phosphate;(b) The percentage deprotonation of HCN in a hydrocyanic acid solution
Write(a) The chemical equation for the proton transfer equilibrium in water and the corresponding expression for Kb and(b) The chemical equation for the proton transfer equilibrium of the conjugate
(a) Sketch the titration curve for the titration of 5.00 mL 0.010 m HCl(aq) with 0.010 m Ca(OH)2(aq), indicating the pH of the initial and final solutions and the pH at the stoichiometric point.
Calculate the equilibrium constants for the following reactions: 2+ (a) 2 Fe³+ (aq) + H₂(g) 2 Fe²+ (aq) + 2 H+(aq) (b) 2 Cr(s) + O₂(g) + 2 H₂O(l) — 2 Cr²+ (aq) + 4 OH (aq)
Barium hydroxide is a base that is sometimes used for titrating acids. When using it, you need to know the actual concentration of hydroxide ion in the solution. What are the molar concentrations of
You have a sample of seawater collected off Hawaii, where there is a lot of volcanic activity. As part of an oceanographic study, you are going to analyze it to see if its composition is markedly
Wine is a complex mixture of over 1000 compounds, many at very low concentrations. A large number of flavorful components are derivatives of phenol, C6H5OH, a weak acid. If you are an enologist
You are working in a plant that produces copper for use in electrical circuits by electrolysis of acidic solutions of CuSO4(aq). A customer has placed an order for a small quantity of high-purity
Muscles produce lactic acid during exercise. Calculate the pH, pOH, and percentage deprotonation of the following aqueous solutions of lactic acid, CH3CH(OH)COOH:(a) 0.11 m;(b) 3.7 * 10–3
As a part of your research program on formic acid, you need to titrate a solution of formic acid with sodium hydroxide solution and want to know what to expect. Calculate the pH of(a) 0.100 m
Balance each of the following skeletal equations by using oxidation and reduction half-reactions. All the reactions take place in acidic solution. Identify the oxidizing agent and reducing agent in
Calculate the pH of 6.50 * 10–8 m HBr(aq).
Iodide ions can be used to precipitate lead(II) ions from 0.010 m Pb(NO3)2(aq).(a) What minimum iodide ion concentration is required for the onset of PbI2 precipitation?(b) What mass (in grams) of
For the exercise in this topic, base your answers on the potentials listed in Table 6M.1 or Appendix 2B, with the exception of the reduction and oxidation of water at pH = 7:Aqueous solutions of (a)
You know that silver chloride is not very soluble in water, but what do you know about its solubility in seawater? You decide to investigate the solubility of silver chloride in solutions with
The concentration of CrO4 2– in a saturated Tl2CrO4 solution is 6.3 * 10–5 mol · L–1. What is the Ksp of Tl2CrO4?
Write the half-reactions and the balanced equation for the cell reaction for each of the following galvanic cells: (a) Ni(s) Ni²+ (aq)|| Ag+(aq) Ag(s) (b) C(gr) |H₂(g)
A careless laboratory technician wants to prepare 200.0 mL of a 0.025 m HCl(aq) solution but uses a volumetric flask of volume 250.0 mL by mistake.(a) What would the pH of the desired solution have
Estimate the enthalpy of deprotonation of formic acid at 25°C, given that Ka = 1.765 * 10–4 at 20°C and 1.768 * 10–4 at 30°C.
Predict the standard potential of each of the following galvanic cells: 3+ (a) Pt(s) Cr³+ (aq), Cr²+ (aq)||Cu²+ (aq) |Cu(s) (b) Ag(s) AgI(s) I (aq)||CI (aq)|AgCl(s) Ag(s) (c) Hg(1) Hg₂Cl₂ (s)
Carbonate and hydrogen carbonate (bicarbonate) ions contribute to buffering in a variety of natural systems. You are investigating their role in groundwater percolating through limestone hills into a
Write the chemical equations for the proton transfer equilibria of the following acids in aqueous solution and identify the conjugate acid–base pairs in each case:(a) H2SO4;(b) C6H5NH3 +,
Methylamine, CH3NH2, is a weak base used as a building block for some pharmaceuticals. If you prepare an aqueous solution of methylamine for use in a synthesis, you might need to know its pH to avoid
Calculate the pH of each of the following solutions of diprotic acids at 25°C, ignoring second deprotonations only when the approximation is justified:(a) 0.010 m H2CO3(aq);(b) 0.10 m
A solution of equal molar concentrations of glyceric acid and sodium glycerate was found to have pH = 3.52.(a) What are pKa and Ka for glyceric acid?(b) What would the pH be if the concentration of
(a) Give the Ka value of each of the following acids:(i) Phosphoric acid, H3PO4, pKa = 2.12; (ii) Phosphorous acid, H3PO3, pKa = 2.00; (iii) Selenous acid, H2SeO3, pKa = 2.46; (iv) Hydrogen
Predict the potential of each of the following cells: (a) Pt(s) H₂(g, 1.0 bar) |HCl(aq, 0.075 mol-L¯¹)||HCl(aq, 1.0 mol-L¯¹)| H₂(g, 1.0 bar) |Pt(s) (b) Zn(s) Zn²+ (aq, 0.37 mol·L¹) ||Ni²+
Calculate the volume of 0.150 m HCl(aq) required to neutralize(a) one-half and(b) all the hydroxide ions in 25.0 mL of 0.110 m NaOH(aq).(c) What is the molar concentration of Na+ ions at the
Measurement of ion concentrations with electrodes is used in a wide range of applications. Suppose you are interested in removing silver ions from exhausted electroplating solutions by precipitating
Balance each of the following skeletal equations by using oxidation and reduction half-reactions. All the reactions take place in acidic solution. Identify the oxidizing agent and reducing agent in
(a) When the pH of 0.10 m HClO2(aq) was measured, it was found to be 1.2. What are the values of Ka and pKa of chlorous acid?(b) The pH of a 0.10 m propylamine, C3H7NH2, aqueous solution was
For the exercise in this topic, base your answers on the potentials listed in Table 6M.1 or Appendix 2B, with the exception of the reduction and oxidation of water at pH = 7:The anode of an
Calculate the pH of 9.78 * 10–8 m KOH(aq).
Estimate the pH required for the onset of precipitation of Ni(OH)2 from(a) 0.060 m NiSO4(aq);(b) 0.030 m NiSO4(aq).
Silver emulsion photographic film is now largely obsolete for amateur photography, but it is still used in a variety of medical and technical applications. You are working on the improvement of a
Write the half-reactions and the balanced equation for the cell reaction for each of the following galvanic cells: 2+ (a) Zn(s) Zn²+ (aq)|| Au³+ (aq)| Au(s) 3+ (b) Fe(s) | Fe²+ (aq) || Fe³+ (aq)
The molar solubility of silver sulfite, Ag2SO3, is 1.55 * 10–5 mol · L–1. What is the Ksp of silver sulfite?
Predict the standard potential of each of the following galvanic cells: 3+ (a) Pt(s)| Fe³+ (aq), Fe²+ (aq)||Ag* (aq) Ag(s) (b) U(s) U³+ aq||V²+ (aq) V(s) 2+ (c) Sn(s) Sn²+ (aq)||Sn4+ (aq),Sn²+
A careless laboratory technician prepares 300.0 mL of 0.0175 m KOH(aq) and pipets 25.0 mL of the solution into a beaker.The beaker is allowed to stand in a warm place for two days before use, during
How many hydronium ions are present at any moment in 100. mL of pure water at 25°C?
You are working in the emergency room of a hospital where a patient suffering from influenza has developed metabolic alkalosis, a condition in which the pH of the blood is too high. You have
Write the chemical equations for the proton transfer equilibria of the following bases in aqueous solution and identify the conjugate acid–base pairs in each case:(a) CN–;(b) NH2NH2,
Calculate the pH of each of the following solutions of diprotic acids at 25°C, ignoring second deprotonations only when that approximation is justified:(a) 0.10 m H2S(aq);(b) 0.15 m H2C4H4O6(aq),
solution of equal molar concentrations of the artificial sweetener saccharin and its sodium salt was found to have pH = 3.08.(a) What are the values of pKa and Ka of saccharin?(b) What would the pH
(a) Give the pKb values of the following bases: (i) Ammonia, NH3, Kb = 1.8 * 10–5; (ii) Deuterated ammonia, ND3, Kb = 1.1 * 10–5; (iii) Hydrazine, NH2NH2, Kb = 1.7 * 10–6; (iv)
Calculate the volume of 0.120 m HCl(aq) required to neutralize(a) One-half and(b) All the hydroxide ions in 25.0 mL of 0.412 m KOH(aq).(c) What is the molar concentration of Cl– ions at the
Predict the potential of each of the following cells: 3+ (a) Cr(s) Cr³+ (aq, 0.37 mol-L-¹)||Pb²+ (aq, 9.5 10³ mol-L-¹) Pb(s) (b) Pt(s) H₂(g, 2.0 bar) |H* (pH = 3.5)||Cl¯(aq, 0.75
(a) The pH of 0.015 m HNO2(aq) was measured as 2.63. What are the values of Ka and pKa of nitrous acid?(b) The pH of 0.10 m C4H9NH2(aq), butylamine, was measured as 12.04. What are the values of Kb
For the exercise in this topic, base your answers on the potentials listed in Table 6M.1 or Appendix 2B, with the exception of the reduction and oxidation of water at pH = 7:A total charge of 4.5 kC
Balance each of the following skeletal equations by using oxidation and reduction half-reactions. All the reactions take place in basic solution. Identify the oxidizing agent and reducing agent in
Calculate the pH of 8.23 * 10–7 m NaNH2(aq)
Decide whether a precipitate will form when each of the following pairs of solutions are mixed:(a) 5.0 mL of 0.10 m K2CO3(aq) and 1.00 L of 0.010 m AgNO3(aq);(b) 3.3 mL of 1.0 m HCl(aq), 4.9 mL of
Write the half-reactions, the balanced equation for the cell reaction, and the cell diagram for each of the following skeletal equations: (a) Ni²+(aq) + Zn (s) → Ni(s) + Zn²+(aq) Ce4+ (b) Ce¹¹
For each reaction that is spontaneous under standard conditions (that is, K > 1), write a cell diagram, determine the standard cell potential, and calculate ΔG° for the reaction: (a) 2 NO3 (aq)
Calculate the molar solubility in water of(a) BiI3 (Ksp = 7.71 * 10–19);(b) CuCl;(c) CaCO3.
Hydrogen peroxide, H2O2, reacts with sulfur trioxide to form peroxomonosulfuric acid, H2SO5, in a Lewis acid–base reaction.(a) Write the chemical equation for the reaction.(b) Draw the Lewis
Calculate the pH and pOH of each of the following aqueous solutions of a strong acid or base: (a) 0.0146 m HNO3(aq); (b) 0.11 m HCl(aq); (c) 0.0092 m Ba(OH)2(aq); (d) 2.00 mL of 0.175 m KOH(aq)
Use data from Tables 6C.1 and 6C.2 to place the following bases in order of increasing strength: F–, NH3, CH3CO2–, C5H5N (pyridine). TABLE 6C.1 Acidity Constants at 25 °C* K₂ 3.0 X 10-1 2.0 X
Use the data in Appendix 2B to calculate E°(U4+/U). 2B STANDARD POTENTIALS AT 25 °C Potentials in Electrochemical Order Reduction half-reaction Strongly oxidizing H4XeO6 + 2 H+ 2 e → XeO3 + 3
Calculate the molar concentrations of H2CO3, HCO3–, CO32–, H3O+, and OH– present in 0.0456 m H2CO3(aq).
Benzoic acid, C6H5COOH, is used as a preservative in food and cosmetics because it is considered to be relatively safe.Suppose you are studying benzoic acid and need to predict the pH of a benzoic
Calculate the pH of the solution that results from mixing(a) 30.0 mL of 0.050 m HCN(aq) with 70.0 mL of 0.030 m NaCN(aq);(b) 40.0 mL of 0.030 m HCN(aq) with 60.0 mL of 0.050 m NaCN(aq);(c) 25.0 mL
A tin electrode in 0.015 m Sn(NO3)2(aq) is connected to a hydrogen electrode in which the pressure of H2 is 1.0 bar. If the cell potential is 0.061 V at 25°C, what is the pH of the electrolyte at
For the exercise in this topic, base your answers on the potentials listed in Table 6M.1 or Appendix 2B, with the exception of the reduction and oxidation of water at pH = 7:(a) When a current of
The percentage deprotonation of benzoic acid in a 0.110 m solution is 2.4%. What is the pH of the solution and the Ka of benzoic acid?
(a) Calculate the pH of 1.89 * 10–5 m and 9.64 * 10–7 m HClO(aq), ignoring the effect of the autoprotolysis of water.(b) Repeat the calculations, taking into account the autoprotolysis of water.
You wish to separate barium ions from calcium ions by selective precipitation. Which anion, fluoride or carbonate, would be the better choice for achieving this precipitation? Why?
Decide on the basis of the information in Table 6C.3 whether carbonic acid is a strong or weak acid in liquid ammonia solvent. Explain your answer. TABLE 6C.3 Conjugate Acid-Base Pairs Arranged by
(a) Complete the following table.(b) Rank the four solutions in order of increasing acidity. [H3O+] (i) 0.50 mol-L-¹ (ii) (iii) (iv) [OH-] -1 0.50 mol-L-¹ pH -0.10 POH -0.10
(a) Write balanced half-reactions for the redox reaction between sodium perchlorate and copper (I) nitrate in an acidic solution.(b) Write the balanced equation for the cell reaction and devise a

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