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engineering
the science and engineering of materials
Chemistry 10th Edition Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste - Solutions
If a solution contains either Pb2+(aq) or Ag+(aq), how can temperature be manipulated to help identify the ion in solution?
Write balanced equations for the dissolution reactions and the corresponding solubility product expressions for each of the following solids. a. Ag2CO3b. Ce(IO3)3c. BaF2
Approximately 0.14 g nickel(II) hydroxide, Ni(OH)2(s), dissolves per liter of water at 20οC. Calculate Ksp for Ni(OH)2(s) at this temperature.
The concentration of Pb2+ in a solution saturated with PbBr2(s) is 2.14 × 10-2 M. Calculate Ksp for PbBr2.
Cream of tartar, a common ingredient in cooking, is the common name for potassium bitartrate (abbreviated KBT, molar mass = 188.2 g/mol). Historically, KBT was a crystalline solid that formed on the casks of wine barrels during the fermentation process. Calculate the maximum mass of KBT that can
Barium sulfate is a contrast agent for X-ray scans that are most often associated with the gastrointestinal tract. Calculate the mass of BaSO4 that can dissolve in 100.0 mL of solution. The Ksp value for BaSO4 is 1.5 × 10-9.
Calculate the molar solubility of Co(OH)3, Ksp = 2. × 3 10-43.
Calculate the solubility of solid Ca3(PO4)2 (Ksp = 1.3 × 10-32) in a 0.20-M Na3PO4 solution.
Calculate the solubility of solid Pb3(PO4)2 (Ksp = 1 × 10-54) in a 0.10-M Pb(NO3)2 solution.
The solubility of Pb(IO3)2(s) in a 0.10-M KIO3 solution is 2.6 × 10-11 mol/L. Calculate Ksp for Pb(IO3)2.
Will a precipitate form when 100.0 mL of 4.0 × 10-4 M Mg(NO3)2 is added to 100.0 mL of 2.0 × 10-4 M NaOH?
If 10.0 mL of 2.0 × 10–3 M Cr(NO3)3 is added to 10.0 mL of a pH = 10.0 NaOH solution, will a precipitate form?
A solution is formed by mixing 50.0 mL of 10.0 M NaX with 50.0 mL of 2.0 × 10-3 M CuNO3. Assume that Cu+ forms complex ions with X- as follows:with an overall reaction Calculate the following concentrations at equilibrium. a. CuX32-b. CuX2-c. Cu+ Cu (aq) + CuX(aq) + X(aq) CuX₂ (aq) +
A solution contains 1.0 × 10-5 M Na3PO4. What concentrations of AgNO3 will cause precipitation of solid Ag3PO4 (Ksp = 1.8 × 10-18)?
A solution contains 3.0 × 10–3 M Mg(NO3)2. What concentrations of KF will cause precipitation of solid MgF2 (Ksp = 6.4 × 10–9)?
A solution contains 0.25 M Ni(NO3)2 and 0.25 M Cu(NO3)2. Can the metal ions be separated by slowly adding Na2CO3? Assume that for successful separation 99% of the metal ion must be precipitated before the other metal ion begins to precipitate, and assume no volume change on addition of Na2CO3.
Write equations for the stepwise formation of each of the following complex ions. a. CoF63-b. Zn(NH3)42+
As sodium chloride solution is added to a solution of silver nitrate, a white precipitate forms. Ammonia is added to the mixture and the precipitate dissolves. When potassium bromide solution is then added, a pale yellow precipitate appears. When a solution of sodium thiosulfate is added, the
The solubility of copper(II) hydroxide in water can be increased by adding either the base NH3 or the acid HNO3. Explain. Would added NH3 or HNO3 have the same effect on the solubility of silver acetate or silver chloride? Explain.
Calculate the equilibrium concentrations of NH3, Cu2+, Cu(NH3)2+, Cu(NH3)22+, Cu(NH3)32+, and Cu(NH3)42+ in a solution prepared by mixing 500.0 mL of 3.00 M NH3 with 500.0 mL of 2.00 × 10-3 M Cu(NO3)2. The stepwise equilibria are Cu²+ (aq) + NH3(aq) CUNH3²+ (aq) + NH3(aq) —Cu(NH3)₂²+
The Ksp of Al(OH)3 is 2 × 10-32. At what pH will a 0.2-M Al3+ solution begin to show precipitation of Al(OH)3?
On a hot day, a 200.0-mL sample of a saturated solution of PbI2 was allowed to evaporate until dry. If 240 mg of solid PbI2 was collected after evaporation was complete, calculate the Ksp value for PbI2 on this hot day.
Consider saturated solutions of the following compounds: a. AgOHb. Cd(OH)2c. Pb(OH)2Calculate the pH of each saturated solution.
Assuming that the solubility of Ca3(PO4)2(s) is 1.6 × 10-7 mol/L at 25οC, calculate the Ksp for this salt. Ignore any potential reactions of the ions with water.
The Ksp for PbI2(s) is 1.4 × 10-8. Calculate the solubility of PbI2(s) in 0.048 M NaI.
The salt MX has a solubility of 3.17 × 10–8 mol/L in a solution with pH = 0.000. If Ka for HX is 1.00 × 10–15, calculate the Ksp value for MX.
A solution saturated with a salt of the type M3X2 has an osmotic pressure of 2.64 × 10-2 atm at 25οC. Calculate the Ksp value for the salt, assuming ideal behavior.
Aluminum ions react with the hydroxide ion to form the precipitate Al(OH)3(s), but can also react to form the soluble complex ion Al(OH)4-. In terms of solubility, Al(OH)3(s) will be more soluble in very acidic solutions as well as more soluble in very basic solutions.a. Write equations for the
An aqueous solution contains a mixture of 0.0500 M HCOOH (Ka = 1.77 × 10-4) and 0.150 M CH3CH2COOH (Ka = 1.34 × 10-5). Calculate the pH of this solution. Because both acids are of comparable strength, the H+ contribution from both acids must be considered.
A 2.14-g sample of sodium hypoiodite is dissolved in water to make 1.25 L of solution. The solution pH is 11.32. What is Kb for the hypoiodite ion?
Calculate the mass of sodium hydroxide that must be added to 1.00 L of 1.00-M HC2H3O2 to double the pH of the solution (assume that the added NaOH does not change the volume of the solution).
Consider 1000. mL of a 1.00 × 10-4-M solution of a certain acid HA that has a Ka value equal to 1.00 × 10-4. How much water was added or removed (by evaporation) so that a solution remains in which 25.0% of HA is dissociated at equilibrium? Assume that HA is nonvolatile.
What mass of NaOH(s) must be added to 1.0 L of 0.050 M NH3 to ensure that the percent ionization of NH3 is no greater than 0.0010%? Assume no volume change on addition of NaOH.
Making use of the assumptions we ordinarily make in calculating the pH of an aqueous solution of a weak acid, calculate the pH of a 1.0 × 10-6 -M solution of hypobromous acid (HBrO, Ka = 2 × 10-9). What is wrong with your answer? Why is it wrong? Without trying to solve the problem, explain what
Consider 50.0 mL of a solution of weak acid HA (Ka = 1.00 × 10-6), which has a pH of 4.000. What volume of water must be added to make the pH = 5.000?
Calculate [OH-] in a 3.0 × 10-7 -M solution of Ca(OH)2.
Calculate the pH of a 1.0 × 10-7 -M solution of NaOH in water.
Complete the table for each of the following solutions: 0.0070 M HNO3 3.0 M KOH [H+] PH РОН [OH-]
Consider 0.10 M solutions of the following compounds: AlCl3, NaCN, KOH, CsClO4, and NaF. Place these solutions in order of increasing pH.
Consider 0.25 M solutions of the following salts: NaCl, RbOCl, KI, Ba(ClO4)2, and NH4NO3. For each salt, indicate whether the solution is acidic, basic, or neutral.
Rank the following 0.10 M solutions in order of increasing pH. a. NH3b. KOHc. HC2H3O2d. KCle. HCl
For solutions of the same concentration, as acid strength increases, indicate what happens to each of the following (increases, decreases, or doesn’t change). a. [H+]b. pHc. [OH-]d. pOHe. Ka
Phosphoric acid is a common ingredient in traditional cola drinks. It is added to provide the drinks with a pleasant tart taste. Assuming that in cola drinks the concentration of phosphoric acid is 0.007 M, calculate the pH of this solution.
When determining the pH of a weak acid solution, sometimes the 5% rule can be applied to simplify the math. At what Ka values will a 1.0-M solution of a weak acid follow the 5% rule?
A solution is tested for pH and conductivity as pictured below: The solution contains one of the following substances: HCl, NaOH, NH4Cl, HCN, NH3, HF, or NaCN. If the solute concentration is about 1.0 M, what is the identity of the solute? 4.6
Calculate the pH of a 0.010-M solution of iodic acid (HIO3, Ka = 0.17).
Use the Lewis acid–base model to explain the following reaction. CO₂(g) + H₂O(1) H₂CO3(aq)
Is an aqueous solution of NaHSO4 acidic, basic, or neutral? What reaction occurs with water? Calculate the pH of a 0.10-M solution of NaHSO4.
Rank the following 0.10 M solutions in order of increasing pH. a. HI, HF, NaF, NaIb. NH4Br, HBr, KBr, NH3c. C6H5NH3NO3, NaNO3, NaOH, HOC6H5, KOC6H5, C6H5NH2, HNO3
Calculate the mass of HONH2 required to dissolve in enough water to make 250.0 mL of solution having a pH of 10.00 (Kb = 1.1 × 10–8).
At 25οC, a saturated solution of benzoic acid (Ka = 6.4 × 10-5 ) has a pH of 2.80. Calculate the water solubility of benzoic acid in moles per liter.
When someone hyperventilates, a condition known as respiratory alkalosis can occur. Explain the cause and effect of respiratory alkalosis.
Which of the following represent conjugate acid–base pairs? For those pairs that are not conjugates, write the correct conjugate acid or base for each species in the pair a. H2O, OH-b. H2SO4, SO42-c. H3PO4, H2PO4-d. HC2H3O2, C2H3O2-
Would you expect Fe3+ or Fe2+ to be the stronger Lewis acid? Explain.
Zinc hydroxide is an amphoteric substance. Write equations that describe Zn(OH)2 acting as a Brønsted–Lowry base toward H+ and as a Lewis acid toward OH-.
Aluminum hydroxide is an amphoteric substance. It can act as either a Brønsted–Lowry base or a Lewis acid. Write a reaction showing Al(OH)3 acting as a base toward H+ and as an acid toward OH-.
Will the following oxides give acidic, basic, or neutral solutions when dissolved in water? Write reactions to justify your answers.a. Li2Ob. CO2c. SrO
Will the following oxides give acidic, basic, or neutral solutions when dissolved in water? Write reactions to justify your answers.a. CaOb. SO2c. Cl2O
Place the species in each of the following groups in order of increasing acid strength. Explain the order you chose for each group. a. HIO3, HBrO3b. HNO2, HNO3c. HOCl, HOId. H3PO4, H3PO3
Calculate the pH of a 0.050-M Al(NO3)3 solution. The Ka value for Al(H2O)63+ is 1.4 × 10-5 .
Sodium azide (NaN3) is sometimes added to water to kill bacteria. Calculate the concentration of all species in a 0.010-M solution of NaN3. The Ka value for hydrazoic acid (HN3) is 1.9 × 10-5.
Arrange the following 0.10 M solutions in order of most acidic to most basic. KOH, KNO3, KCN, NHẠCH, HC1
A 0.050-M solution of the salt NaB has a pH of 9.00. Calculate the pH of a 0.010-M solution of HB.
An unknown salt is either NaCN, NaC2H3O2, NaF, NaCl, or NaOCl. When 0.100 mole of the salt is dissolved in 1.00 L of solution, the pH of the solution is 8.07. What is the identity of the salt?
Calculate [CO32-] in a 0.010-M solution of CO2 in water (usually written as H2CO3). If all the CO32- in this solution comes from the reactionwhat percentage of the H+ ions in the solution is a result of the dissociation of HCO3-? When acid is added to a solution of sodium hydrogen carbonate
Calculate the pH of each of the following solutions.a. 0.12 M KNO2b. 0.45 M NaOClc. 0.40 M NH4ClO4
Calculate the pH of each of the following solutions.a. 0.10 M CH3NH3Clb. 0.050 M NaCN
Calculate the concentrations of all species present in a 0.25-M solution of ethylammonium chloride (C2H5NH3Cl).
Determine [OH-], [H+], and the pH of each of the following solutions.a. 1.0 M KClb. 1.0 M KC2H3O2
Given that the Ka value for acetic acid is 1.8 × 10-5 and the Ka value for hypochlorous acid is 3.5 × 10-8, which is the stronger base, OCl- or C2H3O2-?
Calculate the pH of a 5.0 × 10-3 -M solution of H2SO4.
Calculate the pH of a 2.0-M H2SO4 solution.
A typical vitamin C tablet (containing pure ascorbic acid, H2C6H6O6) weighs 500. mg. One vitamin C tablet is dissolved in enough water to make 200.0 mL of solution. Calculate the pH of this solution. Ascorbic acid is a diprotic acid.
Write out the stepwise Ka reactions for the diprotic acid H2SO3.
Codeine (C18H21NO3) is a derivative of morphine that is used as an analgesic, narcotic, or antitussive. It was once commonly used in cough syrups but is now available only by prescription because of its addictive properties. If the pH of a 1.7 × 10-3 -M solution of codeine is 9.59, calculate Kb.
The pH of a 0.016-M aqueous solution of p-toluidine (CH3C6H4NH2) is 8.60. Calculate Kb.
What is the percent ionization in each of the following solutions?a. 0.10 M NH3b. 0.010 M NH3c. 0.10 M CH3NH2
Calculate the pH of a 0.050-M (C2H5)2NH solution (Kb = 1.3 × 10-3).
Calculate the pH of a 0.20-M C2H5NH2 solution (Kb = 5.6 × 10-4).
Trimethylamine, (CH3)3N, is produced when plants and animals decompose and has a very unpleasant odor. Calculate the [OH–], [H+], and pH of a 0.40-M solution of (CH3)3N (Kb = 7.4 × 10–5).
What are the major species present in a 0.150-M NH3 solution? Calculate the [OH-] and the pH of this solution.
What mass of KOH is necessary to prepare 800.0 mL of a solution having a pH = 11.56?
What are the major species present in the following mixtures of bases?a. 0.050 M NaOH and 0.050 M LiOHb. 0.0010 M Ca(OH)2 and 0.020 M RbOHWhat is [OH-] and the pH of each of these solutions?
What are the major species present in 0.015 M solutions of each of the following bases?a. KOHb. Ba(OH)2What is [OH-] and the pH of each of these solutions?
Calculate [OH-], pOH, and pH for each of the following.a. 0.00040 M Ca(OH)2b. A solution containing 25 g KOH per literc. A solution containing 150.0 g NaOH per liter
Calculate the pH of the following solutions.a. 0.10 M NaOHb. 1.0 × 10-10 M NaOHc. 2.0 M NaOH
One mole of a weak acid HA was dissolved in 2.0 L of solution. After the system had come to equilibrium, the concentration of HA was found to be 0.45 M. Calculate Ka for HA.
A typical sample of vinegar has a pH of 3.0. Assuming that vinegar is only an aqueous solution of acetic acid (Ka = 1.8 × 10-5), calculate the concentration of acetic acid in vinegar.
A solution of formic acid (HCOOH, Ka = 1.8 × 10-4) has a pH of 2.70. Calculate the initial concentration of formic acid in this solution.
The pH of a 0.063-M solution of hypobromous acid (HOBr but usually written HBrO) is 4.95. Calculate Ka.
Trichloroacetic acid (CCl3CO2H) is a corrosive acid that is used to precipitate proteins. The pH of a 0.050-M solution of trichloroacetic acid is the same as the pH of a 0.040-M HClO4 solution. Calculate Ka for trichloroacetic acid.
Calculate the percent dissociation for a 0.22-M solution of chlorous acid (HClO2, Ka = 0.012).
Calculate the percent dissociation of the acid in each of the following solutions.a. 0.50 M acetic acidb. 0.050 M acetic acidc. 0.0050 M acetic acidd. Use Le Châtelier’s principle to explain why percent dissociation increases as the concentration of a weak acid decreases.e. Even though the
A solution contains a mixture of acids: 0.50 M HA (Ka = 1.0 × 10–3), 0.20 M HB (Ka = 1.0 × 10–10), and 0.10 M HC (Ka = 1.0 × 10–12). Calculate the [H+] in this solution.
Saccharin, a sugar substitute, has the formula HC7H4NSO3 and is a weak acid with Ka = 2.0 × 10–12. If 100.0 g of saccharin is dissolved in enough water to make 340 mL of solution, calculate the pH of the resulting solution.
A typical aspirin tablet contains 325 mg acetylsalicylic acid (HC9H7O4). Calculate the pH of a solution that is prepared by dissolving two aspirin tablets in enough water to make one cup (237 mL) of solution. Assume the aspirin tablets are pure acetylsalicylic acid, Ka = 3.3 × 10-4.
A solution is prepared by dissolving 0.56 g benzoic acid (C6H5CO2H, Ka = 6.4 × 10-5 ) in enough water to make 1.0 L of solution. Calculate [C6H5CO2H], [C6H5CO2-], [H+], [OH-], and the pH of this solution.
For propanoic acid (HC3H5O2, Ka = 1.3 × 10-5), determine the concentration of all species present, the pH, and the percent dissociation of a 0.100-M solution.
What are the major species present in 0.250 M solutions of each of the following acids? Calculate the pH of each of these solutions. a. HOC6H5b. HCN
What are the major species present in 0.250 M solutions of each of the following acids? Calculate the pH of each of these solutions. a. HNO2b. CH3CO2H (HC2H3O2)
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