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chemistry and chemical reactivity

Questions and Answers of Chemistry And Chemical Reactivity

What is the pH change when 20.0 mL of 0.100 M NaOH is added to 80.0 mL of a buffer solution consisting of 0.169 M NH3 and 0.183 M NH4Cl?
Phenol, C6H5OH, is a weak organic acid. Suppose 0.515 g of the compound is dissolved in enough water to make 125 mL of solution. The resulting solution is titrated with 0.123 M NaOH.(a) What is the
Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 1.00 × 102 mL of solution and then titrate the solution with 0.108 M NaOH.(a) What was the pH of the
You require 36.78 mL of 0.0105 M HCl to reach the equivalence point in the titration of 25.0 mL of aqueous ammonia.(a) What was the concentration of NH3 in the original ammonia solution?(b) What are
A titration of 25.0 mL of a solution of the weak base aniline, C6H5NH2, requires 25.67 mL of 0.175 M HCl to reach the equivalence point.(a) What was the concentration of aniline in the original
Without doing detailed calculations, sketch the curve for the titration of 30.0 mL of 0.10 M NaOH with 0.10 M HCl. Indicate the approximate pH at the beginning of the titration and at the equivalence
Without doing detailed calculations, sketch the curve for the titration of 50 mL of 0.050 M pyridine, C5H5N (a weak base), with 0.10 M HCl. Indicate the approximate pH at the beginning of the
You titrate 25.0 mL of 0.10 M NH3 with 0.10 M HCl.(a) What is the pH of the NH3 solution before the titration begins?(b) What is the pH at the equivalence point?(c) What is the pH at the halfway
Construct a rough plot of pH versus volume of base for the titration of 25.0 mL of 0.050 M HCN with 0.075 M NaOH.(a) What is the pH before any NaOH is added?(b) What is the pH at the halfway point of
Using Figure 17.11, suggest an indicator to use in each of the following titrations:(a) The weak base pyridine is titrated with HCl.(b) Formic acid is titrated with NaOH.(c) Ethylenediamine, a weak
Using Figure 17.11, suggest an indicator to use in each of the following titrations.(a) NaHCO3 is titrated to CO32− with NaOH.(b) Hypochlorous acid is titrated with NaOH.(c) Trimethylamine is
Name two insoluble salts of each of the following ions.(a) Cl−(b) Zn2+(c) Fe2+
Name two insoluble salts of each of the following ions.(a) SO42−(b) Ni2+(c) Br−
Using the solubility guidelines (Figure 3.10), predict whether each of the following is insoluble or soluble in water.(a) (NH4)2CO3(b) ZnSO4(c) NiS(d) BaSO4Data given in Figure 3.10 Soluble
Predict whether each of the following is insoluble or soluble in water.(a) Pb(NO3)2(b) Fe(OH)3(c) ZnCl2(d) CuS
For each of the following insoluble salts, (1) write a balanced equation showing the equilibrium occurring when the salt is added to water, and (2) Write the Ksp expression.(a) AgCN(b) NiCO3 (c)
For each of the following insoluble salts, (1) write a balanced equation showing the equilibrium occurring when the salt is added to water, and (2) write the Ksp expression.(a) PbSO4(b) BaF2(c) Ag3PO4
When 1.55 g of solid thallium(I) bromide is added to 1.00 L of water, the salt dissolves to a small extent.The thallium(I) and bromide ions in equilibrium with TlBr each have a concentration of 1.9
At 20°C, a saturated aqueous solution of silver acetate, AgCH3CO2, contains 1.0 g of the silver compound dissolved in 100.0 mL of solution. Calculate Ksp for silver acetate. AgCH3CO₂ (s) → Ag+
When 250 mg of SrF2, strontium fluoride, is added to 1.00 L of water, the salt dissolves to a very small extent.At equilibrium, the concentration of Sr2+ is found to be 1.03 × 10−3 M. What is the
Calcium hydroxide, Ca(OH)2, dissolves in water to the extent of 1.78 g per liter. What is the value of Ksp for Ca(OH)2? Ca(OH)₂ (s) → Ca2+ (aq) + 2 OH-(aq)
You add 0.979 g of Pb(OH)2 to 1.00 L of pure water at 25°C. The pH is 9.15. Estimate the value of Ksp for Pb(OH)2.
You place 1.234 g of solid Ca(OH)2 in 1.00 L of pure water at 25°C. The pH of the solution is found to be 12.68. Estimate the value of Ksp for Ca(OH)2.
Estimate the solubility of silver iodide in pure water at 25°C (a) In moles per liter and (b) In grams per liter. Agl(s) Agt (aq) + I¯(aq) =
What is the molar concentration of Au+(aq) in a saturated solution of AuCl in pure water at 25°C? AuCl(s) Au+ (aq) + Cl(aq)
Estimate the solubility of calcium fluoride, CaF2, (a) In moles per liter and(b) In grams per liter of pure water. 2+ CaF₂(s) Ca²+ (aq) + 2 F-(aq)
Estimate the solubility of lead(II) bromide (a) In moles per liter and (b) In grams per liter of pure water.
The Ksp value for radium sulfate, RaSO4, is 4.2 × 10−11. If 25 mg of radium sulfate is placed in 1.00 × 102 mL of water, does all of it dissolve? If not, how much dissolves?
If 55 mg of lead(II) sulfate is placed in 250 mL of pure water, does all of it dissolve? If not, how much dissolves?
Use Ksp values to decide which compound in each of the following pairs is more soluble. (Appendix J.)(a) PbCl2 or PbBr2(b) HgS or FeS(c) Fe(OH)2 or Zn(OH)2Data given in Appendix J TABLE 18A
Use Ksp values to decide which compound in each of the following pairs is more soluble. (Appendix J.)(a) AgBr or AgSCN(b) SrCO3 or SrSO4(c) AgI or PbI2(d) MgF2 or CaF2Data given in Appendix J TABLE
Calculate the molar solubility of silver thiocyanate, AgSCN, in pure water and in water containing 0.010 M NaSCN.
Calculate the solubility of silver bromide, AgBr, in moles per liter, in pure water. Compare this value with the molar solubility of AgBr in 225 mL of water to which 0.15 g of NaBr has been added.
Compare the solubility, in milligrams per milliliter, of silver iodide, AgI,(a) In pure water and(b) In water that is 0.020 M in AgNO3.
What is the solubility, in milligrams per milliliter, of BaF2,(a) In pure water and(b) In water containing 5.0 mg/mL KF?
Calculate the solubility, in moles per liter, of iron(II) hydroxide, Fe(OH)2, in a solution buffered to a pH of 7.00.
Calculate the solubility, in moles per liter, of calcium hydroxide, Ca(OH)2, in a solution buffered to a pH of 12.60.
Which insoluble compound in each pair should be more soluble in nitric acid than in pure water?(a) PbCl2 or PbS(b) Ag2CO3 or AgI(c) Al(OH)3 or AgCl
Which compound in each pair is more soluble in water than is predicted by a calculation from Ksp?(a) AgI or Ag2CO3(b) PbCO3 or PbCl2(c) AgCl or AgCN
Sodium carbonate is added to a solution in which the concentration of Ni2+ ion is 0.0024 M. Will precipitation of NiCO3 occur (a) When the concentration of the carbonate ion is 1.0 × 10−6 M or(b)
You have a solution that has a lead(II) ion concentration of 0.0012 M. If enough soluble chloride-containing salt is added so that the Cl− concentration is 0.010 M, will PbCl2 precipitate?
If the concentration of Zn2+ in 10.0 mL of water is 1.63 × 10−4 M, will zinc hydroxide, Zn(OH)2, precipitate when 4.0 mg of NaOH is added?
You have 95 mL of a solution that has a lead(II) concentration of 0.0012 M. Will PbCl2 precipitate when 1.20 g of solid NaCl is added?
If the concentration of Mg2+ ion in sea water is 1350 mg/L, what OH− concentration is required to precipitate Mg(OH)2?
Zinc hydroxide is amphoteric (Section 16.10). Use equilibrium constants to show that, given sufficient OH−, Zn(OH)2 can dissolve in NaOH.Data given in Section 16.10The concept of acid–base
Will a precipitate of Mg(OH)2 form when 25.0 mL of 0.010 M NaOH is combined with 75.0 mL of a 0.10 M solution of magnesium chloride?
Solid silver iodide, AgI, can be dissolved by adding aqueous sodium cyanide. Calculate Knet for the following reaction. Agl(s) + 2 CN- (aq) ⇒ [Ag(CN)₂]¯(aq) + I- (aq)
What amount of ammonia (moles) must be added to dissolve 0.050 mol of AgCl suspended in 1.0 L of water?
Can you dissolve 15.0 mg of AuCl in 100.0 mL of water if you add 15.0 mL of 6.00 M NaCN?
What is the solubility of AgCl (a) In pure water and (b) In 1.0 M NH3?
The chemistry of silver(I) cyanide:(a) Calculate the solubility of AgCN(s) in water from the Ksp value.(b) Calculate the value of the equilibrium constant for the reactionfrom Ksp and Kf values and
In each of the following cases, decide whether a precipitate will form when mixing the indicated reagents, and write a balanced equation for there action. (a) NaBr(aq) (b) KCl(aq) + +
In each of the following cases, decide whether a precipitate will form when mixing the indicated reagents, and write a balanced equation for the reaction. (a) Na₂SO4(aq) (b) K3PO4(aq) + FeCl3(aq) +
If you mix 48 mL of 0.0012 M BaCl2 with 24 mL of 1.0 × 10−6 M Na2SO4, will a precipitate of BaSO4 form?
Calculate the hydronium ion concentration and the pH of the solution that results when 20.0 mL of 0.15 M acetic acid, CH3CO2H, is mixed with 5.0 mL of 0.17 M NaOH.
Calculate the hydronium ion concentration and the pH of the solution that results when 50.0 mL of 0.40 M NH3 is mixed with 25.0 mL of 0.20 M HCl.
For each of the following cases, decide whether the pH is less than 7, equal to 7, or greater than 7.(a) Equal volumes of 0.10 M acetic acid, CH3CO2H, and 0.10 M KOH are mixed.(b) 25 mL of 0.015 M
Rank the following compounds in order of increasing solubility in water: Na2CO3, BaCO3, Ag2CO3.
A sample of hard water contains about 2.0 × 10−3 M Ca2+. A soluble fluoride containing salt such as NaF is added to “fluoridate” the water (to aid in the prevention of dental cavities). What
What is the pH of a buffer solution prepared from 5.15 g of NH4NO3 and 0.10 L of 0.15 M NH3? What is the new pH if the solution is diluted with pure water to a volume of 5.00 × 102 mL?
If you place 5.0 mg of SrSO4 in 1.0 L of pure water, will all of the salt dissolve before equilibrium is established, or will some salt remain undissolved? Celestite, SrSO4 Strontium sulfate Cengage
Describe the effect on the pH of the following actions or explain why there is not an effect:(a) Adding sodium acetate, NaCH3CO2, to 0.100 M CH3CO2H(b) Adding NaNO3 to 0.100 M HNO3
What is the equilibrium constant for the following reaction?Does the equilibrium lie predominantly to the left or to the right? Will AgI form if iodide ion, I−, is added to a saturated solution of
What volume of 0.200 M HCl must be added to 500.0 mL of 0.250 M NH3 to have a buffer with a pH of 9.00?
A buffer solution is prepared by dissolving 1.50 g each of benzoic acid, C6H5CO2H, and sodium benzoate, NaC6H5CO2, in 150.0 mL of solution.(a) What is the pH of this buffer solution?(b) Which buffer
What volume of 0.120 M NaOH must be added to 100. mL of 0.100 M NaHC2O4 to reach a pH of 4.70?
Calculate the equilibrium constant for the following reaction.Does the equilibrium lie predominantly to the left or to the right? Zn(OH)₂(s) + 2 CN- (aq) → Zn(CN)₂(s) + 2 OH-(aq)
Suppose you eat 28 grams of rhubarb leaves with an oxalic acid content of 1.2% by weight.(a) What volume of 0.25 M NaOH is required to titrate completely the oxalic acid in the leaves?(b) What mass
The solubility product constant for calcium oxalate is estimated to be 4 × 10−9. What is its solubility in grams per liter?
A solution contains 0.10 M iodide ion, I−, and 0.10 M carbonate ion, CO32−.(a) If solid Pb(NO3)2 is slowly added to the solution, which salt will precipitate first, PbI2 or PbCO3?(b) What will be
In principle, the ions Ba2+ and Ca2+ can be separated by the difference in solubility of their fluorides, BaF2 and CaF2. If you have a solution that is 0.10 M in both Ba2+ and Ca2+, CaF2 will begin
Each pair of ions below is found together in aqueous solution. Using the table of solubility product constants in Appendix J, devise a way to separate these ions by adding a reagent to precipitate
The Ca2+ ion in hard water can be precipitated as CaCO3 by adding soda ash, Na2CO3. If the calcium ion concentration in hard water is 0.010 M and if the Na2CO3 is added until the carbonate ion
A solution contains Ca2+ and Pb2+ ions, both at a concentration of 0.010 M. You wish to separate the two ions from each other as completely as possible by precipitating one but not the other using
Each pair of ions below is found together in aqueous solution. Using the table of solubility product constants in Appendix J, devise a way to separate these ions by adding a reagent to precipitate
Some photographic film is coated with crystals of AgBr suspended in gelatin. Some of the silver ions are reduced to silver metal on exposure to light. Unexposed AgBr is then dissolved with sodium
Buffer capacity is defined as the number of moles of a strong acid or strong base that is required to change the pH of 1 L of the buffer solution by one unit. What is the buffer capacity of a
Aniline hydrochloride, (C6H5NH3)Cl, is a weak acid. (Its conjugate base is the weak base aniline, C6H5NH2.) The acid can be titrated with a strong base such as NaOH.Assume 50.0 mL of 0.100 M aniline
The weak base ethanolamine, HOCH2CH2NH2,can be titrated with HCl.Assume you have 25.0 mL of a 0.010 M solution of ethanolamine and titrate it with 0.0095 M HCl. (Kb for ethanolamine is 3.2 ×
The cations Ba2+ and Sr2+ can be precipitated as very insoluble sulfates.(a) If you add sodium sulfate to a solution containing these metal cations, each with a concentration of 0.10 M, which is
You will often work with salts of Fe3+, Pb2+, and Al3+ in the laboratory. (All are found in nature, and all are important economically.) If you have a solution containing these three ions, each at a
For the titration of 50.0 mL of 0.150 M ethylamine, C2H5NH2, with 0.100 M HCl, find the pH at each of the following points, and then use that information to sketch the titration curve and decide on
A buffer solution with a pH of 12.00 consists of Na3PO4 and Na2HPO4. The volume of solution is 200.0 mL.(a) Which component of the buffer is present in a larger amount?(b) If the concentration of
To have a buffer with a pH of 2.50, what volume of 0.150 M NaOH must be added to 100. mL of 0.230 M H3PO4?
What mass of Na3PO4 must be added to 80.0 mL of 0.200 M HCl to obtain a buffer with a pH of 7.75?
You have a solution that contains AgNO3, Pb(NO3)2, and Cu(NO3)2. Devise a separation method that results in having Ag+ in one test tube, Pb2+ in another, and Cu2+ in a third test tube. Use solubility
Suggest a method for separating a precipitate consisting of a mixture of solid CuS and solid Cu(OH)2.
Composition diagrams, commonly known as “alpha plots,” are often used to visualize the species in a solution of an acid or base as the pH is varied. The diagram for 0.100 M acetic acid is shown
Which of the following barium salts should dissolve in a strong acid such as HCl: Ba(OH)2, BaSO4, or BaCO3?
The composition diagram, or alpha plot, for the important acid–base system of carbonic acid, H2CO3, is illustrated. (See Study Question 117 for more information on such diagrams.) (a) Explain
Explain why the solubility of Ag3PO4 can be greater in water than is calculated from the Ksp value of the salt.
Two acids, each approximately 0.01 M in concentration, are titrated separately with a strong base. The acids show the following pH values at the equivalence point: HA, pH = 9.5, and HB, pH = 8.5.(a)
The chemical name for aspirin is acetylsalicylic acid. It is believed that the analgesic and other desirable properties of aspirin are due not to the aspirin itself but rather to the simpler compound
Aluminum hydroxide reacts with phosphoric acid to give AlPO4. The substance is used industrially in adhesives, binders, and cements.(a) Write the balanced equation for the preparation of AlPO4 from
Solid NH4NO3 is placed in a beaker containing water at 25°C. When the solid has completely dissolved, the temperature of the solution is 23.5°C.(a) Was the process exothermic or endothermic?(b) Was
Acetic acid, a weak acid, was added to a beaker containing water at 25°C, giving a solution containing molecular acetic acid, hydronium ion, and acetate ion at equilibrium. The temperature did not
Identify the following processes as either spontaneous or not spontaneous.(a) Ice melts when placed in a flask containing water at 5°C.(b) Hydrogen iodide molecules decompose at 400 K to give a
Identify the following processes as either spontaneous or not spontaneous.(a) Liquid water turns to ice when placed in a freezer at −5°C.(b) Nitrogen gas is compressed to one half its original
Predict whether each of the following processes results in an increase in entropy in the system. (Define reactants and products as the system.)(a) Water vapor condenses as dew (liquid water) at 0°C
Predict whether each of the following processes results in an increase in entropy in the system. (Define reactants and products as the system.)(a) Water vapor condenses to liquid water at 90°C and 1

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