Q&A Hero

Q: What is the molar solubility of lead(II) chromate in 0.10 M HNO3 if the Ksp for PbCrO4 is 2.8 10-13? and the Ka2 for H2CrO4 is 3.0 10-7? Note that H2CrO4 is considered to be a strong acid. A) 9.2 10-11 M B) 2.9 10-10 M C) 9.3 10-7 M D) 3.1 10-4 M

Q: Calculate the molar solubility of thallium(I) chloride in 0.30 M NaCl at 25C. Ksp for TlCl is 1.7 10-4. A) 5.1 10-5 M B) 5.7 10-4 M C) 7.1 10-3 M D) 1.3 10-2 M

Q: What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 12.00? Ksp for Mg(OH)2 is 5.6 10-12. A) 5.6 10-10 M B) 5.6 10-8 M C) 2.4 10-6 M D) 1.1 10-4 M

Q: What is the molar solubility of CaF2 in 0.10 M NaF solution at 25C? The Ksp for CaF2 is A) 8.5 10-10 M B) 3.4 10-10 M C) 3.4 10-9 M D) 2.0 10-4 M

Q: Calculate the solubility (in g/L) of silver carbonate in water at 25C if the Ksp for Ag2CO3 is 8.4 10-12. A) 8.0 10-4 g/L B) 3.5 10-2 g/L C) 4.4 10-2 g/L D) 5.6 10-2 g/L

Q: Calculate the Ksp for silver sulfate if the solubility of Ag2SO4 in pure water is 4.5 g/L. A) 3.0 10-6 B) 1.2 10-5 C) 2.1 10-4 D) 4.2 10-4

Q: What is the most soluble salt of the following set? A) AgCN with Ksp = 6.0 10-17 B) Al(OH)3 with Ksp = 1.9 10-33 C) Fe(OH)3 with Ksp = 2.6 10-39 D) Sn(OH)2 with Ksp = 1.6 10-19

Q: What is the most soluble salt of the following set? A) Ba(OH)2 with Ksp = 5.0 10-3 B) Ca(OH)2 with Ksp = 4.7 10-6 C) Cd(OH)2 with Ksp = 5.3 10-15 D) Fe(OH)2 with Ksp = 2.5 10-37

Q: What is the chromium ion concentration for a saturated solution of Cr(OH)3 if the Ksp for Cr(OH)3 is 6.7 10-31? A) 8.19 10-16 M B) 1.26 10-8 M C) 2.17 10-8 M D) 3.76 10-8 M

Q: What is the silver ion concentration for a saturated solution of Ag2CO3 if the Ksp for Ag2CO3 is 8.4 10-12? A) 2.90 10-6 M B) 2.03 10-4 M C) 2.56 10-4 M D) 4.06 10-4 M

Q: What is the equilibrium constant expression for the Ksp of Ca3(PO4)2? A) Ksp = [Ca2+]3[PO43-]2 B) Ksp = {[Ca2+]3[PO43-]2}/[Ca3PO4] C) Ksp = {[Ca2+]3[PO43-]2}/{[Ca3PO4][H2O]} D) Ksp = 1/{[Ca2+]3[PO43-]2}

Q: The balanced equation for the solubility equilibrium of Fe(OH)2 is shown below. What is the equilibrium constant expression for the Ksp of Fe(OH)2?Fe(OH)2(s) Fe2+(aq) + 2 OH-(aq)A) Ksp = {[Fe2+][OH-]2}/{[Fe(OH)2][H2O]}B) Ksp = {[Fe2+][OH-]2}/[Fe(OH)2]C) Ksp = [Fe2+][OH-]2D) Ksp = 1/{[Fe2+][OH-]2}

Q: Which is nota hydrate of a proton? A) H3O+ B) H9O4+ C) H25O11+ D) H43O21+

Q: What is the geometric shape of the hydrated proton; that is, the hydronium ion H3O+? A) angular B) pyramidal C) trigonal planar D) tetrahedral

Q: Using the conjugate acid-base pairs listed below, complete the following equation with the pair that gives an equilibrium constant Kc> 1._____ + H2CO3_____ + HCO3-A) HF/F-B) HCl/Cl-C) HOCl/OCl-D) HSO42-/SO42-

Q: Using the conjugate acid-base pairs listed below, complete the following equation with the pair that gives an equilibrium constant Kc> 1._____ + HSO3-_____ + H2SO3A) CH3CO2H/ CH3CO2-B) HCO2H/ HCO2-C) HNO2/NO2-D) HNO3/NO3-

Q: Arrange the acids in order of increasing acid strength. A) D < C < A < B B) D < C < B < A C) D < B < A < C D) D < A < C < B

Q: Determine the strongest acid of the set. A) A B) B C) C D) D

Q: The equilibrium constant, K, for the reaction shown below has a value 1.8 10-5. In this reaction which is the strongest acid and which is the strongest base?CH3CO2H(aq) + H2O(l) H3O+(aq) + CH3CO2-(aq)A) CH3CO2H and CH3CO2-B) CH3CO2H and H2OC) H3O+and H2OD) H3O+and CH3CO2-

Q: From the following chemical reactions determine the relative Bronsted-Lowry base strengths (strongest to weakest).2 NaH(s) + H2O(l) -> 2 NaOH + H2(g)NH3(aq) + H2O(l) NH4+(aq) + OH-(aq)A) H-> OH-> NH3B) H-> NH3> OH-C) OH-> H-> NH3D) OH-> NH3> H-

Q: From the following chemical reactions determine the relative Bronsted-Lowry base strengths (strongest to weakest).HNO3(aq) + H2O(l) -> H3O+(aq) + NO3-(aq)HF(aq) + H2O(l) H3O+(aq) + F-(aq)A) HNO3> H3O+> HFB) NO3-> H2O > F-C) F-> H2O > NO3-D) F-> NO3-> H2O

Q: From the following chemical reactions determine the relative Bronsted-Lowry acid strengths (strongest to weakest).HClO4(sol) + CH3COOH(l) -> CH3C2(OH)2+(sol) + ClO4-(aq)H2SO4(sol) + CH3COOH(l) CH3C(OH)2+(sol) + HSO4-(sol)A) HClO4> H2SO4> CH3COOHB) HClO4> H2SO4> CH3C(OH)2+C) HClO4> CH3COOH > H2SO4D) HClO4> CH3C(OH)2+> H2SO4

Q: From the following chemical reactions determine the relative Br∅nsted-Lowry acid strengths (strongest to weakest).HClO4(aq) + H2O(l) -> H3O+(aq) + ClO4-(aq)HNO2(aq) + H2O(l) H3O+(aq) + NO2-(aq)A) HClO4> H3O+> HNO2B) HClO4> HNO2> H3O+C) H3O+> HClO4> HNO2D) H3O+> HNO2> HClO4

Q: From the following chemical reactions determine the relative Bronsted-Lowry acid strengths (strongest to weakest).HCl(aq) + H2O(l) -> H3O+(aq) + Cl-(aq)HCN(aq) + H2O(l) H3O+(aq) + CN-(aq)A) HCl > HCN > H3O+B) HCl > H3O+> HCNC) H3O+> HCl > HCND) HCN > H3O+> HCl

Q: What is the strongest Bronsted-Lowry acid in the chemical reaction shown below?2 HNO3(aq) + Ba(OH)2(aq) -> Ba(NO3)2(aq) + 2 H2O(l)A) HNO3B) Ba(OH)2C) Ba(NO3)2D) H2O

Q: Which Bronsted-Lowry acid has the strongest conjugate base?A) HBrB) HClO4C) HFD) HI

Q: Which Bronsted-Lowry base has the strongest conjugate acid?A) CH3CO2-B) CN-C) F-D) NO3-

Q: Which of the following Bronsted-Lowry acids does notbehave as a strong acid when it is dissolved in water?A) HBrB) HClC) HNO2D) HClO4

Q: Write a balanced equation for the dissociation of the Bronsted-Lowry acid HSO4-in water.A) HSO4-(aq) + H2O(l) H2SO4(aq) + OH-(aq)B) HSO4-(aq) + H2O(l) SO42-(aq) + H3O+(aq)C) HSO4-(aq) + H2O(l) SO32-(aq) + OH-(aq)D) HSO4-(aq) + H2O(l) SO3(g) + OH-(aq) + H2O(l)

Q: Which one of the following can behave either as a Bronsted-Lowry acid or a Bronsted-Lowry base in an aqueous solution reaction?A) HSO3-B) NH3C) HID) H3PO4

Q: What is the conjugate acid of the Bronsted-Lowry base HAsO42-?A) H2AsO4-B) AsO43-C) H2OD) H3O+

Q: What is the conjugate base of the Bronsted-Lowry acid HPO42-?A) H3PO4B) H2PO4-C) HPO42-D) PO43-

Q: Identify the conjugate acid/base pairs present in an aqueous solution of hydrogen sulfate ion, HSO4-. A) HSO4-/SO42-and H3O+/H2O B) H2SO4/HSO4-and H2O/OH- C) HSO4-/H2O and H3O+/SO42- D) HSO4-/H2O and H2SO4/OH-

Q: What are the conjugate acid-base pairs in the following chemical reaction?NH3(aq) + H2O(l) NH4+(aq) + OH-(aq)A) NH3, H2O and NH4+, OH-B) NH3, NH4+and H2O, OH-C) NH3, OH-and H2O, NH4+D) NH3and NH4+

Q: What are the Bronsted-Lowry acids in the following chemical reaction?HBr(sol) + CH3COOH(sol) CH3C(OH)2+(sol) + Br-(sol)A) HBr, CH3COOHB) HBr, CH3C(OH)2+C) CH3COOH, CH3C(OH)2+D) CH3COOH, Br-

Q: What are the Bronsted-Lowry bases in the following chemical reaction?C5H5N(aq) + H2O(l) C5H5NH+(aq) + OH-(aq)A) C5H5N, H2OB) C5H5N, C5H5NH+C) C5H5N, OH-D) C5H5N, H2O, OH-

Q: Indicate all the Bronsted-Lowry acids in the following chemical reaction.HCl(aq) + H2O(aq) H3O+(aq) + Cl-(aq)A) HCl, H2OB) HCl, H3O+C) HCl, Cl-D) HCl, H2O, H3O+

Q: In the following chemical equation indicate the reactant that is a Bronsted-Lowry acid.HCN(aq) + H2O(l) H3O+(aq) + CN-(aq)A) HCNB) H2OC) H3O+D) CN-

Q: Which one of the following species acts as a Bronsted-Lowry acid in water?A) NaHB) NH4+C) CH3NH2D) C6H6

Q: A Bronsted-Lowry acid is best defined as a substance that canA) accept a hydroxide ion.B) donate a hydroxide ion.C) accept a proton.D) donate a proton.

Q: When dissolved in water, which of the following compounds is an Arrhenius base? A) CH3OH B) HOCl C) KOH D) KCl

Q: An Arrhenius base is best defined as a A) proton donor. B) hydroxide acceptor. C) substance that dissociates in water to produce aqueous hydrogen ions. D) substance that dissociates in water to produce aqueous hydroxide ions.

Q: When dissolved in water, which of the following compounds is an Arrhenius acid? A) HCN B) NaOH C) NaF D) CH3CH2OH

Q: An Arrhenius acid is best defined as a A) hydroxide donor. B) proton acceptor. C) substance that dissociates in water to produce aqueous hydrogen ions. D) substance that dissociates in water to produce aqueous hydroxide ions.

Q: In the reaction between NO2and H2O that produces HNO3, the Lewis acid is ________ and the Lewis base is ________.

Q: In the aquation reaction Co2++ 6 H2O -> [Co(H2O)6]2+, the Lewis acid is ________ and the Lewis base is________.

Q: The acid strength of an oxoacid having the general formula HnYOmincreases as the electronegativity of Y ________ and as the oxidation number of Y ________.

Q: A 0.10 M KNO2solution will have a pH ________ seven.

Q: A 0.050 M solution of hydroxylamine, NH2OH, having Kb= 9.1 10-9has a pH of ________.

Q: Erythromycin is a basic antimicrobial with pKb= 5.2. A 1.0 10-3M solution of erythromycin has a pH of and a percent ionization.

Q: Phenobarbital has a pKa= 7.4. Compared to a 1.0 10-3M solution, 1.0 10-4M phenobarbital will have a ________ (higher, lower) pH and a ________ (higher, lower) percent ionization.

Q: Phenobarbital is an antiepileptic drug with a water solubility of 4.3 10-3M and pKa= 7.4. What is the pH and percent ionization of 4.3 10-3M phenobarbital?

Q: A 1.25 10-4M solution of the anti-inflammatory drug naproxen has a pH = 4.2. The Kaand pKaof naproxen are ________ and ________.

Q: In order for the reaction A-+ H2CO3HA + HCO3-to have an equilibrium constant Kc< 1, the Kaof HA must be ________ (greater, less) than the Kaof H2CO3.

Q: In order for the reaction HA + HSO3-A-+ H2SO3to have an equilibrium constant Kc< 1, the Kaof HA must be ________ (greater, less) than the Kaof HSO3-.

Q: The value of Kafor a 0.250 M HCN solution having a pH of 4.956 is ________.

Q: The pH of a 0.025 M KOH solution is ________.

Q: Bromothymol blue indicator changes color from yellow at a pH of 6.0 to blue at a pH of 7.6. Methyl red indicator changes color from red at a pH of 4.4 to yellow at a pH of 6.2. A sample of saliva having [H3O+] = 6.310 10-7would impart a ________ color to bromothymol blue and a ________ color to methyl red.

Q: Bromothymol blue indicator changes color from yellow at a pH of 6.0 to blue at a pH of 7.6. Phenol red indicator changes color from yellow at a pH of 6.8 to red at a pH of 8.4. A sample of pancreatic fluid having [OH-] = 1.258 10-6would impart a ________ color to bromothymol blue and a ________ color to phenol red.

Q: One way to prepare a solution with a pH of 10.00 is to dissolve ________ grams of CaO in enough water to make 500 mL of solution.

Q: At 50C the value of Kwis 5.5 10-14, and the pH of a neutral solution at 50C is ________.

Q: At the normal body temperature of 37C, Kw= 2.42 10-14. The H3O+concentration of normal blood ranges from 3.5 10-8to 4.5 10-8. The OH-concentration of normal blood ranges from ________ to ________, and blood is ________ (acidic, basic, neutral).

Q: Undersea flora prefer a maximum concentration of OH-of 1.58 10-5. The concentration of H3O+in the seawater is ________, and this solution is ________ (acidic, basic, neutral).

Q: The concentration of H3O+in human sweat can be as low as 2.5 10-6. The concentration of OH-in the sweat is ________, and this solution is ________ (acidic, basic, neutral).

Q: An acidic solution with hydronium ion concentration [H+] = 1.60 10-3M has a hydroxide ion concentration [OH-] = ________.

Q: The number of waters of hydration in the hydrate proton H7O3+is ________.

Q: A proton hydrated by four water molecules has the formula ________.

Q: The equilibrium constant for the reaction below has the value Ka= 3.5 10-4. In this reaction the stronger Bronsted-Lowry acid is ________ and the weaker Bronsted-Lowry acid is ________.HF(aq) + H2O(l) H3O+(aq) + F-(aq)

Q: The Br∅nsted-Lowry acids in the chemical equation below are ________ and ________.HNO2(aq) + H2O(l) H3O+(aq) + NO2-(aq)

Q: Which one of the following salts, when dissolved in water, produces the solution with the lowestpH?A) NaClB) KClC) MgCl2D) AlCl3

Q: Calculate the pH of a 1.60 M CH3NH3Cl solution. Kbfor methylamine, CH3NH2, is 3.7 10-4. A) 1.61 B) 5. 18 C) 8. 82 D) 12.39

Q: Calculate the pH of a 1.60 M KBrO solution. Kafor hypobromous acid, HBrO, is 2.0 10-9. A) 2.55 B) 4.25 C) 9. 75 D) 11.45

Q: Calculate the pH of a 0.800 M NaCH3CO2solution. Kafor acetic acid, CH3CO2H, is 1.89 10-5. A) 2. 42 B) 4.68 C) 9.32 D) 11. 58

Q: Which one of the following salts, when dissolved in water, produces the solution with a pH closestto 7.00? A) NH4Br B) CaO C) KHSO4 D) Cs I

Q: Which one of the following salts, when dissolved in water, produces the solution with the highestpH? A) RbI B) RbBr C) RbCl D) RbF

Q: Which one of the following salts, when dissolved in water, produces the solution with the highestpH? A) KH CO3 B) CsClO4 C) RaO D) CH3CH3NH3Cl

Q: Determine the ammonia concentration of an aqueous solution that has a pH of 11. 00. The equation for the dissociation of NH3(Kb = 1.8 10-5) isNH3(aq) + H2O(l) NH4+(aq) + OH-(aq).A) 3.0 MB) 0. 056 MC) 1.8 10- 2MD) 1.0 10-3M

Q: Aniline, (C6H5NH2, Kb= 4.3 10-10at 25C) is an industrially important amine used in the making of dyes. Determine the pH of an aniline solution made by dissolving 6.90 g of aniline in enough water to make 100 mL of solution. A) 4. 75 B) 9. 25 C) 9. 50 D) 10. 50

Q: What is the pH of a 0.30 M pyridine solution that has Kb= 1.9 10-9? The equation for the dissociation of pyridine isC5H5N(aq) + H2O(l) C5H5NH+(aq) + OH-(aq).A) 4. 62B) 8.72C) 9. 38D) 10. 38

Q: What is the pH of a 0. 200 M NH3solution that has Kb= 1.8 10-5? The equation for the dissociation of NH3isNH3(aq) + H2O(l) NH4+(aq) + OH-(aq).A) 2.02B) 2. 72C) 11. 98D) 11.28