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Q:
What is the solubility (in g/L) of barium chromate at 25ºC? The solubility product constant for barium chromate is 1.2x10-10at 25ºC.A) 0.42 g/LB) 3.0 x10-8g/LC) 1.5 x10-8g/LD) 0.079 g/LE) 0.0028 g/L
Q:
What is the molar solubility of aluminum hydroxide at 25ºC? The solubility product constant for aluminum hydroxide is 4.6x10-33at 25ºC.A) 2.3 x10-33MB) 6.8 x10-17MC) 4.6 x10-33MD) 3.6 x10-9ME) 1.0 x10-11M
Q:
What is the molar solubility of barium fluoride at 25ºC? The solubility product constant for barium fluoride is 1.0x10-6at 25ºC.A) 6.3 x10-3MB) 1.0 x10-6MC) 5.0 x10-7MD) 1.0 x10-3ME) 1.6 x10-2M
Q:
What is the molar solubility of calcium sulfate at 25ºC? The solubility product constant for calcium sulfate is 2.4x10-5 at 25ºC.A) 2.4 x10-5MB) 3.5 x10-2MC) 1.2 x10-5MD) 1.8 x10-2ME) 4.9 x10-3M
Q:
What is the molar solubility of silver(I) bromide at 25ºC? The solubility product constant for silver(I) bromide is 5.0x10-13at 25ºC.A) 7.1 x10-7MB) 2.5 x10-13MC) 4.2 x10-4MD) 5.0 x10-5ME) 5.0 x10-13M
Q:
Rank the following metal sulfides in order of increasing molar solubility in water. SaltKspCoS4 x10-21CuS6 x10-36FeS6 x10-18HgS1.6 x10-52MnS2.5 x10-10A) MnS < FeS < CoS < CuS < HgSB) FeS < HgS < CoS < CuS < MnSC) HgS < CuS < CoS < FeS < MnSD) CuS < CoS < FeS < MnS < HgSE) CoS < CuS < FeS < HgS < MnS
Q:
What is the solubility (in g/L) of silver(I) bromide at 25ºC? The solubility product constant for silver(I) bromide is 5.0x10-13 at 25ºC.A) 9.4 x10-3g/LB) 9.4 x10-11g/LC) 1.3 x10-4g/LD) 4.7 x10-11g/LE) 7.9 x10-2g/L
Q:
What is the solubility (in g/L) of aluminum hydroxide at 25ºC? The solubility product constant for aluminum hydroxide is 4.6x10-33 at 25ºC.A) 3.6 x10-31g/LB) 8.2 x10-10g/LC) 2.8 x10-7g/LD) 5.3 x10-15g/LE) 1.8 x10-31g/L
Q:
A saturated solution of which of the following salts will have the greatest molar concentration of silver ion?A) Ag2S (Ksp= 8 x10-51)B) AgCl (Ksp= 1.8 x10-10)C) Ag2CrO4(Ksp= 1.2 x10-12)D) Ag2CO3(Ksp= 8.1 x10-12)E) Ag4Fe(CN)6 (Ksp= 8.5 x10-45)
Q:
A saturated solution of which of the following salts will have the lowest molar concentration of chromate ion?A) BaCrO4(Ksp= 2.1 x10-10)B) CuCrO4(Ksp= 3.6 x10-6)C) Ag2CrO4(Ksp= 1.2 x10-12)D) Hg2CrO4(Ksp= 2.0 x10-9)E) Tl2CrO4(Ksp= 9.8 x10-13)
Q:
Rank the following salts in order of increasing molar solubility. SaltKsp BaSO4 1.1 x10-10 AgCl 1.8 x10-10 BaCO3 9.1 x10-9 CdS 8 x10-27 PbSO4 1.8 x10-8 A) CdS < AgCl < BaSO4< BaCO3< PbSO4B) CdS < AgCl < BaCO3< BaSO4< PbSO4C) CdS < BaSO4< AgCl < BaCO3< PbSO4D) PbSO4< BaCO3< AgCl < BaSO4< CdSE) PbSO4< BaCO3< BaSO4< AgCl < CdS
Q:
Which of the following salts has the lowest molar solubility?A) SrCO3(Ksp= 9.3 x10-10)B) MnS (Ksp= 2.5 x10-10)C) BaF2(Ksp= 1.0 x10-6)D) BaSO4(Ksp= 1.1 x10-10)E) AgCl (Ksp= 1.8 x10-10)
Q:
Which of the following salts has the highest molar solubility in water?A) SrCO3(Ksp= 9.3 x10-10)B) BaSO4 (Ksp= 1.1 x10-10)C) PbS (Ksp= 2.5 x10-27)D) BaCrO4(Ksp= 1.2 x10-10)E) AgCl (Ksp= 1.8 x10-10)
Q:
The silver-ion concentration in a saturated solution of silver(I) chromate is 1.3 x10-4M. What is Ksp for silver(I) chromate?A) 2.9 x10-16B) 4.2 x10-9C) 8.8 x10-12D) E) 1.7 x10-8
Q:
The hydroxide ion concentration of a saturated solution of Fe(OH)2is M. What is the solubility product constant for Fe(OH)2?
A) B) C) D) E)
Q:
The solubility of silver(I) carbonate is 3.6 x10-2g/L. What is the solubility product constant for silver(I) carbonate?A) 4.4 x10-15B) C) 1.7 x10-8D) 1.3 x10-4E) 1.3 x10-3
Q:
The solubility of lead(II) sulfate is 4.0 x10-2g/L. What is the solubility product constant for lead(II) sulfate?A) 1.7 x10-8B) 1.3 x10-4C) 1.6 x10-3D) 4.6 x10-15E) 8.9 x10-12
Q:
After mixing an excess PbCl2 with a fixed amount of water, it is found that the equilibrium concentration of Pb2+is 1.6 x10-2M. What is Ksp for PbCl2?A) 4.0 x10-6B) 1.6 x10-5C) 2.5 x10-4D) 4.8 x10-2E) 1.0 x10-6
Q:
The solubility of strontium carbonate in water at 25ºC is g/L. What is the Ksp of this sparingly soluble salt?A) B) C) D) E)
Q:
The concentration of calcium carbonate in a saturated aqueous solution of the salt at 25ºC is M. What is the Ksp of this sparingly soluble salt?A) B) C) D) E)
Q:
What is the correct mathematical expression for finding the molar solubility (s) of Sn(OH)2?
A) 2s3= Ksp
B) 4s3= Ksp
C) 108s5= Ksp
D) 2s2= Ksp
E) 8s3= Ksp
Q:
What is the relationship between molar solubility (s) and Ksp for calcium fluoride?A) B) C) D) E)
Q:
Figures I"IV represent ionic compounds formed upon the mixing of an aqueous solution containing cation C with an aqueous solution containing anion A. Identify the figure(s) that represent(s) products for which Ksp= 108s5, where sis the molar solubility of the ionic compound. A) only II
B) both I and II
C) only IV
D) only III
E) only I
Q:
Figures I"IV represent ionic compounds formed upon the mixing of an aqueous solution containing cation C with an aqueous solution containing anion A. Identify the figure(s) that represent(s) products for which Ksp= 4s3, where sis the molar solubility of the ionic compound. A) both I and II
B) only II
C) only IV
D) only I
E) only III
Q:
Figures I"IV represent ionic compounds formed upon the mixing of an aqueous solution containing cation C with an aqueous solution containing anion A. Identify the figure(s) that represent(s) products for which Ksp= s2, where sis the molar solubility of the ionic compound. A) only I
B) only II
C) only IV
D) only III
E) both I and II
Q:
What is the solubility product expression for Sn(IO3)2?A) Ksp= [Sn2+][IO3-]2B) Ksp= [Sn4+][2IO32-]2C) Ksp= [Sn2+][2IO3-]D) Ksp= [Sn4+][IO32-]2E) Ksp= [Sn2+][2IO3-]2
Q:
What is the solubility product expression for Pb3(PO4)4?A) Ksp= [Pb3+]4[PO44-]3B) Ksp= [3Pb3+][4PO43-]C) Ksp= [3Pb3+]3[4PO43-]4D) Ksp= [Pb2+]3[PO43-]2E) Ksp= [Pb4+]3[PO43-]4
Q:
What is the solubility product expression for La2(CO3)3?A) Ksp= [2La3+]2[3CO32-]3B) Ksp= [La2+]2[CO32-]3C) Ksp= [2La3+]2[CO32-]3D) Ksp= [2La3+][3CO32-]E) Ksp= [La3+]2[CO32-]3
Q:
What is the solubility product expression for mercury(I) iodide, Hg2I2?A) Ksp= [Hg22+][2I-]2B) Ksp= [Hg22+][I-]2C) Ksp= [Hg22+][2I- ]D) Ksp= [Hg2][I2]E) Ksp= [Hg+]2[I-]2
Q:
What is the solubility product expression for Zn3(PO4)2?A) Ksp= [Zn32+][(PO43-)2]B) Ksp= [3Zn2+]3[2PO43-]2C) Ksp= [Zn2+][2PO43-]D) Ksp= [Zn3+]2[PO42-]3E) Ksp= [Zn2+]3[PO43-]2
Q:
What is the solubility product expression for Th(IO3)4?A) Ksp= [Th4+][4IO3-]4B) Ksp= [Th4+][IO3-]C) Ksp= [Th][IO3]4D) Ksp= [Th4+][IO3-]4E) Ksp= [Th4+][IO3-]
Q:
What is the solubility product expression for Al(OH)3?A) Ksp= [Al3+][3OH-]B) Ksp= 3[Al3+][OH-]3C) Ksp= [Al3+][OH-]3D) Ksp= [Al3+][3OH-]3E) Ksp= [Al3+][OH-]
Q:
Which of the following particulate views is/are consistent with a heterogeneous equilibrium? I II III
A) I only
B) II only
C) III only
D) II and III
E) I, II, and III
Q:
Cation C and anion A form an ionic compound for which Ksp= 4s3, where sis the molar solubility of the ionic compound. Which of Figures I"III represent(s) possible results of the mixing of an aqueous solution containing cation C with an aqueous solution containing an ion A?A) only IIIB) only IIC) both I and IID) only IE) both I and III
Q:
Cation C and anion A form an ionic compound for which Ksp= s2, where sis the molar solubility of the ionic compound. Which of Figures I"III represent(s) possible results of the mixing of an aqueous solution containing cation C with an aqueous solution containing anionA? A) only I
B) only III
C) both I and III
D) both I and II
E) only II
Q:
What is the percent ionization of a solution prepared by dissolving 0.0111 mol of chloroacetic acid, (HC2H2O2Cl) in 1.80 L of water? For chloroacetic acid, Ka=1.4x10-3.A) 0.62 %B) 100 %C) 38 %D) 62 %E) 0.23 %
Q:
What is the pH of a solution prepared by dissolving 0.0265 mol of chloroacetic acid, (HC2H2O2Cl) in 1.30 L of water? For chloroacetic acid, Ka=1.4x10-3.A) 1.69B) 2.33C) 11.67D) 12.31E) 2.27
Q:
What is the equilibrium concentration of chloroacetic acid, HC2H2O2Cl, in a solution prepared by dissolving 0.0221 mol of HC2H2O2Cl in 1.20 L of water? For chloroacetic acid, Ka=1.4x10-3.A) 4.43 x10-3MB) 1.84 x10-2MC) 5.08 x10-3MD) 1.40 x10-2ME) 9.21 x10-3M
Q:
It is safe to make the simplifying assumption that xcan be neglected in the denominator of the equilibrium equation whenA) B) C) D) E)
Q:
What is the equilibrium pH of an initially 5.1 M solution of hypoiodous acid, HOI, at 25ºC (Ka=)?A) 4.97B) 7.00C) 5.12D) 4.81E) 8.33
Q:
What is the equilibrium hydronium ion concentration of an initially 4.2 M solution of hypochlorous acid, HOCl, at 25ºC (Ka=)?A) MB) MC) MD) ME) M
Q:
What is the equilibrium pH of an initially 0.26 M solution of the monoprotic acid hydrazoic acid at 25ºC (Ka=)?A) 2.62B) 7.00C) 2.32D) 11.68E) 4.68
Q:
What is the hydronium-ion concentration of a 0.30 Msolution of HCN (Ka=4.9x10-10) at 25ºC?A) 1.7 x10-4MB) 3.4 x10-6MC) 2.2 x10-6MD) 1.2 x10--5ME) 4.0 x10-5M
Q:
What is the equilibrium percent ionization of an initially 0.40 M solution of the monoprotic acid propanoic acid, HC3H5O2, at 25ºC (Ka=)?A) 0.58%B) 1.2%C) 0.0013%D) 0.13%E) 1.4%
Q:
The equilibrium hydronium ion concentration of an initially 0.150 Msolution of a monoprotic weak acid is M. The acid dissociation constant is at 25ºC. What is the pH of this solution?A) 2.85B) 7.00C) 11.15D) 5.71E) 0.82
Q:
What is Kafor a weak monoprotic acid if a 0.020 Msolution of the acid has a pH of 3.23 at 25ºC?A) 5.9 x 10-2B) 1.7 x 10-5C) 7.8 x 10-2D) 1.2 x 10-6E) 3.5 x 10-4
Q:
A 0.10 M solution of a weak monoprotic acid has a pH of 3.40 at 25ºC. What is the acid-ionization constant, Ka, for this acid?A) 1.6 x 10-6B) 4.0 x 10-4C) 3.4 x 10-5D) 1.2 x 10-3E) 1.8 x 10-7
Q:
A 0.10 Msolution of a weak monoprotic acid has a hydronium-ion concentration of 4.2 x 10-4M. What is the acid-ionization constant, Ka, for this acid?A) 2.0 x 10-2B) 2.9 x 10-3C) 4.2 x 10-4D) 1.8 x 10-6E) 5.0 x 10-5
Q:
An initially 2.2 Maqueous solution of a weak monoprotic acid has a total ionconcentration of Mwhen equilibrium is established. What is the acid-ionization constant, Ka, of the weak acid? (assume Ca/Ka102)A) B) C) D) E)
Q:
A 0.10 M aqueous solution of a weak acid HA has a pH of 5.00. What is the value of Ka for HA?A) 1.0 x 10-8B) 1.0 x 10-6C) 1.0 x 10-7D) 1.0 x 10-5E) 1.0 x 10-9
Q:
A 7.5 x 10-3M solution of acetic acid, HC2H3O2, is 4.9% ionized at 25ºC. In a 7.5 x 10-4M solution, the percentage of ionization would beA) 100%.B) <4.9%.C) >4.9%.D) the same.E) zero.
Q:
A 0.010 Maqueous solution of a weak acid HA has a pH of 5.0. What is the degree of ionization of HA in the solution?A) 1 %B) 0.01 %C) 10 %D) 0.1 %E) 0.001 %
Q:
Equal moles of the indicated acids are dissolved in the amounts of water shown in the beakers below. In which solution will the percent ionization of the acid be the lowest? A) All have equal percent ionization of acid.
B) III
C) IV
D) II
E) I
Q:
At a temperature of 25ºC an initally 0.048 Msolution of a weak monoprotic acid is 2.7 % ionized once equilibrium is established. What is the acid-ionization constant, Ka, for this acid? (assume Ca/Ka102)A) B) C) D) E)
Q:
What is the pH of an initially 0.580 M solution of a weak monoprotic acid that is 0.24 % ionized when equilibrium is established? (assume Ca/Ka102)A) 2.85B) 7.00C) 0.85D) 9.12E) 11.15
Q:
A 0.20 Msolution of a weak monoprotic acid is 0.18 % ionized. What is the acid-ionization constant, Ka, for this acid?A) 1.3 x 10-6B) 1.8 x 10-6C) 0.9 x 10-4D) 1.6 x 10-5E) 6.5 x 10-7
Q:
What is the percent ionization of a 1.8M HC2H3O2 solution (Ka=1.8 x 10-5 ) at 25ºC?A) 0.57 %B) 0.32 %C) 2.2 %D) 0.18 %E) 0.24 %
Q:
Rank acetic acid (HC2H3O2), hydrocyanic acid (HOCN), and hydrofluoric acid (HF) in order of increasing strength. Acid Ka HC2H3O2 1.8 x 10-5 HOCN 3.5 x 10-4 HF 6.8 x 10-4 A) HC2H3O2< HOCN < HFB) HOCN < HC2H3O2< HFC) HOCN < HF < HC2H3O2D) HF < HOCN < HC2H3O2E) HF < HC2H3O2< HOCN
Q:
Consider the Ka values for the following acids:Cyanic acid, HOCN, 3.5 x 10-4Formic acid, HCHO2, 1.7 x 10-4Lactic acid, HC3H5O3, 1.3 x 10-4Propionic acid, HC3H5O2, 1.3 x 10-Benzoic acid, HC7H5O2, 6.3 x 10-5Given initially equimolar soutions of each weak acid, which solution will have the highest hydronium ion concentration once equilibrium is established?A) cyanic acidB) benzoic acidC) lactic acidD) formic acidE) propionic acid
Q:
Consider the Ka values for the following acids:Cyanic acid, HOCN, 3.5 x 10-4Formic acid, HCHO2, 1.7 x 10-4Lactic acid, HC3H5O3, 1.3 x 10-4Propionic acid, HC3H5O2, 1.3 x 10-5Benzoic acid, HC7H5O2, 6.3 x 10-5Which has the strongest conjugate base?A) propionic acidB) benzoic acidC) lactic acidD) formic acidE) cyanic
Q:
For the equilibrium that exists in an aqueous solution of nitrous acid (HNO2, a weak acid), the equilibrium-constant expression isA) K=B) K=C) K=D) K= [H+][NO2-].E) none of these
Q:
What is the equilibrium expression for the equilibrium A-(aq) + H3O+(aq) HA(aq) + H2O(l)?A) B) C) D) E) Kb
Q:
For which of the following equilibria does Kccorrespond to the acid-dissociation constant, Ka, of H2PO4-?A) H2PO4-(aq)+ H3O+(aq) H3PO4(aq) + H2O(l)B) H2PO4-(aq) + H2O(l) H3PO4(aq) + OH-(aq)C) H2PO4-(aq) + H2O(l) H3O+(aq) + HPO42-(aq)D) H3PO4(aq) + H2O(l) H3O+(aq) + H2PO4-(aq)E) HPO42-aq) + H2O(l) H2PO4-(aq) + OH-(aq)
Q:
For which of the following equilibria does Kccorrespond to the acid-ionization constant, Ka,of HC2O4-?A) HC2O4-(aq) + H2O(l) H2C2O4(aq) + OH-(aq)B) H2C2O4(aq) + H2O(l) H3O+(aq) + HC2O4-(aq)C) HC2O4-(aq) + H2O(l) H3O+(aq) + C2O42-(aq)D) HC2O4-(aq) + OH-(aq) C2O42-(aq) + H2O(l)E) HC2O4-(aq) + H3O+(aq) H2C2O4(aq) + H2O(l)
Q:
For which of the following equilibria does Kccorrespond to the acid-ionization constant, Ka,of HCO3-?A) HCO3-(aq) + OH-(aq) CO32-(aq) + H2O(l)B) H2CO3(aq) + H2O(l) HCO3-(aq) + H3O+(aq)C) HCO3-(aq) + H2O(l) H2CO3(aq) + OH-(aq)D) HCO3-(aq) + H3O+(aq) H2CO3(aq) + H2O(l)E) HCO3-(aq) + H2O(l) CO32-(aq) + H3O+(aq)
Q:
Which of the following is/are true concerning the acid-ionization of a monoprotic weak acid?
1) The products of an acid-ionization include the hydronium ion (hydrogen ion) or hydroxide ion.
2) The percent ionization of a weak acid is greatest for the most dilute solution.
3) A weak acid ionization constant is only valid in an aqueous solvent.
A) 1 only
B) 2 only
C) 3 only
D) 2 and 3
E) 1, 2, and 3
Q:
For which of the following equilibria does Kccorrespond to an acid-ionization constant, Ka?A) NH3(aq) + H3O+(aq) NH4+(aq) + H2O(l)B) NH4+(aq) + OH-(aq) NH3(aq) + H2O(l)C) F-(aq) + H2O(l) HF(aq) + OH-(aq)D) HF(aq) + OH-(aq) H2O(l) + F-(aq)E) NH4+(aq) + H2O(l) NH3(aq) + H3O+(aq)
Q:
In the titration of a weak monoprotic acid with a strong base, the pH at the endpoint will beA) equal to the pKa of the weak acid.B) less than 7.00.C) equal to 7.00.D) greater than the pKa of the weak acid.E) less than the pKa of the weak acid.
Q:
In the titration of a weak monoprotic acid with a strong base, the pH at the endpoint will beA) equal to the pKa of the weak acid.B) greater than 7.00.C) equal to 7.00.D) less than 7.00.E) less than the pKaof the weak acid.
Q:
In the titration of a weak monoprotic acid with a strong base, the pH of the titration solution halfway to the endpoint will beA) equal to the pKa of the weak acid.B) greater than 7.00.C) equal to 7.00.D) greater than the pKaof the weak acid.E) less than the pKaof the weak acid.
Q:
Titration of 0.4089 g of an unknown monoprotic acid dissolved in 25.00 mL of water requires 28.45 mL of 0.1521 M NaOH to reach the end point. What is the molar mass of the acid?A) 94.49 g/molB) 0.01058 g/molC) 107.5 g/molD) 2.186 g/molE) 2.718 g/mol
Q:
Consider the titration of 300.0 mL of 0.410 M NH3(Kb= 1.8 x10-5) with 0.500M HNO3. After 150.0 mL of 0.500M HNO3has been added, what is the pH of the solution?A) 4.94B) 9.06C) 6.06D) 11.06E) none of these
Q:
Which of the following statements is true concerning the titration of a weak base by a solution of hydrochloric acid?A) The solution is basic at the equivalence point.B) The solution is acidic at the equivalence point.C) At the equivalence point, the pH is determined by the hydrolysis of chloride ion.D) At the equivalence point, the pH is 7.E) At the equivalence point, there is excess hydrochloric acid.
Q:
A weak base is titrated with a hydrochloric acid solution. What is the pH at the equivalence point?
A) equal to pKa
B) equal to 7
C) equal to pKb
D) greater than 7
E) less than 7
Q:
A sample of ammonia (Kb= 1.8 x10-5) is titrated with 0.1 M HCl. At the equivalence point, what is the approximate pH of the solution?A) 5B) 1C) 9D) 7E) 11
Q:
The following titration curve depicts the titration of a weak acid with a strong base. Which of the labeled points is/are part of the buffer region.A) II onlyB) III onlyC) I onlyD) II and VE) I and IV
Q:
Which acid-base combination is depicted by this titration curve? A) Titration of a weak acid with a strong base.
B) Titration of a weak base with a strong acid.
C) Titration of a strong acid with a strong base.
D) Titration of a strong base with a strong acid.
E) Not enough information provided.
Q:
A 25.00-mL sample of propionic acid, HC3H5O2, of unknown concentration was titrated with 0.151 M KOH. The equivalence point was reached when 41.28 mL of base had been added. What is the hydroxide-ion concentration at the equivalence point? Ka for propionic acid is 1.3x10-5 at 25ºC.A) 1.5 x10-9MB) 1.0 x10-7MC) 1.1 x10-5MD) 8.5 x10-6ME) 1.1 x10-3M
Q:
A 25.00-mL sample of propionic acid, HC3H5O2, of unknown concentration was titrated with 0.101M KOH. The equivalence point was reached when 42.20mL of base had been added. What is the concentration of the propionate ion at the equivalence point?A) 0.101 MB) 0.147 MC) 0.0634 MD) 0.170 ME) 0.128 M
Q:
A 25.00-mL sample of propionic acid, HC3H5O2, of unknown concentration was titrated with 0.155M KOH. The equivalence point was reached when 35.94 mL of base had been added. What was the original concentration of the propionic acid?A) 0.295 MB) 0.111 MC) 0.108 MD) 0.155 ME) 0.223 M