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Chemistry
Q:
For which of the following equilibria does Kccorrespond to a base-ionization constant, Kb?A) H3O+(aq) + OH-(aq) 2H2O(l)B) HCO3-(aq) + OH-(aq) CO32-(aq) + H2O(l)C) HOCl(aq) + H2O(l) H3O+(aq) + OCl-(aq)D) CO32-(aq) + H2O(l) HCO3-(aq) + OH-(aq)E) HCHO2(aq) + NH3(aq) CHO2-(aq) + NH4+(aq)
Q:
What is the equilibrium concentration of H2C2O4 in a 0.230 Moxalic acid, H2C2O4, solution? For oxalic acid, Ka1= 5.6 x10-2 and Ka2= 5.1 x10-5.A) 1.4 x10-1MB) 1.1 x10-1MC) 2.3 x10-1MD) 5.1 x10-5ME) 8.9 x10-2M
Q:
What is the concentration of C2O42-in a 0.370 Moxalic acid, H2C2O4, solution? For oxalic acid, Ka1= 5.6 x10-2and Ka2= 5.1 x10-5.A) 1.2 x10-1MB) 4.3 x10-3MC) 4.3 x10-3MD) 5.1 x10-5ME) 1.4 x10-1M
Q:
What is the concentration of HC2O4-in a 0.390 M oxalic acid, H2C2O4, solution? For oxalic acid, Ka1= 5.6 x10-2and Ka2= 5.1 x10-5.A) 4.4 x10-3MB) 1.2 x10-1MC) 1.5 x10-1MD) 4.5x10-3ME) 5.1 x10-5M
Q:
What is the hydroxide-ion concentration of a 0.240 M oxalic acid, H2C2O4, solution? For oxalic acid, Ka1= 5.6 x10-2and Ka2= 5.1 x10-5.A) 2.9 x10-12MB) 8.6 x10-14MC) 3.5 x10-3MD) 1.1 x10-13ME) 1.0 x10-7M
Q:
What is the hydronium-ion concentration of a 0.350 M oxalic acid, H2C2O4, solution? For oxalic acid, Ka1= 5.6 x10-2and Ka2= 5.1 x10-5.A) 1.1 x10-1MB) 1.4 x10-1MC) 1.0 x10-7MD) 4.2 x10-3ME) 4.2 x10-3M
Q:
What is the concentration of CO32- in a 0.030 M solution of carbonic acid, H2CO3? For carbonic acid, Ka1= 4.2 x10-7and Ka2= 4.8 x10-11.A) 3.0 x10-2MB) 1.1 x10-4MC) 5.6 x10-5MD) 4.8 x10-11ME) 4.2 x10-7M
Q:
What is the concentration of HCO3- in a 0.029 M solution of carbonic acid, H2CO3? For carbonic acid, Ka1= 4.2 x10-7and Ka2= 4.8 x10-11.A) 1.1 x10-4MB) 2.9 x10-2MC) 5.5 x10-5MD) 4.8 x10-11ME) 4.2 x10-7M
Q:
What is the hydronium-ion concentration in a 0.030 M solution of carbonic acid, H2CO3? For carbonic acid, Ka1= 4.2 x10-7and Ka2= 4.8 x10-11.A) 3.0 x10-2MB) 4.2 x10-7MC) 4.8 x10-11MD) 1.1 x10-4ME) 5.6 x10-5M
Q:
The equilibrium hydronium ion concentration of an initially 0.228 Msolution of a diprotic weak acid (H2A) is M. What is Ka1? (assume Ca/Ka102 and Ka1>> Ka2)A) B) C) D) E) not enough information provided
Q:
In a 0.10 M solution of a diprotic acid H2A (Ka1= 3.6 x10-5 and Ka2= 9.8 x10-10 at 25ºC), what is the equilibrium concentration of A2"?A) 9.9 x10-6 MB) 9.8 x10-10 MC) 1.9 x10-3 MD) 0.20 ME) 0.10 M
Q:
Two unlabeled solutions are found to have a pH of 4.00. Which of the following is/are reasonable conclusions regarding the composition of each solution?
1) The molar concentration of H3O+is the same in both solutions.
2) The relatively high pH compared to a solution of strong acid is consistent with neither solution containing a strong acid.
3) One or both solutions may contain a weak monoprotic or multiprotic acid.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 3
E) 1, 2, and 3
Q:
Which of the following is/are true concerning multiprotic acids where Ka1>> Ka2?1) In a solution made from H3A, the equilibrium concentration of H3O+and H2A-can be accurately determined from the first ionization without accounting for the remaining ionizations.2) In a solution made from H2A, the equilibrium concentration of the fully deprotonated form of the acid (A2-) is approximately equal to Ka1.3) In general the second ionization constant of a triprotic acid is nearly equal to the third ionization constant and both are much smaller than the first ionization constant.A) 1 onlyB) 2 onlyC) 3 onlyD) 1 and 3E) 1, 2, and 3
Q:
For a 0.10 M solution of glutaric acid, HO2C(CH2)3CO2H (Ka1= 4.6 x10-5, Ka2=3.9x10-6), rank the following species in order of increasing equilibrium concentration.A) H3O+< -O2C(CH2)3COO-< HO2C(CH2)3COO-< OH-< HO2C(CH2)3CO2HB) OH-< -O2C(CH2)3COO-< H3O+< HO2C(CH2)3COO-< HO2C(CH2)3CO2HC) OH-< -O2C(CH2)3COO-< HO2C(CH2)3COO-< H3O+< HO2C(CH2)3CO2HD) H3O+< HO2C(CH2)3CO2H < HO2C(CH2)3COO-< -O2C(CH2)3COO-< OH-E) OH-< -O2C(CH2)3COO-< HO2C(CH2)3COO-< HO2C(CH2)3CO2H < H3O+
Q:
Hydrosulfuric acid, H2S, is a weak diprotic acid. In a 0.1 M solution of the acid, which of the following species is present in the largest amount?A) HS-B) S2-C) H2SD) H3O+E) OH-
Q:
For a 0.05 M H2SO3solution, which of the following relationships is true?A) [SO32-] > [H2SO3]B) [SO32-] > [HSO3-]C) [HSO3-] > [H2SO3]D) [H2SO3] > [H+]E) [H+] > [H2SO3]
Q:
In a 0.01 M solution of 1,4-butanedicarboxylic acid, HOOCCH2CH2COOH (Ka1= 2.9 x10-5, Ka2= 5.3 x10-6), which species is present in the lowest concentration?A) -OOCCH2CH2COO-(aq)B) H2OC) HOOCCH2CH2COO-(aq)D) H3O+(aq)E) HOOCCH2CH2COOH(aq)
Q:
In a 0.01 M solution of 1,4-butanedicarboxylic acid, HOOCCH2CH2COOH (Ka1=2.9x10-5, Ka2=5.3x10-6), which species is present in the highest concentration?A) HOOCCH2CH2COO-(aq)B) HOOCCH2CH2COOH(aq)C) H3O+(aq)D) -OOCCH2CH2COO-(aq)E) OH-(aq)
Q:
Phosphoric acid, H3PO4, will undergo three successive ionization reactions to varying extents in water. What is the balanced equilibrium identified as Ka3?A) H2PO4-(aq) + H2O(l) H3O+(aq) + HPO42-(aq)B) HPO42-(aq) + H2O(l) PO43-(aq) + H3O+(aq)C) H2PO4-(aq)+ H3O+(aq) H3PO4(aq) + H2O(l)D) H3PO4(aq) + H2O(l) H3O+(aq) + H2PO4-(aq)E) PO43-(aq) + H2O(l) HPO42-(aq) + OH-(aq)
Q:
Which of the following represents the usual relationship of acid-ionization constants for a triprotic acid?A) B) C) D) E)
Q:
A 8.80-g sample of homogentisic acid, a weak organic acid having Ka= 4.0 x10-5, is dissolved in 25.00 mL of water and its pH is measured to be 2.039. What is the molar mass of homogentisic acid?A) 168 g/molB) 964 g/molC) 2.09 g/molD) 4.20 g/molE) 352 g/mol
Q:
Which solution would cause blue litmus to turn red?A) a solution of pH 10B) a solution of 0.01 MNH3C) a solution of pOH 4D) a solution of 0.005 MCH3COOHE) a solution of 0.10 MNaOH
Q:
What is the hydroxide-ion concentration in a solution formed by combining 200.mL of 0.15M HCl with 300.mL of 0.090M NaOH at 25ºC?HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)A) 1.7 x 10-13MB) 0.090 MC) 1.7 x 10-12MD) 0.054 ME) 1.0 x 10-7M
Q:
The pH of a solution of a strong base is 10.27 at 25ºC. What is its hydronium-ion concentration?A) 2.9 x 10-3 MB) 1.9 x 10-4 MC) 1.4 x 10-4MD) 5.4 x 10-11 ME) 1.4 x 10-2M
Q:
The pOH of a solution is 5.06. What is its hydronium-ion concentration?A) 1.1 x 105MB) 1.1 x 10-9MC) 8.7 x 10-6MD) 5.06 ME) 6.3 x 10-3M
Q:
A solution has a pOH of 5.36. What is its hydroxide-ion concentration?A) 1.8 x 10-4 MB) 5.4 MC) 2.3 x 10-9 MD) 4.4 x 10-6 ME) 4.7 x 10-3 M
Q:
A solution has a pH of 10.20 at 25ºC. What is the hydroxide-ion concentration at 25ºC?A) 3.8 MB) 2.2 x 10-2MC) 1.6 x 10-4MD) 6.3 x 10-11ME) 1.0 x 10-7M
Q:
Which of the following solutions has the highest hydroxide-ion concentration?A) 0.1 M HClB) a solution with pH = 5C) 0.1 M H2SO4D) pure waterE) a solution with pOH = 12
Q:
What is the pOH of a solution prepared by dissolving 0.465 L of HCl(g), measured at STP, in enough water such that the total volume of the solution is 4.50 L? (R=0.0821 L·atm/(K·mol))A) 12.317B) 7.000C) 1.683D) 11.664E) 2.336
Q:
What is the pH of a solution prepared by dissolving 0.365 L of HCl(g), measured at STP, in enough water such that the total volume of the solution is 6.00L? (R=0.0821 L·atm/(K·mol))A) 2.566B) 11.434C) 1.788D) 7.000E) 12.212
Q:
What is the pOH of a solution prepared by dissolving 0.287 g of KOH(s) in 7.00L of water?
A) 10.864
B) 3.136
C) 2.291
D) 11.709
E) 7.000
Q:
What is the pH of a solution prepared by dissolving 0.739 g of NaOH(s) in 4.50L of water?
A) 1.733
B) 12.267
C) 7.000
D) 11.613
E) 2.387
Q:
What is the pOH of a 0.0092 M CsOH solution?A) 2.04B) 16.04C) 9.31D) 4.69E) 11.96
Q:
What is the pH of a 0.0086 M LiOH solution?A) 9.24B) 11.93C) 2.07D) 4.76E) 16.07
Q:
What is the pOH of a 0.065 M HNO3 solution?A) 12.81B) 11.27C) 15.19D) 1.19E) 2.73
Q:
A solution has a hydroxide-ion concentration of 0.043 M. What is its pH?
A) 15.37
B) 12.63
C) 17.15
D) 7.00
E) 1.37
Q:
A solution has a hydronium-ion concentration of 0.0082 M. What is its pOH?
A) 2.09
B) 16.09
C) 9.20
D) 4.80
E) 11.91
Q:
What is the pOH of a 0.0055 M Ba(OH)2solution?A) 9.49B) 11.74C) 12.04D) 1.96E) 2.26
Q:
What is the pH of a 0.0035 M Ba(OH)2solution?A) 9.04B) 11.54C) 2.46D) 11.85E) 2.15
Q:
The pOH of a solution is 5.22. What is the pH of the solution?
A) 5.22
B) 8.78
C) 6.03
D) 7.00
E) 2.68
Q:
Which solution has the highest pH?A) 0.1 M Ba(OH)2B) 0.1 M CH3COOHC) 0.1 M HClD) 0.1 M NH3E) 0.1 M NaOH
Q:
A solution has a pH value of 3.76. What is the pOH for this solution?
A) 7.00
B) 3.72
C) 3.76
D) 1.74
E) 10.24
Q:
What pH should a solution have if its pH is about the same as that of vinegar?
A) about 8
B) about 11
C) about 1
D) about 6
E) about 3
Q:
Which aqueous solution has the lowest pH?A) 0.30 M HClB) 0.30 M NaOHC) 0.30 M NH3D) 0.30 M Ba(OH)2E) 0.30 M H2SO4
Q:
At 25C, what is the pH of a 10.0 M HBr solution?A) 1.000B) 0.000C) 10.000D) -1.000E) 14.000
Q:
The hydronium-ion concentration of a solution is 2.5 x 10"6M. What is the pH of the solution?A) 6.81B) 3.77C) 2.00D) 5.60E) 10.60
Q:
What is the pH of a 0.0042 M hydrochloric acid solution?A) 5.47B) 11.62C) 7.00D) 8.53E) 2.38
Q:
What is the pH of the final solution when 25 mL of 0.025 M HCl has been added to 35mL of 0.040M HCl at 25ºC?A) 3.22B) 1.78C) 1.47D) 2.69E) 3.39
Q:
What is the pOH of a 0.044 M HI solution?A) 3.12B) 12.64C) 10.88D) 15.36E) 1.36
Q:
What is the pH of a 0.051 M HClO4 solution?A) 15.29B) 2.98C) 12.71D) 1.29E) 11.02
Q:
A solution has a hydroxide-ion concentration of 0.0030M. What is the pOH of the solution?
A) 11.48
B) 2.52
C) 7.00
D) 8.19
E) 5.81
Q:
A solution in which the pH is 1.5 would be described as
A) neutral.
B) very acidic.
C) slightly basic.
D) slightly acidic.
E) very basic.
Q:
Which of the following expressions is not equivalent to pH?A) -log [H+(aq)]B) C) 14.0 - pOHD) E) -log Kw
Q:
What is the hydronium-ion concentration of a 0.0038M Ba(OH)2solution?A) 7.6 x 10-3MB) 3.8 x 10-3MC) 1.3 x 10-12MD) 2.6 x 10-12ME) 1.0 x 10-7M
Q:
What is the hydronium-ion concentration of a 0.0087M LiOH solution?A) 1.1 x 10-12MB) 8.7 x 10-3MC) 1.0 x 10-14MD) 1.0 x 10-7ME) 8.7 x 10-17M
Q:
At 25ºC a solution has a hydroxide-ion concentration of 4.94 x 10-5M. What is its hydronium-ion concentration?A) 4.94 x 10-19MB) 1.00 x 10-7MC) 1.00 x 10-14MD) 4.94 x 10-5ME) 2.02 x 10-10M
Q:
The concentration of H3O+in a solution is 7 x 10-4M at 25ºC. What is its hydroxide-ion concentration?A) 7 x 10-4MB) 1 x 10-10MC) 2 x 10-10MD) 3 x 10-10ME) 1 x 10-11M
Q:
At 20ºC, the ion-product constant of water, Kw, is . What is the pH of pure water at 20ºC?A) 7.000B) 6.501C) 7.181D) 7.081E) none of these
Q:
What is the hydronium-ion concentration in a solution formed by combining 750mL of 0.10MNaOH with 250mL of 0.30M HCl?NaOH(aq) + HCl(aq)→ NaCl(aq) + H2O(l)A) 0.075 MB) 1.7 x 10-13MC) 1.0 x 10-7MD) 0.30 ME) 0.10 M
Q:
What is the equilibrium concentration of amide ion (NH2-) in liquid ammonia at 25ºC? ("am"=dissolvedinammonia)2NH3(l) NH4+(am) + NH2-(am); Kc= 1.8 x 10-24 at 25ºCA) 2.6 x 10-12MB) 3.6 x 10-24MC) 1.3 x 10-12MD) 1.8 x 10-24ME) 9.0 x 10-25M
Q:
The equilibrium constant for the autonionization of water (shown below) increases with increasing temperature, from 1.01 x10-14 at 25ºC to 5.31 x10-14 at 50°C.H2O(l) + H2O(l) H3O+(aq) + OH-(aq)Which of the following statements is consistent with this behaviour?A) The autoionization of water is an endothermic reaction.B) The autoionization of water is an exothermic reaction.C) The hydronium ion concentration at equilibrium increases with increasing temperature.D) The hydronium ion concentration at equilibrium decreases with increasing temperature.E) Both A and C.
Q:
The autoionization of water, as represented by the equation below, is known to be endothermic. Which of the following correctly states what occurs as the temperature of water is raised?H2O(l) + H2O(l) H3O+(aq) + OH-(aq)A) The pH of the water decreases, and the water becomes more acidic.B) The pH of the water decreases, and the water remains neutral.C) The pH of the water increases, and the water remains neutral.D) The pH of the water does not change, and the water remains neutral.E) The pH of the water increases, and the water becomes more acidic.
Q:
The ionization constant of water at a temperature above 25ºC is 1.7 x 10"14. What is the pH of pure water at this temperature?2H2O(l) H3O+(aq) + OH"(aq)A) 7.88B) 5.68C) 6.88D) 13.85E) 7.00
Q:
Rank H3PO4, H2PO4-, and HPO42-in order of increasing acid strength.A) HPO42-< H2PO4-< H3PO4B) H2PO4-< HPO42-< H3PO4C) H2PO4-< H3PO4< HPO42-D) HPO42-< H3PO4< H2PO4-E) H3PO4< H2PO4-< HPO42-
Q:
Which of the following solutes, dissolved in 1.0 kg of water, would be expected to provide the fewest particles and to freeze at the highest temperature?A) 0.10 mol HClOB) 0.10 mol HClO3C) 0.10 mol HClO2D) 0.10 mol HClO4E) 0.10 mol HCl
Q:
Which of the following is the strongest acid?
A) HClO2
B) HCl
C) HClO4
D) HClO
E) HClO3
Q:
Rank the following in order of decreasing acid strength: H2O, H2S, H2Se, H2Te
A) H2Te > H2Se > H2S > H2O
B) H2O > H2S > H2Se > H2Te
C) H2Se > H2Te > H2S > H2O
D) H2S > H2Te > H2Se > H2O
E) H2Se > H2S > H2Te > H2O
Q:
Which of the following is the strongest acid in aqueous solution?
A) H3AsO4
B) H3PO4
C) H3PO3
D) H3SbO4
E) H3AsO3
Q:
Which solution has the highest pH?
A) 0.10 MHBr(aq)
B) 0.10 MHI(aq)
C) 0.10 MHF(aq)
D) 0.10 MHCl(aq)
E) 0.10 MHClO4(aq)
Q:
Which of the following statements is incorrect?A) One reason why HCl is a stronger acid than HF is that the H-Cl bond is weaker than the H"F bond.B) F-is a stronger base than Cl-.C)One reason why HCl is a stronger acid than HF is that Cl is more electronegative than F.D) The acids HBr and HI both appear equally strong in water.E) One reason why HCl is a stronger acid than HF is that Cl has a larger atomic radius than F.
Q:
Rank the following in order of decreasing acid strength in aqueous solution: HCl, HOCl, HOBr, HOI.
A) HCl > HClO > HBrO > HIO
B) HIO > HBrO > HClO > HCl
C) HCl > HIO > HBrO > HClO
D) HClO > HCl > HBrO > HIO
E) HClO > HBrO > HCl > HIO
Q:
Which of the following statements is true concerning an aqueous solution of the strong acid HBr?A) Br-is a stronger acid than H2O.B) Br-is a stronger base than OH-.C) H3O+is a stronger acid than HBr.D) H2O is a stronger acid than HBr.E) H2O is a stronger base than Br".
Q:
Which of the following statements is true concerning an aqueous solution of the weak base NH3?A) OH-is a stronger base than NH3.B) OH-is a stronger acid than NH4+.C) NH4+is a stronger acid than H3O+.D) NH3is a weaker base than H2O.E) H2O is a stronger acid than H3O+.
Q:
Given equal concentrations of the following acids, which exhibits the greatest amount of ionization in water?
A) nitrous acid
B) chlorous acid
C) ascorbic acid
D) hydrobromic acid
E) citric acid
Q:
Which of the following reactions is not product-favored?A) NaOH(aq) → Na+(aq) + OH-(aq)B) NH3(aq) + H2O(l) → NH4+(aq) + OH-(aq)C) HClO4(aq) + H2O(l) → H3O+(aq) + ClO4-(aq)D) HCl(aq) + H2O(l) → H3O+(aq) + Cl-(aq)E) H2SO4(aq) + H2O(l) → H3O+(aq) + HSO4-(aq)
Q:
What is the leveling effect?
A) All bases are 100% ionized in water.
B) All acids are 100% ionized in solvents other than water.
C) All strong acids are 100% ionized in water.
D) An acid with a higher concentration in water has a lower pH than an acid with a lower concentration in water.
E) A base with a higher concentration in water has a lower pH than a base with a lower concentration in water.
Q:
The acid strength decreases in the series HBr > HSO4-> CH3COOH > HCN > HCO3-. Which of the following is the strongest base?A) SO42-B) CO32-C) CH3COO-D) Br-E) CN-
Q:
Which of the following acids has the strongest conjugate base?A) HClOB) HClO4C) HClO2D) HClO3E) HCl
Q:
Which of the following acids has the weakest conjugate base in aqueous solution?A) CH3COOHB) HOClC) HFD) HNO2E) HClO4
Q:
Which of the following concerning the relative strength of acids and bases is/are correct?
1) As the acidity of the acid decreases, the basicity of the conjugate base increases.
2) The hydronium ion is the strongest acid that can be found in aqueous solution.
3) All acids classified as strong acids in aqueous solution have the same acidity in a more acidic solvent like acetic acid.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1, 2, and 3