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59 Cards in this Set
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According to the Arrhenius concept, an acid is a substance that ________. a. is capable of donating one or more H+ b. causes an increase in the concentration of H+ in aqueous solutions c. can accept a pair of electrons to form a coordinate covalent bond d. reacts with the solvent to form the cation formed by autoionization of that solvent e. tastes bitter |
b. causes an increase in the concentration of H+ in aqueous solutions
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A Bronsted-Lowry base is defined as a substance that _______. a. increases [H+] when placed in H2O b. decreases [H+] when placed in H2O c. increases [OH-] when placed in H2O d. acts as a proton acceptor e. acts as a proton donor |
d. acts as a proton acceptor
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A Bronsted-Lowry acid is defined as a substance that _______. a. increases [H+] when placed in H2O b. decreases [H+] when placed in H2O c. increases [OH-] when placed in H2O d. acts as a proton acceptor e. acts as a proton donor |
e. acts as a proton donor
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A substance that is capable of acting as both an acid and a base is _______. a. autosomal b. conjugated c. amphoteric d. saturated e. miscible |
c. amphoteric |
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The molar concentration of hydronium ion in pure water at 25C is ______. a. 0.00 b. 1.0 X 10^-7 c. 1.0 X 10^-14 d. 1.00 e. 7.00 |
b. 1.0 X 10^-7
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The molar concentration of hydroxide ion in pure water at 25C is ______. a. 1.00 b. 0.00 c. 1.0 X 10^-14 d. 1.0 X 10^-7 e. 7.00 |
d. 1.0 X 10^-7
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The magnitude of Kw indicates that ______. a. water autoionizes very slowly b. water autoionizes very quikly c. water autoionizes only to a very small extent d. the autoionization of water is exothermic |
c. water autoionizes only to a very small extent
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The concentration of water in pure water is approximately ______ M. a. 18 b. 100 c. 55 d. 0.100 e. 83 |
c. 55 |
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In basic solution, ________. a. [H3O+] = [OH-] b. [H3O+] > [OH-] c. [H3O+] < [OH-] d. [H3O+] = 0M e. [OH-] > 7.00 |
c. [H3O+] < [OH-]
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Which solution below has the highest concentration of hydroxide ions? a. pH = 3.21 b. pH = 12.6 c. pH = 7.93 d. pH = 9.82 e. pH = 7.00 |
b. pH = 12.6
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Which one of the following statements regarding Kw is false? a. pKw is 14.00 at 25C b. the value of Kw is always 1.0 X 10^-14 c. Kw changes with temperature d. the value of Kw shows that water is a weak acid e. Kw is known as the ion product of water |
b. the value of Kw is always 1.0 X 10^-14
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The hydride ion, H-, is a stronger base than the hydroxide ion, OH-. The product(s) of the reaction of hydride ion with water is/are _______. a. H3O+(aq) b. OH-(aq) + H2(g) c. OH-(aq) + 2 H+(aq) d. no reaction occurs e. H2O2(aq) |
b. OH-(aq) + H2(g)
-H+ H- + H2O --> OH- + H2 |
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An aqueous solution contains 0.100 M NaOH. The solution is _____. a. very dilute b. highly colored c. basic d. neutral e. acidic |
c. basic |
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Nitric acid is a strong acid. This means that ____. a. aqueous solutions of HNO3 contain equal concentrations of H+(aq) and OH-(aq) b. HNO3 does not dissociate at all when it is dissolved in water c. HNO3 dissociates completely to H+(aq) and NO3-(aq) when it dissolves in water d. HNO3 produces a gaseous product when it is neutralized e. HNO3 cannot be neutralized by a weak base |
c. HNO3 dissociates completely to H+(aq) and NO3-(aq) when it dissolves in water
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Of the following acids, ______ is not a strong acid. a. HNO2 b. H2SO4 c. HNO3 d. HClO4 e. HCl |
a. HNO2
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Of the following, ____ is a weak acid. a. HF b. HCl c. HBr d. HNO3 e. HClO4 |
a. HF
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Which of the following is the weakest acid? a. HF (Ka=6.8x10^-4) b. HClO (Ka=3.0x10^-8) c. HNO2 (Ka=4.5x10^-4) d. HCN (Ka=4.9x10^-10) e. acetic acid (Ka=1.8x10^-5) |
d. HCN (Ka=4.9x10^-10)
smallest Ka |
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Of the acids in the table below, _______ is the strongest acid. Acid Ka HOAc 1.8x10^-5 HCHO2 1.8x10^-4 HClO 3.0x10^-8 HF 6.8x10^-4 a. HOAc b. HCHO2 c. HClO d. HF e. HOAc and HCHO2 |
d. HF biggest Ka |
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Which of the following is a Bronsted-Lowry acid? a. (CH3)3NH+ b. CH3COOH c. HF d. HNO2 e. all of the above |
e. all of the above
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Classify the following compounds as weak acids (W) or strong acids (S): nitrous acid hydrochloric acid hydrofluoric acid a. W W W b. S S S c. S W W d. W S S e. W S W |
e. W S W
nitrous acid HNO3 (W) hydrochloric acid HCL (S) hydrofluoric acid HF (W) |
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Classify the following compounds as weak acids (W) or strong acids (S):
hypochlorous acid perchloric acid chloric acid a. W S S b. S S S c. S W W d. W W W e. W S W |
a. W S S
hypochlorous acid HClO (W) perchloric acid HClO4- (S) chloric acid HClO3 (S) |
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Ammonia is a ______ . a. weak acid b. strong base c. weak base d. strong acid e. salt |
c. weak base
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HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kb for A-? a. HA(aq) + H2O(l) <--> H2A+(aq) + OH-(aq) b. A-(aq) + H3O+(l) <--> HA(aq) + H2O(l) c. HA(aq) + OH-(aq) <--> H2O(l) + H+(aq) d. A-(aq) + H2O(l) <--> HA(aq) + OH-(aq) e. A-(aq) + OH-(aq) <--> HOA-2(aq) |
d. A-(aq) + H2O(l) <--> HA(aq) + OH-(aq)
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Classify the following compounds as weak bases (W) or strong bases (S): ammonia flouride ion sodium hydroxide a. W W S b. S S S c. S W W d. W S S e. W S W |
a. W W S
ammonia NH3 (W) flouride ion F (W) sodium hydroxide NaOH- (S) |
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Which of the following ions will act as a weak base in water? a. OH- b. Cl- c. NO3- d. ClO- e. none of the above will act as a weak base in water |
d. ClO-
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Which of the following aqueous solutions has the highest {OH-]? a. a solution with a pH of 3.0 b. a 1x10^-4 M solution of HNO3 c. a solution with a pOH of 12.0 d. pure water e. a 1x10^-3M solution of NH4Cl |
d. pure water
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A 0.0035 M aqueous solution of a particular compound has a pH=2.46. The compound is _______. a. a weak base b. a weak acid c. a strong acid d. a strong base e. a salt |
c. a strong acid |
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Of the following substances, an aqueous solution of _______ will form basic solutions. NH4Cl Cu(NO3)2 K2CO3 NaF a. NH4Cl, Cu(NO3)2 b. K2CO3, NH4Cl c. NaF only d. NaF, K2CO3 e. NH4Cl only |
d. NaF, K2CO3
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A 0.1M aqueous solution of _____ will have a pH of 7.0 at 25C. NaOCl KCl NH4Cl Ca(OAc)2 a. NaOCl b. KCl c. NH4Cl d. Ca(OAc)2 e. KCl and NH4Cl |
b. KCl
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A 0.1M solution of ______ has a pH of 7.0. a. Na2S b. KF c. NaNO3 d. NH4Cl e. NaF |
c. NaNO3
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An aqueous solution of _______ will produce a basic solution. a. NH4ClO4 b. KBr c. NaCl d. NaHSO4 e. Na2SO3 |
e. Na2SO3
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Of the following, which is the strongest acid? a. HIO b. HIO4 c. HIO2 d. HIO3 e. the acid strength of all of the above is the same |
b. HIO4
has the most O's |
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Which of the following acids will be the strongest? a. H2SO4 b. HSO4- c. H2SO3 d. H2SeO4 e. HSO3- |
a. H2SO4
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Of the following, which is the strongest acid? a. HClO b. HClO3 c. HClO2 d. HClO4 e. HIO |
d. HClO4
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HCl |
SA |
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H2SO4 |
SA |
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HNO3 |
SA |
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HBr |
SA |
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HI |
SA |
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HClO3 |
SA |
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HClO4 |
SA |
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CH3- |
SB |
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H- |
SB |
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O-2 |
SB |
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NaOH |
SB |
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KOH |
SB |
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Ca(OH)2 |
SB |
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Sr(OH)2 |
SB |
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Ba(OH)2 |
SB |
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HF |
WA |
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HNO2 |
WA |
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C6H5COOH |
WA |
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CH3COOH |
WA |
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HClO |
WA |
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HCN |
WA |
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HOC6H5 |
WA |
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NH3 |
WB |
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In which of the following aqueous solutions does the weak acid exhibit the highest percentage ionization? a. 0.01 M HC2H3O2 (Ka=1.8x10^-5) b. 0.01 M HNO2 (Ka=4.5x10^-4) c. 0.01 M HF (Ka=6.8x10^-4) d. 0.01 M HClO (Ka=3.0x10^-8) e. these will all exhibit the same percentage ionization |
c. 0.01 M HF (Ka=6.8x10^-4)
Biggest Ka |
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Of the compounds below, a 0.1 M aqueous solution of _____ will have the highest pH. a. KCN, Ka of HCN=4.0x10^-10 b. NH4NO3, Kb of NH3=1.8x10^-5 c. NaOAc, Ka of HOAc=1.8x10^-5 d. NaClO, Ka of HClO=3.2x10^-8 e. NaHS, Kb of HS-=1.8x10^-7 |
a. KCN, Ka of HCN=4.0x10^-10
smallest Ka/Kb = highest pH |
