ライフサイエンスコーパス: aq

1 we compared the reaction rates between Hg(0)aq and a number of selected organic ligands with varying

2 xhibited little or no reactivity toward Hg(0)aq either at pH 7.

3 suggest that thiol-induced oxidation of Hg(0)aq is important under anoxic conditions and can affect H

4 gher thiol/Hg ratios resulted in higher Hg(0)aq oxidation rates than larger aromatic thiols at lower

5 The rate and extent of Hg(0)aq oxidation varied greatly depending on the chemical an

6 Significant Hg(0)aq oxidation was observed with all thiols but not with l

7 to assess the role of these ligands in Hg(0)aq oxidation.

8 id) also led to substantially increased Hg(0)aq oxidation.

9 en dissolved aqueous elemental mercury (Hg(0)aq) and organic ligands in general, and thiol compounds

10 formation, and that the controlled Mn(OH)2 (aq) formation can affect the system's saturation and sub

11 We found that IS controls Mn(OH)2 (aq) formation, and that the controlled Mn(OH)2 (aq) form

12 a typical aqueous tracer ((198)Hg(NO(3))(2)(aq)).

13 tes and finally to the dilution of the CO(2)(aq) solution by diffusion.

14 solution of carbonate host rock by the CO(2)(aq) solution will slightly increase porosity, which may

15 The reactions of CO(2)(aq) with a series of linear and methyl substituted prima

16 rsible carbamate formation reaction of CO(2)(aq) with a series of substituted cyclic secondary amines

17 In terms of the forward reaction of CO(2)(aq) with amine, the order with increasing rate constants

18 ilibrium constants for the reaction of CO(2)(aq) with sterically hindered amines and (b) an attempt t

19 xperimental conditions (i.e., 0.1 mM Mn(2+) (aq) concentration and pH 10.1) were chosen to be relevan

20 ubly charged cations like Mg(2+)aq and Ca(2+)aq, induce a localization of the H(+)aq hydration struct

21 particular doubly charged cations like Mg(2+)aq and Ca(2+)aq, induce a localization of the H(+)aq hyd

22 ent of silver by mercury: Ag(np) + 1/2Hg(2+)(aq) --> Ag(+)(aq) + 1/2Hg(l).

23 the dominant active catalyst and not Co(2+)(aq) or cobalt oxide.

24 Extraction of Co4POM, but not Co(2+)(aq) or CoOx into toluene from water, and other experimen

25 ecifically, we quantify the amount of Co(2+)(aq) released from Co4POM by two methods (cathodic adsorp

26 hat catalytic O2 evolution by Co4POM, Co(2+)(aq), and CoOx have different dependences on buffers, pH,

27 tive cleavage of DNA was observed for Cu(2+)(aq) under the conditions used, the kinetics of cleavage

28 < 5 from the reaction between NO2 and Fe(2+)(aq) present in thin films of water coating the surface,

29 saturated soils released more nPP and Fe(2+)(aq) than well-drained soils; whereas, nonreductive parti

30 producing MnOx minerals by oxidizing Mn(2+)(aq) at rates that are 3 to 5 orders of magnitude faster

31 This isolated MnxG shows activity for Mn(2+)(aq) oxidation to form manganese oxides.

32 minerals in the presence of uranyl (UO2)(2+)(aq) resulted in the preferential incorporation of U into

33 are responsible for the oxidation of Mn(2+)((aq)) to insoluble Mn(3+/4+) oxides (MnO(x)()) in natural

34 </=0.001 M) solutions of dissolved As(2)O(3)(aq) was pure c-GaAs(s) at much lower temperatures than 2

35 CH2Cl2, 0.02-0.04 in CH3CN, and <0.01 in 30% aq CH3CN.

36 ficiency for O(2) evolution in 1.0 M HClO(4)(aq) of nearly unity.

37 tive Au/Ag(UPD) electrode in 0.1 M H(2)SO(4)(aq) exhibit a primary stripping peak for the Ag UPD adla

38 ethyl)naphthalene with a mixture of [HBF(4)](aq) and (CF(3)CO)(2)O affords the corresponding dication

39 the removal of up to 99% of the added V(5+)(aq) and suggest microbial mediation.

40 measurements of deltaH(ACID) (gas) or pK(a) (aq).

41 fer of solutes from water to L-ascorbic acid(aq) have been calculated.

42 sions with higher Df), and the release of Ag(aq) increases.

43 at and below 20 mug L(-1) by adsorbing Ag(+)(aq).

44 by mercury: Ag(np) + 1/2Hg(2+)(aq) --> Ag(+)(aq) + 1/2Hg(l).

45 evaluated using methanol/water and aqueous (aq) solutions.

46 tants for the formation of Br(2)O and BrOCl (aq) have not been previously reported, we have calculate

47 oligonucleotide deprotection (55 degrees C, aq NH3) and was converted to a cyclonucleoside (14).

48 The polyatomic model of CF4(aq) studied gives a satisfactory description of the expe

49 ibutions to the hydration free energy of CF4(aq) that naturally arise from chemical contributions def

50 tested for the hydrophobic hydration of CF4(aq).

51 translate into Antarctic surface-water CO2 (aq) concentrations that are as much as 2.5 times higher

52 roduced in these analytical systems, and CO2(aq) to form the peroxycarbonate radical, *C04-.

53 ecreases under high CO2 concentrations ([CO2(aq)]) constituting a negative feedback.

54 bjected to coupled gradual increases in [CO2(aq)] and temperature over a few million generations in a

55 can be extracted from the molalities of CO2(aq) and HCO3(-).

56 L is supported by direct manipulation of CO2(aq) concentrations by the addition of CO2(g) or carbonic

57 s completely quenched in the presence of CO2(aq).

58 three dissolved inorganic carbon species CO2(aq), HCO3(-), and CO3(2-) of alkaline solutions under hi

59 r dilutable metabolite provided by Comamonas aq. that regulates gene expression, accelerates developm

60 tment of the intermediate epoxide with concd aq H2SO4 promoted highly regioselective ring-opening (di

61 ides were deprotected under mild conditions (aq ammonia-EtOH, rt).

62 Cr(aq)OO(2+) reacts with NO(2) with k = 2.3 x 10(8) M(-1) s

63 with Cr(aq)OO(2+), a species accompanying Cr(aq)O(2+) in our preparations.

64 *) reaction yielded isobutene, CO(2), and Cr(aq)(3+), in addition to chromate.

65 The reaction between Cr(aq)O(2+) and NO generates Cr(aq)ONO(2+), k > 10(4) M(-1)

66 he kinetics of the rapid reaction between Cr(aq)OO(2+) and NO were determined by laser flash photolys

67 A superoxochromium complex Cr(aq)OO(2+) reacts with acetylperoxyl radicals, CH(3)C(O)O

68 NO(3)(-) and a chromium nitrato complex, Cr(aq)ONO(2)(2+).

69 initially produced peroxynitrito complex, Cr(aq)OONO(2+), undergoes O-O bond homolysis followed by so

70 tion between Cr(aq)O(2+) and NO generates Cr(aq)ONO(2+), k > 10(4) M(-1) s(-1).

71 The aquachromyl(IV) ion, Cr(aq)O(2+), reacts with acetaldehyde and pivaldehyde by hy

72 identified as a nitritochromium(III) ion, Cr(aq)ONO(2+), is a precursor to a portion of free NO(2)(-)

73 eaction toward superoxochromium(III) ion, Cr(aq)OO(2+).

74 ss NO, the stoichiometry changes to [NO]/[Cr(aq)OO(2+)] = 3:1, and the reaction produces close to 3 m

75 e determined by laser flash photolysis of Cr(aq)NO(2+) in O(2)-saturated acidic aqueous solutions, k

76 by some known and some novel chemistry of Cr(aq)O(2+) and NO(2).

77 radical coupling at the remote oxygen of Cr(aq)OO(2+), followed by elimination of O(2) and formation

78 radical coupling at the remote oxygen of Cr(aq)OO(2+), followed by elimination of O(2) and formation

79 produces close to 3 mol of nitrite/mol of Cr(aq)OO(2+).

80 The Cr(aq)OO(2+)/C(CH(3))(3)C(O)OO(*) reaction yielded isobuten

81 The rate constant for the Cr(aq)OO(2+)/CH(3)C(O)OO(*) cross reaction, k(Cr) = 1.5 x 1

82 With limiting NO, the Cr(aq)OO(2+)/NO reaction has a 1:1 stoichiometry and produc

83 (*) in parallel with the decomposition to Cr(aq)O(2+) and (*)NO2, both of which were identified in st

84 In the suggested mechanism, the transient Cr(aq)OOOO(O)CC(CH(3))(3)(2+) branches into two sets of pro

85 In the next step, the radicals react with Cr(aq)OO(2+), a species accompanying Cr(aq)O(2+) in our pre

86 r disproportionates and ultimately yields Cr(aq)(3+) and HCrO(4)(-).

87 ntrolling aqueous uranium concentrations (cU(aq)).

88 sults and measured data reveals that high cU(aq) and its depth-specific distribution depending on red

89 ll-front mobilization and results in high cU(aq) within the redoxcline.

90 background uranium concentrations (median cU(aq) < 0.5 mug L(-1)).

91 , the modeling results indicate that peak cU(aq) occurring at this redox front increase along with th

92 g-Western Pomerania (Germany) reveal peak cU(aq) up to 75 mug L(-1) but low background uranium concen

93 ng such groundwater contamination by peak cU(aq), we reanalyzed measured redox potentials and total c

94 The rhodium hydride (Rh-D)(aq) and rhodium hydroxide (Rh-OD)(aq) bond dissociation

95 e corresponding alcohols with DDQ/THF or DDQ/aq THF in excellent yields.

96 tion (IFEaq) and deprotonation (DeltaGdeprot,aq) free energies were estimated using thermochemical cy

97 chanism depending upon pH since DeltaGdeprot,aq<BDFEaq and ETFEaqBDFEaq.

98 BDFEaq has been correlated with DeltaGdeprot,aq and ETFEaq with r=0.74 and 0.87 respectively.

99 r of light energy into solvated electrons (e(aq)(-)), and (2) as an acceptor of an electron to create

100 f redox reactions involving reduction by e(-)aq generated by the electron beam during in situ liquid

101 tion experiments, the hydrated electrons e(-)aq created by the electron beam are responsible for the

102 he concentration of hydrated electrons, [e(-)aq].

103 imaging can be used to measure not only [e(-)aq] but also the rate of reduction of a metal-ion comple

104 ve suggested that the aqueous electron, e(-)(aq), may play a significant role in the radiation chemis

105 lt to distinguish, experimentally, from e(-)(aq) in bulk water, using either optical absorption or ph

106 t significantly different from those of e(-)(aq) in bulk water and as such are incompatible with diss

107 toring forces on the water molecules of e(-)(aq), which suggests that the outlying proton is a poor h

108 cs to induce DNA strand breaks, whereas e(-)(aq) in bulk water lies too far below the vacuum level to

109 ron rich environment, usually designated FeS(aq), and its role in controlling solubility of different

110 species, both of which can be processed from aq solution.

111 The centrosymmetric H(aq)(+) ions are linked via short H bonds, forming a true

112 longer O...O separations than in discrete H(aq)(+) ions, indicating greater delocalization of positi

113 Three different types of H(aq)(+) clusters are found in these tubes: a symmetrical

114 rystallizes in nanometer-diameter tubes of H(aq)(+) enclosed by walls of carborane anions.

115 ese results will change the description of H(aq)(+) in textbooks of chemistry, and a more extensive d

116 All of the H(aq)(+) cations show unexpectedly longer O...O separation

117 The hydrogen ion in water, H(aq)(+), is a unique H(13)O(6)(+) entity that defines the

118 d Ca(2+)aq, induce a localization of the H(+)aq hydration structures.

119 2O)n, serve as finite model systems for H(+)(aq), which are amenable to highly sensitive and selectiv

120 nsistent molecular level description of H(+)(aq).

121 The excess proton in water, H(+)(aq), plays a fundamental role in aqueous solution chemis

122 ydrolysis of water: Me2+aq --> [MeOH]+aq + H+aq.

123 wn in a chemostat with 65 microM of added H2(aq) .

124 nt density of -10 mA cm(-2) in 0.500 M H2SO4(aq).

125 itu and operando conditions in 0.500 M H2SO4(aq).

126 In 1 N HBr (aq), the photocatalyst undergoes excited-state electron

127 oxide-covered GaAs nanocrystals with 6 M HCl(aq).

128 lemental selenium, and (iii) addition of HCl(aq).

129 olkg(-1) thiamine HCl(aq) and pyridoxine HCl(aq) solutions over temperature range (288.15-318.15)K at

130 , 0.15, 0.25 and 0.35)molkg(-1) thiamine HCl(aq) and pyridoxine HCl(aq) solutions over temperature ra

131 ple, E(+/)*, in 0.1 M perchloric acid (HClO4(aq)) to be tuned from -0.69 to -1.03 V vs NHE.

132 treatment of soil organic matter with 2% HF(aq) dramatically reduces this problem but may generate s

133 mple of the soil that was treated with 2% HF(aq).

134 e porous Si from the reaction of V2 O5 in HF(aq) as Ox1 and H2 O2 (aq) as Ox2 with Si powder and wafe

135 structural alterations that accompany the HF(aq) treatment, as indicated by the 13C NMR data.

136 composition study of the Ag(2)O/V(2)O(5)/HF((aq)) ternary system, leading to the precipitation of eit

137 -10.0 for the reaction HgS(s) + H2O = HgOHSH(aq) as reported by Dyrssen and Wedborg (1991).

138 This moderates the concentration of HI(aq) and so facilitates catalytic turnover via neutral 4.

139 1)](-)H(3)O(+) and catalyzes the reaction HI(aq) + MeOAc --> MeI + HOAc.

140 possible reassessment of NIST-certified Ho3+(aq) band locations.

141 all of the instruments to the consensus Ho3+(aq) band locations.

142 AMET) have evaluated the performance of Ho3-(aq)-based Certified Reference Materials (CRMs) under "ro

143 icantly greater than when reacted with Ag(I)(aq) alone.

144 imal reactivity between azurin and the Ag(I)(aq) species formed as a result of NP oxidative dissoluti

145 was determined by measuring effluent Fe(II) (aq) concentration and by spectroscopically monitoring th

146 s determined from fitting the delta(56)Fe(II)aq (1.79 per thousand and 2.15 per thousand) and the del

147 e and some lepidocrocite; oxidation of Fe(II)aq alone favored lepidocrocite.

148 on potential (EH) of the Fe(III) oxide/Fe(II)aq redox couple as a function of dissolved Fe(II) where

149 equilibration of sorbed iron and with Fe(II)aq using published fractionation factors, is consistent

150 ynechococcus PCC 7002, aqueous Fe(II) (Fe(II)aq) is oxidized and precipitated as amorphous Fe(III) ox

151 ith complete equilibrium exchange with Fe(II)aq.

152 heavier delta(56)Fe compositions than Fe(II)aq.

153 magnetite was induced via addition of Fe(II)aq.

154 with solutions containing nPbO2(s) or Pb(II)aq in different water matrices for 7-14 days to investig

155 Prolonged presence of S(-II)aq in experiments with hematite in combination with a la

156 pared to lepidocrocite, consumption of S(-II)aq proceeded slower with hematite, but yielded maximum d

157 essed when exposed to aqueous sulfide (S(-II)aq) at pH 8.0.

158 rtality was decreased in the order of Fe(II)(aq) > CMC-nZVI > nZVI > nFe(3)O(4).

159 )-R2 complex from the apo protein and Fe(II)(aq) (k(obs) = 0.29 +/- 0.03 s(-1)), which is the slowest

160 Relative to oxidation of Fe(II)(aq) alone, both goethite and gamma-Al2O3 surfaces increa

161 subchronic exposure to nFe(3)O(4) or Fe(II)(aq) at environmentally relevant concentrations (0.5-5 mg

162 and reactive oxygen species (ROS) and Fe(II)(aq) production, thus increasing mortality and oxidative

163 modern sediments may reflect greater Fe(II)(aq) utilization and variations in source composition.

164 Fe isotope excursions reflect partial Fe(II)(aq) utilization during abiotic pyrite formation rather t

165 ombined fractionation factors between Fe(II)(aq), mackinawite, and pyrite permit the generation of py

166 oavailable than suspended CMC-nZVI or Fe(II)(aq).

167 on oxide (nFe(3)O(4)) or ferrous ion [Fe(II)(aq)] at mug/L-mg/L levels to assess the causal toxic eff

168 further evidence of the importance of Mn(II)(aq)-MnO2(s) interactions and the attendant production of

169 were associated with production of Pu(III)((aq)).

170 l reactivity investigated by irradiations in aq CH3OH.

171 salts reveal the presence of two isomers in aq solutions.

172 liminated upon photolysis of the quinones in aq CH3CN to produce an o-quinone methide intermediate th

173 rosiloxane (PMHS) made hypercoordinate by KF(aq) allows Me(3)SnH to be recycled during a Pd(0)-cataly

174 metal hydroxide by hydrolysis of water: Me2+aq --> [MeOH]+aq + H+aq.

175 de by hydrolysis of water: Me2+aq --> [MeOH]+aq + H+aq.

176 ctive species that forms upon binding of Mn2+aq to apo-WOC.

177 horothioate (pNPPT), from water to 0.6 (mol) aq DMSO (60 mol % water in DMSO) were measured calorimet

178 faces, i.e., sDNNS(-) (DCE) + protamine(n+) (aq) right harpoon over left harpoon protamine-DNNS compl

179 ccurs readily under basic conditions (R(3)N, aq pK(a) > 9) at t < 25 degrees C to give a variety of p

180 nt molar enthalpy function (L(phi)) for NaCl(aq) varies strongly and nonlinearly with concentration i

181 IC experiments involving duplex DNA in NaCl(aq) using molecular dynamics (MD) simulation, the three-

182 perties of the glassy carbon (GC)|0.2 M NaOH(aq) interface as a function of the applied potential, E.

183 of I(2), 4 h, 110 degrees C; 2nd step, NaOH(aq), 1 h, 100 degrees C) resulted in the formation of im

184 e injections is even better (n = 1520, [NH4+(aq)] = 2.5 microM, RSD = 2%).

185 pptv (15 nM for 500 microL of injected NH4+(aq)) with an inexpensive light emitting diode photodiode

186 n catalyst that forms as a thin film from Ni(aq)(2+) solutions containing borate electrolyte (Ni-B(i)

187 hanism of Fe(3+) loading of Fbp from Fe(NTA)(aq) in the presence of phosphate at pH 6.5.

188 eaction of V2 O5 in HF(aq) as Ox1 and H2 O2 (aq) as Ox2 with Si powder and wafers.

189 and the driving force for formation of O2.- (aq), which increases as cluster-anion charge becomes mor

190 ide (Rh-D)(aq) and rhodium hydroxide (Rh-OD)(aq) bond dissociation free energies for [(TSPP)Rh-D(D(2)

191 Of the methods tested, the analysis of aq LS containing electrolytes was simplest by LS DESI MS

192 Tb(OH)(aq)(2+) also reports a likely location of this binding s

193 It is striking that micromolar Tb(OH)(aq)(2+) concentrations are compatible with tertiary fold

194 he lanthanide metal ion terbium(III), Tb(OH)(aq)(2+), reversibly inhibit the ribozyme by competing fo

195 reasing cluster size (the onset of the PH(+)(aq) fluorescence spectrum is 600 nm and the maximum is 5

196 ted particulate Po (Po(p)): dissolved Po (Po(aq)) ratios in the cultures, consistent with efficient P

197 ess, PPI(+)(PrOH) + H3O(+) --> PPII(2+)(PrOH/aq) + H2O, we determine DeltaG = -20 +/- 19 kJ.mol(-1),

198 PPII(+)(PrOH/aq) + H3O(+) --> PPII(2+)(PrOH/aq) +H2O.

199 -435 +/- 70 J.mol(-1).K(-1) for PPII(+)(PrOH/aq) + H3O(+) --> PPII(2+)(PrOH/aq) +H2O.

200 minor process, PPI(+)(PrOH) --> PPII(+)(PrOH/aq) without protonation, we determine DeltaG = -9 +/- 20

201 However, Pu((aq)) increased by an order of magnitude in some treatmen

202 ng the dissociation of dissolved acids RCOOH(aq).

203 d to be K(T)(gas) = 2.768 x 10(-12) and K(T)(aq) = 5.469 x 10(-14).

204 azolyl)quinoline (Quinox) as ligand and TBHP(aq) as oxidant to deliver single ketone constitutional i

205 d, quinoline-2-oxazoline (Quinox), and TBHP((aq)) as the terminal oxidant provides good yields of the

206 of O(2) and formation of CH(3)COOH and Cr(V)(aq)O(3+).

207 of O(2) and formation of CH(3)COOH and Cr(V)(aq)O(3+).

208 genic sites, the origin of high delta53Cr(VI)aq is tentatively ascribed to preferential release of 53

209 dominated and industrial sites, delta53Cr(VI)aq was shifted toward higher values, compared to the pol

210 Ferrihydrite was exposed to Tc(VII)(aq) containing cement leachates (pH 10.5-13.1), and crys

211 fluoroacetate salts which, on treatment with aq NaOH, provide the free amines.

212 oiety with TFA, and immediate treatment with aq.

213 indqvist-type [H(x)()Nb(6)O(19)](8)(-)(x)()((aq)) polyoxoanion and aqueous solution as a function of