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 There was no evidence of Hg(0)((aq)) abundance directly limiting mercury methylation.

11 A ubiquitous pathway for Hg(0)((aq)) formation was not identified based on geochemical d

12 reasing the concentration of volatile Hg(0)((aq)) relative to Hg(II)(i).

13 The concentration ratio of Hg(0)((aq)) to Hg(II)(i) exhibited an inverse relationship to H

14 o volatile dissolved gaseous mercury (Hg(0)((aq))) and toxic methylmercury (MeHg) govern mercury bioa

15 f aqueous mercury species (Hg(II)(i), Hg(0)((aq)), MeHg) and relevant geochemical constituents in por

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

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

18 ated by H(2)CO(3)* (which includes both CO(2(aq)) and H(2)CO(3)) at moderately alkaline pH conditions

19 ne, ethane, >C4 compounds, and possibly CO(2(aq)) and methane.

20 em behavior and 22% molar conversion of CO(2(aq)) to methane.

21 ate constants for e(aq)(-) quenching by CO(2(aq)), measured in acidic solutions equilibrated with CO(

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

23 CO(2) dissolved in aqueous solutions CO(2)(aq) is important to CO(2) capture, storage, photo-/elect

24 icient epsilon was derived for in situ CO(2)(aq) quantification up to 58 atm.

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

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

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

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

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

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

31 nm) of 5-100 mM PA under steady state [O(2)(aq)] = 260 muM (1.0 <= pH <= 4.5) for photon fluxes betw

32 is directly proportional to both the SiO(2)(aq) concentration and temperature of serpentinization.

33 silica-secreting organisms, elevated SiO(2)(aq) concentrations in Precambrian seawater would have ge

34 ucture, which itself is caused by low SiO(2)(aq) concentrations in serpentinizing fluids derived from

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

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

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

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

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

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

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

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

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

44 < 5 from the reaction between NO2 and Fe(2+)(aq) present in thin films of water coating the surface,

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

46 d growth of hematite by modifying the Fe(2+)(aq)/Fe(3+)(aq) ratio at the reaction interface.

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

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

49 x reactions, such as the oxidation of Mn(2+)(aq) to Mn(IV) oxide solids.

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

51 using ferrihydrite (2.0 g L(-1)) and Fe(2+)((aq)) (200 muM) for comparison.

52 on magnetite and siderite, and with Fe(2+)((aq)) reaction products.

53 Fe(2+)((aq)) was either added (type I) or formed through hematit

54 Removal during reaction with Fe(2+)((aq)) was observed after 8 h, concomitant with precipitat

55 In the presence of both hematite and Fe(2+)((aq)), NTO was quantitatively reduced to 3-amino-1,2,4-tr

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

57 3) from an aqueous phase of varying NO(3(-) (aq)) concentration with tributyl phosphate (TBP) in dode

58 </=0.001 M) solutions of dissolved As(2)O(3)(aq) was pure c-GaAs(s) at much lower temperatures than 2

59 occurring as dihydrogen polonate (H(2)PoO(3)(aq)) or, under strongly reducing conditions, as a hydrog

60 hematite by modifying the Fe(2+)(aq)/Fe(3+)(aq) ratio at the reaction interface.

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

62 Pulses of high CH(4(aq)) concentration coincide with supraglacially forced s

63 d mean; range from 2.4 to 11 tonnes) of CH(4(aq)) transported laterally from the ice-sheet bed.

64 xport of methane-supersaturated waters (CH(4(aq))) from the ice-sheet bed during the melt season.

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

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

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

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

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

70 Extraction of hop samples with 70% acetone (aq) followed by a C-18 Solid Phase Extraction yielded po

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

72 5, 0.09 and 0.13) mol kg(-1) nicotinic acid((aq)) (vitamin B3) solutions have been investigated by ex

73 ded in 1 x 10(-4) mol kg(-1) nicotinic acid((aq)) solutions.

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

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

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

77 AgNP correlates with the formation of AgCl((aq)), suggesting that it is the most photoactive species

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

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

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

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

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

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

84 result of the multiphase reaction of Cl(-)((aq)) with ClONO(2), formed from the reaction of ClO and

85 s of pH, initial cobalt to iron ratios ([Co](aq)/[Fe](aq)), with/without S(0), and the presence/absen

86 the exact phase being dependent on the [Co](aq)/[Fe](aq) value.

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

132 energy of the ion transfer reaction (DeltaG('aq->org)) and water-1,2-dichloroethane partition coeffic

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

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

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

136 e experiment employing chloroacetate as an e(aq)(-) probe revealed that continued e(aq)(-) exposure a

137 q)(-) exposure abates DOM chromophores and e(aq)(-) scavenging capacity over a several hour time scal

138 applied to a diluted AFFF to characterize e(aq)(-) reactions with 15 PFASs identified by liquid chro

139 an e(aq)(-) probe revealed that continued e(aq)(-) exposure abates DOM chromophores and e(aq)(-) sca

140 /F exchange pathways in hydrated electron (e(aq)(-))-induced PFOA degradation were revealed.

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

142 ultraviolet-generated hydrated electrons (e(aq)(-)).

143 s (ARPs) that generate hydrated electrons (e(aq)(-); e.g., UV-sulfite) have emerged as a promising re

144 ates strongly reducing hydrated electrons (e(aq)(-); NHE = -2.9 V) that have been shown to effectivel

145 ply previously reported rate constants for e(aq)(-) quenching by CO(2(aq)), measured in acidic soluti

146 es-specific bimolecular rate constants for e(aq)(-) quenching by H(2)CO(3)*, HCO(3)(-), and CO(3)(2-)

147 termediates or unreactive end-products via e(aq)(-) reactions with precursor structures in AFFF.

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

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

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

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

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

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

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

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

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

157 with hydroxide bridges have lower DeltaH(f,(aq)) and are more stable than those containing only pero

158 able than wheel-like clusters, and DeltaH(f,(aq)) can be accurately estimated using only DeltaH(f,(c)

159 alpy of formation of aqueous POMs (DeltaH(f,(aq))), and enthalpy of formation of POM crystals (DeltaH

160 the probable oxidative behavior of iron (Fe(aq)(2+) -> Fe(surf)(3+)) in clay minerals are fundamenta

161 t phase being dependent on the [Co](aq)/[Fe](aq) value.

162 initial cobalt to iron ratios ([Co](aq)/[Fe](aq)), with/without S(0), and the presence/absence of sul

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

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

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

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

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

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

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

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

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

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

173 2O)n, serve as finite model systems for H(+)(aq), which are amenable to highly sensitive and selectiv

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

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

176 gnificantly helping to compensate for (H(+))(aq)'s kinetic deficiency in sustaining the large proton

177 ncy is 10 to 20x greater than that of (H(+))(aq), often considered to be the major protonating agent

178 order of magnitude more abundant than (H(+))(aq) in the blood plasma and in the oceans.

179 r, CA is about 70x more abundant than (H(+))(aq) in the blood plasma, where we argue that its overall

180 ile CA is somewhat less reactive than (H(+))(aq), it is more than 1 order of magnitude more abundant

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

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

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

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

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

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

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

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

189 , 0.15, 0.25 and 0.35)molkg(-1) thiamine HCl(aq) and pyridoxine HCl(aq) solutions over temperature ra

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

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

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

193 In each (CuO, MO(2))/bpy/HF(aq) (M = Ti, Zr, Hf) system, the polar noncentrosymmetri

194 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

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

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

197 -10.0 for the reaction HgS(s) + H2O = HgOHSH(aq) as reported by Dyrssen and Wedborg (1991).

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

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

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

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

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

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

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

205 The limit of detection (LOD) of Ag(I)(aq) was 14 +/- 6 mug L(-1), and measured dissolution rat

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

222 iculate goethite with (57)Fe-enriched Fe(II)(aq) and used atom probe tomography (APT) to resolve the

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

224 ges its structural Fe(III) atoms with Fe(II)(aq) is complicated by recrystallization models with unte

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

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

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

228 ommonly coexists with aqueous Fe(II) (Fe(II)(aq)), which accelerates recrystallization by coupled ele

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

230 In the presence of Fe(II)(aq), the abiogenic precipitates were composed of more cr

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

232 imilar to the isotopic composition of Fe(II)(aq).

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

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

235 (3)(2-) and Ca(2)UO(2)(CO(3))(3)) by Fe(II)((aq)), while ferrihydrite surface-catalyzed reduction of

236 from homogeneous U(VI) reduction by Fe(II)((aq)).

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

238 l reactivity investigated by irradiations in aq CH3OH.

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

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

241 ations in cells (C(free)) and embryos (C(int;aq)) based on nominal effect concentrations (C(nom)).

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

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

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

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

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

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

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

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

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

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

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

253 Cells assimilate nFeS((aq)) to meet Fe/S nutritional demands by mobilizing and

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

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

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

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

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

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

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

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

262 PND can produce up to 0.3 (Tg x yr(-1)) of (aq)SOA, assuming the average flux of the precursor at 0.

263 , oxidized TAs were the major components of (aq)SOAs.

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

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

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

267 er than aqueous phase concentration ([(*)OH](aq)).

268 ial of the ion transfer reaction (Delta(org)(aq)Phi(')), diffusion coefficients (D), formal free Gibb

269 nts than in the absence of bacteria (k(org)-(aq)2-MN = 0.01 +/- 0.003 cm h(-1)).

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

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

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

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

274 -435 +/- 70 J.mol(-1).K(-1) for PPII(+)(PrOH/aq) + H3O(+) --> PPII(2+)(PrOH/aq) +H2O.

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

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

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

278 sions (-56 Mg C km(-2) year(-1) ) and SigmaF(aq) (-28 Mg C km(-2) year(-1) ) reduced NEP by 13% and 7

279 y (NEP), fire-related C emissions and SigmaF(aq) (comprising both downstream transport and gaseous ev

280 monsoonal events-up to 39% of annual SigmaF(aq) was exported in one event.

281 ult in considerable aquatic C export (SigmaF(aq) ).

282 y tropics in the future will increase SigmaF(aq) and fire emissions, potentially further reducing the

283 l months during the dry season, while SigmaF(aq) significantly offset NEP during the wet season, with

284 room temperature in a green solvent system (aq.

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

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

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

288 contribute to the high yields of terpenoic (aq)SOAs reported previously.

289 fields at the active site indicates that the aq [EMIm][EtSO(4)] medium facilitates the reaction by pr

290 e cloud condensation nuclei activity of the (aq)SOA formed after the evaporation of water.

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

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

293 As(V)((aq)) species can react with available cations to form in

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

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

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

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

298 oiety with TFA, and immediate treatment with aq.

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

300 Aqueous vanadate (H(x)V(V)O(4)((3-x)-)((aq))) concentrations are often controlled by surface com