ライフサイエンスコーパス: H2SO4

1 H2SO4 had a profound hindering effect on Hg(0) uptake du

2 H2SO4-mediated one-pot stereocontrolled (4 + 2) annulati

3 -doped diamond electrode, using 0.30molL(-1) H2SO4 as supporting electrolyte.

4 86 and 1.40 V (vs. Ag/AgCl) in 0.1 mol L(-1) H2SO4 medium.

5 This process, predicated on oleum's (100% H2SO4 with excess SO3) ability to intercalate between in

6 characterized using cyclic voltammetry in a H2SO4 solution.

7 he intermolecular transfer of sulfuric acid (H2SO4) and sulfur trioxide (SO3) from an acidic sulfopep

8 However, sulfuric acid (H2SO4) can form on the external and internal surfaces of

9 er led to the suggestion that sulfuric acid (H2SO4) must photolyze at high altitudes.

10 ee radicals (sCIs) in gaseous sulfuric acid (H2SO4) production.

11 Sulfuric acid (H2SO4), bisulfate (HSO4(-)), and sulfate (SO4(2-)) are a

12 Sulfuric acid (H2SO4), formed from oxidation of sulfur dioxide (SO2) em

13 lted via neutralization of the anolyte acid, H2SO4, by reaction with the base mineral silicate at the

14 ple thermal drying of h-BN in Bronsted acids H2SO4, H3PO4, and HClO4.

15 cular interaction energy between HCOO(-) and H2SO4 through the electron delocalization and formation

16 ces of OSCs, with contributions from MSA and H2SO4 of a similar order of magnitude.

17 face, with opposite sign to S MIF in SO2 and H2SO4.

18 nt of the intermediate epoxide with concd aq H2SO4 promoted highly regioselective ring-opening (dista

19 ns in SBSL spectra from concentrated aqueous H2SO4 solutions.

20 dic polarization of Pt electrodes in aqueous H2SO4 leads to the formation of a surface oxide (PtO).

21 of LOD and LOQ for Pt electrodes in aqueous H2SO4 solutions that employs cyclic voltammetry and freq

22 f these epoxides upon treatment with aqueous H2SO4 proceeded by nucleophilic attack with inversion at

23 SO4, and Mg(HSO4)2 salt solutions as well as H2SO4 and HCl acid solutions are investigated by means o

24 )-hydride, which is then rapidly oxidized by H2SO4 to regenerate Pt(II)-X2.

25 O)(H2SO4)2 to form Pd(eta2-HSO4)(HSO4)2(CH3)(H2SO4) and Pd(eta2-HSO4)(HSO4)2(CH3CO)(H2SO4), respectiv

26 s found to be via oxidation of Pd(HSO4)(CH3)(H2SO4)2 and Pd(HSO4)(CH3CO)(H2SO4)2 to form Pd(eta2-HSO4

27 of a bisulfate ligand to form Pd(HSO4)(CH3)(H2SO4)2.

28 (CH3)(H2SO4) and Pd(eta2-HSO4)(HSO4)2(CH3CO)(H2SO4), respectively.

29 of Pd(HSO4)(CH3)(H2SO4)2 and Pd(HSO4)(CH3CO)(H2SO4)2 to form Pd(eta2-HSO4)(HSO4)2(CH3)(H2SO4) and Pd(

30 ill react with CO to produce Pd(HSO4)(CH3CO)(H2SO4)2.

31 The complex H2SO4-H2O has been observed by rotational spectroscopy i

32 ed with piranha solution (a mixture of concd H2SO4 and 30% H2O2) to increase the concentration of sil

33 ol-5-amines 5 with Et2NH and then with concd H2SO4 gives 5H-pyrazolo[3,4-e][1,2,4]dithiazine-3-carbon

34 f formed ethylene with the hot, concentrated H2SO4 solvent cleanly generate EtOSO3H as the initial pr

35 With more concentrated H2SO4 solutions (approximately 10(-2) M) and higher lase

36 ulti-wall carbon nanotubes (MWNTs) in dilute H2SO4 were sprayed onto both sides of a Nafion membrane

37 A film of dilute H2SO4 is formed on the top of two metal capillary tubes

38 solutions highly resemble that of the dilute H2SO4 solution (0.26 M) at a comparable pH.

39 utral oligosaccharides are doped with dilute H2SO4 solutions.

40 hough, by reoxidation of palladium by either H2SO4 or O2.

41 ngates by 0.07(2) A relative to that in free H2SO4, and the S=O bond involved in the secondary intera

42 ions case, particle formation potential from H2SO4 will drop by about two orders of magnitude compare

43 led nanotubes with either HNO3/H2SO4 or H2O2/H2SO4 mixtures produces the oxidized groups (O/C = 5.5-6

44 tract was examined in the strong acidic (HCl+H2SO4) solution.

45 obic condensation reactions promoted by HCl, H2SO4, or CH3CO2H.

46 s found during the reaction of THB with HCl, H2SO4, and HClO4, while HG from CH3COOH or TRIS buffer a

47 As a result, the population of (HCOO(-))(H2SO4) drops significantly at higher temperatures, rende

48 s demonstrate the existence of the (HCOO(-))(H2SO4) pair at an energy slightly below the conventional

49 pletion in the spectra assigned to (HCOO(-))(H2SO4), and has also been verified by ab initio molecula

50 ytes that are acidic, such as, KH2PO4, HNO3, H2SO4, etc.

51 of single-walled nanotubes with either HNO3/H2SO4 or H2O2/H2SO4 mixtures produces the oxidized group

52 er cleaning the surfaces for 10-20 cycles in H2SO4 on all materials but pyrolytic carbon (PyC).

53 f corresponding cyclohexanone derivatives in H2SO4/CH3CN.

54 Absorption of Hg in H2SO4 was unlikely a significant contributor, when Hg(0)

55 y electrochemical anodisation of tantalum in H2SO4-HF medium.

56 presence of two sulfuric acid molecules in (H2SO4)m x base x (H2O)6 clusters is always sufficient to

57 Under mild conditions, i.e., low H2SO4 concentration (approximately 10(-3) M) and thresho

58 In 1.00 M H2SO4, 1,10-phenanthroline-mono-N-oxide (phenO) is the s

59 t the reversible hydrogen potential in 0.1 M H2SO4 and 1.0 M KOH.

60 reement between Im chi((2)) spectra of 1.1 M H2SO4 and 1.1 M HCl acid solutions indicate that HSO4(-)

61 ction reaction (ORR) on Pt UME-NPEs in 0.1 M H2SO4 are also shown.

62 ed region relative to neat water, with 1.1 M H2SO4 being more enhanced than 1.1 M HCl.

63 the oxygen reduction reaction (ORR) in 0.5 M H2SO4 (Hg, Au, Ag, Cu, Pt, Pd, Pd80Co20, and Au60Cu40) u

64 activity in challenging acidic media (0.5 M H2SO4), showing a half-wave potential of 0.85 V vs RHE a

65 ormance after 35 hours of operation in 0.5 M H2SO4.

66 ER) under strongly acidic conditions (0.50 M H2SO4, pH 0.3).

67 h of sustained hydrogen production in 0.50 M H2SO4.

68 r in situ and operando conditions in 0.500 M H2SO4(aq).

69 current density of -10 mA cm(-2) in 0.500 M H2SO4(aq).

70 O-acetylation followed by 25 microL of 0.6 M H2SO4, 1 h at 80 degrees C for acid hydrolysis of PS pre

71 The sCI channel, however, contributes minor H2SO4 production compared with the conventional OH chann

72 atmospheric concentrations of gas phase MSA, H2SO4, and SO2 under current emissions of fossil fuel-as

73 4.1 +/- 0.1 by automatic additions of 0.01 N H2SO4 or Ca(OH)2.

74 nding alpha-ketoaldehydes by new a DMSO-NaBr-H2SO4 oxidation system in yields up to 90% within a shor

75 Samples with varying amounts of H2SO4 and NaCl were used to develop the new alpha, which

76 oach is used to examine how contributions of H2SO4 and MSA to particle formation will change in a lar

77 This work focuses on the effects of H2SO4 and O2 on the Hg(0) uptake capacity and reversibil

78 ively functionalized to the ethanol ester of H2SO4, ethyl bisulfate (EtOSO3H) as the initial product,

79 uncertainty associated with an evaluation of H2SO4 production from the sCI reaction channel is the la

80 In general, the maximum of H2SO4 production from the sCI channel is found in the la

81 eaned (oxidation) by boiling in a mixture of H2SO4 and HNO3 (3:1) at 200 degrees C for 2h to remove g

82 ficient causes significant overestimation of H2SO4 loss rates compared with H2SO4 production rates.

83 that excitation of vibrational overtones of H2SO4 and its hydrate in the near-infrared and visible l

84 ptimum conditions predicted: mobile phase of H2SO4 0.005 mol L(-1) solution, flow rate of 0.3 mL min(

85 inally, the production and the loss rates of H2SO4 are compared.

86 ent between the loss and production rates of H2SO4.

87 irradiation of aqueous solutions of H2O2 or H2SO4 to form HO(*) and H(*), respectively, and confirme

88 from primary sludge by acidification (HCl or H2SO4), followed by separation using centrifugation for

89 cocktail of ClSO3H (85-95% w/w) and HOAc or H2SO4.

90 water, and dilute acid (0.05 weight percent H2SO4).

91 Direct measurement by phenol-H2SO4 confirmed the presence of carbohydrate on recombin

92 is calibrated using two acid-base reactions: H2SO4 + HEPES buffer, and NaOH + HCl.

93 en the two principal reactants with solvent (H2SO4) molecules significantly affects the structure of

94 of SO2, which produces SO3 and subsequently H2SO4, an important constituent of aerosols and acid rai

95 m the interface or become trapped by surface H2SO4.

96 chemical shifts are reported for bulk SWNTs, H2SO4-treated SWNTs, SWNT-Nafion polymer composites, SWN

97 ric acid extraction with a yield higher than H2SO4 extraction resulted in a very branched pectin with

98 Cl group, 3.7 meq/liter below control in the H2SO4 group, and unchanged from control in the HNO3 grou

99 hanges reflect substantial distortion of the H2SO4 moiety in response to only a single water molecule

100 One of the H2SO4 protons forms a short, direct hydrogen bond to the

101 d a re-determination of the structure of the H2SO4 unit within the complex.

102 itial product, which further reacts with the H2SO4 solvent to generate ITA.

103 The acid hydrolysis, using H2SO4 as a catalyst, increases the ionic strength of the

104 e oxidation method (Fenton < (NH4)2S2O8 with H2SO4 < HNO3 with H2O2) the concentration of oxygen-cont

105 H3PO4, Fenton-like reaction, (NH4)2S2O8 with H2SO4 and HNO3 with H2O2 into a different surface oxidat

106 estimation of H2SO4 loss rates compared with H2SO4 production rates.

107 odation almost always leads to reaction with H2SO4 molecules.

108 d test are preincubation of the samples with H2SO4 before addition of the orcinol reagent, decreased

109 Thus, with H2SO4 and HNO3 the sole constraint on removal of the aci

110 aste water with boric acid, waste water with H2SO4) and food samples (pomegranate flower, organic pea