ライフサイエンスコーパス: formation constant

1 pported by experimentally determined complex formation constants and excellent fits of response curve

2 l data, we have determined the T-Hg-T bridge formation constant at 25 degrees C, K(1) = 8.92 +/- 0.42

3 It results from the high formation constants between phosphates and iron ions.

4 can be explained in light of changes in the formation constants between the ions and ionophores with

5 The respective M(II)(TPPS)(NO) formation constants calculated from k(on)/k(off) ratios

6 The resulting formation constants correspond well to literature values

7 text] where (CO(3))beta(1) is the PbCO(3)(0) formation constant, e(i) are molar absorptivity ratios,

8 f Fe2+ (1026 s(-1)) corresponded well to the formation constant for the Fe3+-tyrosinate complex (920

9 rane) decrease as [PVC] increases, while the formation constants for the complex of the solute with i

10 aracterize the stoichiometry and the complex formation constants for this ionophore.

11 Speciation modeling that includes formation constants for U ternary complexes reveals that

12 The formation constants for Zn(II)-GGG with a Cys4, Cys3His1

13 thymines, generating a T-Hg-T complex with a formation constant higher than that one of the coupling

14 in the visual cycle after all-trans-retinal formation; constant illumination of eyecups produced a b

15 A lower-limit estimate of the formation constant in our standard buffer (40 mm Tris (p

16 an be conveniently used to calculate complex formation constants in situ.

17 metric method to determine ionophore complex formation constants in solvent polymeric membrane phases

18 The calculation of the complex formation constants in the polymeric membrane with creat

19 The conditional formation constants (in the presence of 50 mM Tris) of P

20 ulky lysine side chains, bind more strongly (formation constants K(f) approximately tens of M(-1)) th

21 Formation constants, K(M)(1), and K(M)(1)red, and rate c

22 ia the adduct [(tpfc)MnIII(ArINTs)], 3, with formation constant K3 = (10 +/- 2) x 10(3) L mol-1.

23 ) allowed calculation of the ternary complex formation constant (Ka').

24 th independent measurement of the Eu(DPA)(+) formation constant (Ka) allowed calculation of the terna

25 tion with the metal-ligand (citrate) complex formation constant (Kf).

26 Formation constants (Kf) proved the formation of stable

27 The formation constant (KML = [ML]/[M][L]) of In(III)--6SS i

28 lexes were small; the differences in complex formation constants lead to a larger rate of reaction fo

29 eadily observed in ESI-MS, even though their formation constants may be several orders of magnitude l

30 +) is consistent with the pattern of complex formation constants observed in the mixed solvent 80% me

31 arkably high thermodynamic stability, with a formation constant of 10(54).

32 e to determine the stoichiometry and overall formation constant of an ion-ionophore complex.

33 stic kinetic model, except that the apparent formation constant of Fe(II)-SRFA complexes is substanti

34 nding with nitrosonium/nitric oxide with the formation constant of K(B) approximately 10(8) M(-)(1) a

35 titrations have determined the thermodynamic formation constant of the [In(octapa)](-) complex to be

36 erization leading to dimers and trimers with formation constants of 1.61 x 10(3) and 6.61 x 10(3) M(-

37 artition coefficients and receptor-substrate formation constants of a target species, phenobarbital,

38 The formation constants of both complexes are determined fro

39 real-time using five ligands with differing formation constants of Cu(II) complexation.

40 ocycles bind Fe(II) in aqueous solution with formation constants of log K = 13.5 and 19.2, respective

41 Values of formation constants of the T1Cu(II)T2Cu(II)-SO(2)(.-) an

42 nhibition may not be seen because of the low formation constants of the vanadate-hydroxamic acid comp

43 he fluorophilic crown ether, with cumulative formation constants of up to 10(15.0) and 10(21.0) for o

44 On the basis of this, we report refined formation constants (+/-SE) for the three aqueous Hg(II)

45 ble metal cyanide complexes possess a higher formation constant than cyanoaurate.

46 ium wherein methoxide leads to a much larger formation constant than isopropoxide.

47 exation stoichiometry is needed to yield the formation constants that are consistent with those deter

48 equilibria involving DPP and metal ions gave formation constants that show that DPP has a higher affi

49 the UV-vis-NIR titration shows the stepwise formation constants to be K(1) = 8.9 x 10(8) M(-1) and K

50 The overall formation constants were calculated: log beta(110) = 39.

51 ellent agreement; for example, netropsin/DNA formation constants were determined to be K = 1.7x10(8)

52 , and thus increases in the overall reaction formation constants, were observed for all noncovalent i