46. CHEMWORK 2+ ion forms complex ions with I' as follows: The Hg Hg2IHgI = 1.0...
Lunes CHEMWORK The Hg2+ ion forms complex ions with I as follows: Hg2+ + HgT+ HgI + 1 =Hg2 K1 = 1.0 108 K2=1.0 x 105 K3 -1.0 x 10° K4 = 1.0 * 108 Hgl2 + 1 + HgI3 HgI3 + 1 = Hg142 A solution is prepared by dissolving 0.057 mol Hg(NO3)2 and 5.00 mol Nal in enough water to make 1.0 L of solution. Calculate the equilibrium concentration of [Hg142]. (Hg142) = M Calculate the equilibrium concentration...
The Hg2 ion forms complex ions with I' as follows: Hg2 HgI* K1 1.0x 108 HglIHg2 Ка— 1.0 х 105 Hgl2 IHgl3" K3 1.0 x 109 Hgl3IHgl42K4= 1.0 x 108 A solution is prepared by dissolving 0.044 mol Hg(NO3)2 and 5.00 mol Nal in enough water to make 1.0 L of solution Calculate the equilibrium concentration of [Hgl42 ]. [Hgl 2- Calculate the equilibrium concentration of [I']. [ Calculate the equilibrium concentration of [Hg [Hg2= м
The Hg2+ ion forms complex ions with I- as
follows:
Hg2+ + I-
HgI+
K1 = 1.0 × 108
HgI+ + I-
HgI2
K2 = 1.0 × 105
HgI2 + I-
HgI3-
K3 = 1.0 × 109
HgI3- + I-
HgI42-
K4 = 1.0 × 108
A solution is prepared by dissolving 0.053 mol
Hg(NO3)2 and 5.00 mol NaI in enough water to
make 1.0 L of solution.
Calculate the equilibrium concentration of
[HgI42- ].
[HgI42- ] = M
Calculate...
The Hg2+ ion forms complex ions with I- as follows:
Hg2+ + I-
HgI+
K1 = 1.0 × 108
HgI+ + I-
HgI2
K2 = 1.0 × 105
HgI2 + I-
HgI3-
K3 = 1.0 × 109
HgI3- + I-
HgI42-
K4 = 1.0 × 108
A solution is prepared by dissolving 0.045 mol
Hg(NO3)2 and 5.00 mol NaI in enough water to
make 1.0 L of solution.
Calculate the equilibrium concentration of
[HgI42- ].
[HgI42- ] = ? M...
Calculate the molar concentration of Hg+2 ion.
estion 1 For the aqueous (Hg(NH3)4]2+ complex has a Ky - 1,8 x 1019 at 25°C. Suppose equal volumes of 0.0082 M Hg(NO3)2 solution and 0.72 M NH3 solution were mixed. Calculate the equilibrium concentration (M) of aqueous (Please enter your answer is scientific notation. For example if you answer was 3.15 x 10. please enter 3.1585) Answer should be in 2 significant figures.
For the aqueous (Hg(NH3)4]2+ complex has a K - 1.8 x 1019 at 25°C. Suppose equal volumes of 0.0082 M Hg(NO3)2 solution and 0.72 M NHg solution were mixed. Calculate the equilibrium concentration (M) of aqueous Hg2+ ion. (Please enter your answer is scientific notation. For example if you answer was 3.15 x 106, please enter 3.1585) Answer should be in 2 significant figures.
Question 1 For the aqueous (Hg(NH3)4]2+ complex has a Kt - 1.8 x 1019 at 25°C. Suppose equal volumes of 0.0082 M Hg(NO3)2 solution and 0.72 M NH3 solution were mixed. Calculate the equilibrium concentration (Mof aqueous Hg2+ ion. (Please enter your answer is scientific notation. For example if you answer was 3.15 x 106, please enter 3.155) Answer should be in 2 significant figures
Mercury (II) forms the soluble neutral complex Hg(SCN)2 with the ligand SCN- The overall formation constant B2 for binding of SCN to Hg2+ is 2.0 x 1017 Calculate the equilibrium molar concentrations of Hg2+ and SCN- and Hg(SCN)2 in a solution prepared by mixing 10 mL of 0.0200 M Hg2+ with 10 mL of 0.0200 M SCN". Make reasonable simplifying assumptions... and state them!
please explain thoroughly. thanks
4. Mercury (II) forms the soluble neutral complex Hg(SCN)2 with the ligand SCN The overall formation constant B2 for binding of SCN to Hg?* is 2.0 x 10" Calculate the equilibrium molar concentrations of Hg2+ and SCN and Hg(SCN) in a solution prepared by mixing 10 mL of 0.0200 M Hg2+ with 10 mL of 0.0200 M SCN Make reasonable simplifying assumptions... and state them!
please explain. thanks
4. Mercury (II) forms the soluble neutral complex Hg(SCN)2 with the ligand SCN The overall formation constant B2 for binding of SCN to Hg?* is 2.0 x 10" Calculate the equilibrium molar concentrations of Hg2+ and SCN and Hg(SCN) in a solution prepared by mixing 10 mL of 0.0200 M Hg2+ with 10 mL of 0.0200 M SCN Make reasonable simplifying assumptions... and state them!