1- In the presence of excess OH-, the Zn2+(aq) ion forms a hydroxide complex ion, Zn(OH)42-....
1- In the presence of excess OH-, the
Zn2+(aq) ion forms a hydroxide complex
ion, Zn(OH)42-. Calculate
the concentration of free Zn2+ ion when
1.32×10-2mol
ZnSO4(s) is added to 1.00 L of solution
in which [OH- ] is held constant (buffered at pH
12.40). For
Zn(OH)42-, Kf =
4.6×1017.
[Zn2+] = ------ M
2-
What is the approximate concentration of free
Hg2+ ion at equilibrium when
1.86×10-2 mol mercury(II)
nitrate is added to 1.00 L of solution
that is 1.310 M in
Cl-. For
[HgCl4]2-, Kf =
1.2×1015.
- [Hg2+] = ------- M
Homework Answers
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1- In the presence of excess OH-, the
Zn2+(aq) ion forms a hydroxide complex
ion, Zn(OH)42-....
In the presence of excess OH-, the Zn2+(aq) ion forms a hydroxide complex ion, Zn(OH)42-. Calculate...
In the presence of excess OH-, the Zn2+(aq) ion forms a hydroxide complex ion, Zn(OH)42-. Calculate the concentration of free Zn2+ ion when 1.54×10-2 mol Zn(CH3COO)2(s) is added to 1.00 L of solution in which [OH- ] is held constant (buffered at pH 12.70). For Zn(OH)42-, Kf = 4.6×1017. [Zn2+] = M
In the presence of excess OH-, the Zn2+(aq) ion forms a hydroxide complex ion, Zn(OH)42-. Calculate...
In the presence of excess OH-, the Zn2+(aq) ion forms a hydroxide complex ion, Zn(OH)42-. Calculate the concentration of free Zn2+ ion when 1.57×10-2 mol Zn(NO3)2(s) is added to 1.00 L of solution in which [OH- ] is held constant (buffered at pH 12.20). For Zn(OH)42-, Kf = 4.6×1017. [Zn2+]=___M please explain
In the presence of excess OH-, the Al3+(aq) ion forms a hydroxide complex ion, Al(OH)4-. Calculate the concentration of...
In the presence of excess OH-, the Al3+(aq) ion forms a hydroxide complex ion, Al(OH)4-. Calculate the concentration of free Al3+ ion when 1.32×10-2 mol Al(NO3)3(s) is added to 1.00 L of solution in which [OH- ] is held constant (buffered at pH 13.00). For Al(OH)4-, Kf = 1.1×1033. [Al3+] = ?M
Calculate concentration of species in a solution containing a complex ion In the presence of excess...
Calculate concentration of species in a solution containing a complex ion In the presence of excess OH, the Al3 (aq) ion forms a hydroxide complex ion, AIOH)4. Calculate the concentration of free Al3 ion when 1.46*102 mol Al(NO3)3(s) is added to 1.00 L of solution in which [OH-] is held constant (buffered at pH 12.60). For Al(OH)4, K?1.1x1033.
Given the Ksp of Zn(OH)2 is 3.0x10-1, determine the Zn2 ion concentration when the pH of...
Given the Ksp of Zn(OH)2 is 3.0x10-1, determine the Zn2 ion concentration when the pH of the solution is buffered to pH=12.00 (so that the hydroxide ion concentration is 0.010 M). 1. Zn(OH)2(s) A. [Zn2] 3.0x10-12 M B. [Zn2 3.7x10- M C. [Zn23.0x10-10 M D. [Zn2] 9.1x10-3 M E. [Zn2] 1.5x10-13 M Zn2 (aq) + 20H (aq) Ksp 3.0x10-16 2. When silver carbonate, Ag,COs, is mixed with water, it dissolves to some extent to form a saturated solution where the...
Calculate concentration of species in a solution containing a complex ion. In the presence of excess...
Calculate concentration of species in a solution containing a complex ion. In the presence of excess OH^ -, the Al^ 3+ (aq) ion forms a hydroxide complex ion, Al(OH)^ -_4. Calculate the concentration of free Al^ 3+ ion when 1.64 times 10^-2 mol Al(CH_3COO)_3(s) is added to 1.00 L of solution in which [OH^ -] is held constant (buffered at pH 12.10). For Al(OH)_4^ -, K_f = 1.1 times 10^33.
5) Zinc forms a precipitate with the hydroxide ion (Zn(OH)2) as well as several complex ions....
5) Zinc forms a precipitate with the hydroxide ion (Zn(OH)2) as well as several complex ions. Given the equilibria below, calculate the concentration of each zinc species in a solution saturated with Zn(OH)2 and [OH') fixed at 3.2 x 107M Zn(OH)2(8) Ksp = 3 x 10-16 Zn(OH)* K= 1 x 104 Zn(OH)2(aq) K = 2 x 1010 Zn(OH)3 K = 8 x 1013 Zn(OH)42 K= 3 x 1015
A) Consider the insoluble compound zinc hydroxide, Zn(OH)2. The zinc ion also forms a complex with...
A) Consider the insoluble compound zinc hydroxide, Zn(OH)2. The zinc ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of Zn(OH)2(s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Zn(NH3)42+, Kf = 2.9×109. Specify states such as (aq) or (s) and provide K. K = ______ B) Consider the insoluble compound nickel(II) hydroxide, Ni(OH)2. The nickel ion also forms a complex with cyanide ions....
Calculate concentration of species in a solution containing a complex ion. Close Problem In the p...
Calculate concentration of species in a solution containing a complex ion. Close Problem In the presence of excess OH-, the Al3+(aq) ion forms a hydroxide complex ion, Al(OH)4-. Calculate the concentration of free Al3+ ion when 1.21×10-2 mol Al(CH3COO)3(s) is added to 1.00 L of solution in which [OH- ] is held constant (buffered at pH 12.60). For Al(OH)4-, Kf = 1.1×1033. [Al3+] = M
please help What is the approximate concentration of free Cu* ion at equilibrium when 1.57x102 mol...
please help
What is the approximate concentration of free Cu* ion at equilibrium when 1.57x102 mol copperII) nitrate is added to 1.00 L of solution that is 1.380 M in NH3. For [Cu(NH3)4j2, Kf 2.1 1013 [Cu2 м What is the approximate concentration of free Fe2* ion at equilibrium when 1.42x102mol iron(II) nitrate is added to 1.00 L of solution that is 1.38so M in CN. For [Fe(CN)6]4, Kf=1.0x1035 [Fe"]= In the presence of excess OH, the Al*(aq) ion forms...
Calculate concentration of species in a solution containing a complex ion In the presence of excess OH, the Al3 (aq) ion forms a hydroxide complex ion, AIOH)4. Calculate the concentration of free Al3 ion when 1.46*102 mol Al(NO3)3(s) is added to 1.00 L of solution in which [OH-] is held constant (buffered at pH 12.60). For Al(OH)4, K?1.1x1033.
Given the Ksp of Zn(OH)2 is 3.0x10-1, determine the Zn2 ion concentration when the pH of the solution is buffered to pH=12.00 (so that the hydroxide ion concentration is 0.010 M). 1. Zn(OH)2(s) A. [Zn2] 3.0x10-12 M B. [Zn2 3.7x10- M C. [Zn23.0x10-10 M D. [Zn2] 9.1x10-3 M E. [Zn2] 1.5x10-13 M Zn2 (aq) + 20H (aq) Ksp 3.0x10-16 2. When silver carbonate, Ag,COs, is mixed with water, it dissolves to some extent to form a saturated solution where the...
Calculate concentration of species in a solution containing a complex ion. In the presence of excess OH^ -, the Al^ 3+ (aq) ion forms a hydroxide complex ion, Al(OH)^ -_4. Calculate the concentration of free Al^ 3+ ion when 1.64 times 10^-2 mol Al(CH_3COO)_3(s) is added to 1.00 L of solution in which [OH^ -] is held constant (buffered at pH 12.10). For Al(OH)_4^ -, K_f = 1.1 times 10^33.
5) Zinc forms a precipitate with the hydroxide ion (Zn(OH)2) as well as several complex ions. Given the equilibria below, calculate the concentration of each zinc species in a solution saturated with Zn(OH)2 and [OH') fixed at 3.2 x 107M Zn(OH)2(8) Ksp = 3 x 10-16 Zn(OH)* K= 1 x 104 Zn(OH)2(aq) K = 2 x 1010 Zn(OH)3 K = 8 x 1013 Zn(OH)42 K= 3 x 1015
please help
What is the approximate concentration of free Cu* ion at equilibrium when 1.57x102 mol copperII) nitrate is added to 1.00 L of solution that is 1.380 M in NH3. For [Cu(NH3)4j2, Kf 2.1 1013 [Cu2 м What is the approximate concentration of free Fe2* ion at equilibrium when 1.42x102mol iron(II) nitrate is added to 1.00 L of solution that is 1.38so M in CN. For [Fe(CN)6]4, Kf=1.0x1035 [Fe"]= In the presence of excess OH, the Al*(aq) ion forms...
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