An industrial wastewater contains cadmium, ammonia, and chloride, and is in equilibrium with Cd(OH)2(s). (a) Write...
An industrial wastewater contains cadmium, ammonia, and chloride, and is in equilibrium with Cd(OH)2(s). (a) Write the general mass balance equation for soluble Cd. (b) Write the general mass balance equation for ammonia-N. (c) Write the general mass balance equation for Chloride. (d) Write the equation for the solubility (S) of Cd.
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![The general mass balance sau i mass balance Equation for ammonia- Total Concentration of Mitt i [Nts] + [NH4+] + [cd (NH3) t]](http://img.homeworklib.com/questions/0aaca740-70bd-11ea-8119-1d2a37498871.png?x-oss-process=image/resize,w_560)
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An industrial wastewater contains cadmium, ammonia, and
chloride, and is in equilibrium with Cd(OH)2(s). (a) Write...
Determine the solubility of Cadmium in equilibrium with Cadmium hydroxide, Cd(OH)2, as a function of pH....
Determine the solubility of Cadmium in equilibrium with Cadmium hydroxide, Cd(OH)2, as a function of pH. Ksp = 5.33 x 10^ -15
A rechargeable nickel-cadmium (NiCd) battery contains the following half-reactions: NiO2 +2H2O(l)+2e– → Ni(OH)2 +2OH– E0 =0.49V...
A rechargeable nickel-cadmium (NiCd) battery contains the following half-reactions: NiO2 +2H2O(l)+2e– → Ni(OH)2 +2OH– E0 =0.49V Cd(OH)2 +2e– →Cd(s)+2OH– E0 =–0.81V a. What is the standard cell potential or voltage of this NiCd cell? b. Write the net chemical reaction in the direction of spontaneous reaction. Is cadmium oxidized or reduced? c. Write an expression for the reaction quotient Q. What is Q if the electrolyte concentrations are: [NiO2] = 1 M and [Cd(OH)2] = 0.01M and [Ni(OH)2] = 0.001...
Will not precipitate in the presence of limited (or excess) base or ammonia. Therefore, KOH is no...
will not precipitate in the presence of limited (or excess) base or ammonia. Therefore, KOH is not amphoteric and does not form an ammonia complex. Prelab forms a precipitate in the presence of limited NaOH and ammonia. This precipitate n the presence of excess ammonia but NOT in the presence of excess NaOH a. Is Cd'2 amphoteric and/or does it form an ammonia complex? b. Write the equation for the reaction of Cd (aq) with limited OH c. Write the...
Consider the half‑reaction for the reduction of Cd 2+ Cd2+ to Cd(s) Cd(s) . Cd 2...
Consider the half‑reaction for the reduction of Cd 2+ Cd2+ to
Cd(s) Cd(s) . Cd 2 +(aq)+2 e − ⟶Cd(s) ? ∘ Cd 2+ /Cd =−0.403 V
Cd2+(aq)+2e−⟶Cd(s)ECd2+/Cd∘=−0.403 V Calculate the potential of the
cadmium electrode at 25 ∘ C 25 ∘C when immersed in a 0.0560 M
0.0560 M solution of CdBr 2 . CdBr2. ? Cd = ECd= V V Calculate the
potential of the cadmium electrode at 25 ∘ C 25 ∘C when immersed in
a 0.0330...
Nickel-cadmium (nicad) alkaline batteries are currently very popular because they maintain a constant potential and are...
Nickel-cadmium (nicad) alkaline batteries are currently very popular because they maintain a constant potential and are rechargeable. The relevant half-cell reactions for such batteries are given in this table. Half-Reaction, Cd(OH)2(s) + 2e- -> Cd(s) + 2 OH- (aq) E(volts) = -0.809 NiOOH(s)+ H2O(l) + e- -> Ni(OH)2(s)+OH-(aq) E(volts) = +0.490 A) Write a balanced equation for the process that produces electricity in a nicad battery and specify the half- reaction that occurs at the anode. B) Calculate the potential expected...
The following half-reactions occur during use of the rechargeable nickel-cadmium battery: Ca(OH)2(s) + 2e → Cd(s)...
The following half-reactions occur during use of the rechargeable nickel-cadmium battery: Ca(OH)2(s) + 2e → Cd(s) + 20H(aq) NiO(OH)(s) + H20(1) + e- → Ni(OH)2(s) + OH(aq) This battery has a potential of 1.35 V under standard conditions, with nickel as the cathode. What potential does this battery produce if its hydroxide ion concentration is 1.97 x 10-2 M? E = V the tolerance is +/-2%
Write a balanced net ionic equation to show why the solubility of Mn(OH)2(s) increases in the...
Write a balanced net ionic equation to show why the solubility of Mn(OH)2(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid Use the pull-down boxes to specify states such as (aq) or (s) (aq) 2H2O Mn(OH)2 2H Mn2+ (s) (aq) (I) K
Write a balanced net ionic equation to show why the solubility of Cu(OH)2(s) increases in the...
Write a balanced net ionic equation to show why the solubility of Cu(OH)2(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid. Use the pull-down boxes to specify states such as (aq) or (s). K-
In an ammonia solution, the silver ion, Ag, forms the colorless, but soluble diamminesilver(I) complex ion,...
In an ammonia solution, the silver ion, Ag, forms the colorless, but soluble diamminesilver(I) complex ion, Ag(NH3)2. If ammonia is added to a solution that contains an AgCI precipitate, the solid dissolves completely. Write a net-ionic equation for the equilibrium involved and explain the shift that takes place. Choose the best answer. AgCl(s) +2 NH3(a)Ag(NH3)2 (aa) C(aq) Adding ammonia to AgCl(s) dissolves the solid by displacing chloride ions with ammonia molecules, forming a soluble complex ion Ag (a2 NH3(aq) Ag(NH32...
Write a balanced net ionic equation to show why the solubility of Zn(CN)2(s) increases in the pre...
Write a balanced net ionic equation to show why the solubility
of Zn(CN)2(s) increases in the presence
of a strong acid and calculate the equilibrium constant for the
reaction of this sparingly soluble salt with acid.
I really need help with both because I am on my last attempt and
cannot seem to understand exactly how to solve for K. Thank you for
your help! I will be sure to rate your answer if it is correct.
Write a balanced...
will not precipitate in the presence of limited (or excess) base or ammonia. Therefore, KOH is not amphoteric and does not form an ammonia complex. Prelab forms a precipitate in the presence of limited NaOH and ammonia. This precipitate n the presence of excess ammonia but NOT in the presence of excess NaOH a. Is Cd'2 amphoteric and/or does it form an ammonia complex? b. Write the equation for the reaction of Cd (aq) with limited OH c. Write the...
Consider the half‑reaction for the reduction of Cd 2+ Cd2+ to
Cd(s) Cd(s) . Cd 2 +(aq)+2 e − ⟶Cd(s) ? ∘ Cd 2+ /Cd =−0.403 V
Cd2+(aq)+2e−⟶Cd(s)ECd2+/Cd∘=−0.403 V Calculate the potential of the
cadmium electrode at 25 ∘ C 25 ∘C when immersed in a 0.0560 M
0.0560 M solution of CdBr 2 . CdBr2. ? Cd = ECd= V V Calculate the
potential of the cadmium electrode at 25 ∘ C 25 ∘C when immersed in
a 0.0330...
The following half-reactions occur during use of the rechargeable nickel-cadmium battery: Ca(OH)2(s) + 2e → Cd(s) + 20H(aq) NiO(OH)(s) + H20(1) + e- → Ni(OH)2(s) + OH(aq) This battery has a potential of 1.35 V under standard conditions, with nickel as the cathode. What potential does this battery produce if its hydroxide ion concentration is 1.97 x 10-2 M? E = V the tolerance is +/-2%
Write a balanced net ionic equation to show why the solubility of Mn(OH)2(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid Use the pull-down boxes to specify states such as (aq) or (s) (aq) 2H2O Mn(OH)2 2H Mn2+ (s) (aq) (I) K
Write a balanced net ionic equation to show why the solubility of Cu(OH)2(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid. Use the pull-down boxes to specify states such as (aq) or (s). K-
In an ammonia solution, the silver ion, Ag, forms the colorless, but soluble diamminesilver(I) complex ion, Ag(NH3)2. If ammonia is added to a solution that contains an AgCI precipitate, the solid dissolves completely. Write a net-ionic equation for the equilibrium involved and explain the shift that takes place. Choose the best answer. AgCl(s) +2 NH3(a)Ag(NH3)2 (aa) C(aq) Adding ammonia to AgCl(s) dissolves the solid by displacing chloride ions with ammonia molecules, forming a soluble complex ion Ag (a2 NH3(aq) Ag(NH32...
Write a balanced net ionic equation to show why the solubility
of Zn(CN)2(s) increases in the presence
of a strong acid and calculate the equilibrium constant for the
reaction of this sparingly soluble salt with acid.
I really need help with both because I am on my last attempt and
cannot seem to understand exactly how to solve for K. Thank you for
your help! I will be sure to rate your answer if it is correct.
Write a balanced...
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