All Questions
Tagged with aqueous-solution redox
68
questions
20
votes
3
answers
15k
views
Why copper(I) is unstable in aqueous medium?
I am expecting that $\ce{Cu+}$ attains a $\mathrm d^{10}$ configuration by losing one electron from s-subshell. Since it has fully filled d-orbital, it should be stable. But it is found that it is ...
- 26.3k
9
votes
2
answers
1k
views
Why does Devarda's alloy include copper?
Devarda's alloy is used in the detection of nitrates. However, judging by the reaction equation, only aluminium plays the role of reducer:
$$\ce{3NaNO3 + 8Al + 5NaOH + 18H2O -> 8Na[Al(OH)4] + 3NH3(...
- 3,276
8
votes
2
answers
6k
views
Can lead(II) oxidize tin metal in aqueous solution?
According to my textbook, element $\ce{X}$ can oxidize element $\ce{Y}$ if $\ce{X}$ was lower in the activity series.
Lead is lower than Tin in the activity series table in the textbook, but the ...
- 83
7
votes
1
answer
7k
views
Does iron(III) sulfate react with copper?
As my understanding, there should be an oxidation-reduction reaction:
$$
\ce{2 Fe^3+ + Cu → 2Fe^2+ + Cu^2+}
$$
However, I always see the process using $\ce{FeCl3}$ to etch copper, but I never ...
- 173
6
votes
2
answers
568
views
Balancing reaction between copper and nitric acid given the ratio of formed nitrogen oxides
Problem
$\ce{Cu}$ reacts with $\ce{HNO3}$ according to the equation
$$\ce{Cu + HNO3 -> Cu(NO3)2 + NO + NO2 + H2O}$$
If $\ce{NO}$ and $\ce{NO2}$ are formed in 2:3 ratio, what is coefficient of $\ce{...
- 511
6
votes
1
answer
315
views
Would sodium metal react differently with aqueous solutions than with pure water?
I know sodium metal reacts violently with water, but what about aqueous solutions (like sodium bicarbonate). Also, what would the reaction kinetics be?
I have watched YouTube videos were a small ...
- 864
6
votes
2
answers
31k
views
Electrolysis of aqueous copper (II) nitrate
There are two copper blocks sitting in the $\ce{Cu(NO3)2 (aq)}$ solution, a battery is attached onto both of them, providing enough energy to start the reaction.
Since solid pieces of copper are ...
- 257
5
votes
1
answer
3k
views
What happens to potassium if potassium permanganate is reduced in a redox reaction? How can I identify spectator ions?
I'm trying to get a fool-proof way of finding the products of a redox reaction. I can do both the oxidation and reduction the half reactions. For example in the potassium permanganate with hydrogen ...
5
votes
1
answer
3k
views
How would I calculate the Normality of a 0.00167 molar solution of KIO₃?
I need a 0.01 N solution of $\ce{KIO3}$ to use as a standard in a Winkler titration. The protocol that I am using specifies that this is 0.3567 g L-1, which I have calculated to be 0.00167 M based on ...
- 233
4
votes
1
answer
4k
views
Reaction of aqueous sodium carbonate with aluminum foil
Aqueous sodium hydroxide is known to react with aluminum foil in an exothermic, hydrogen-gas releasing reaction like $$\ce{2NaOH(aq) + 2Al(s) + 2H2O(\ell) → 2NaAlO2(aq) + 3H2(g)}$$
However, on ...
- 1,556
4
votes
1
answer
2k
views
Can silver metal be used to electrochemically reduce copper?
I have a solution of copper(II) ions and several cations. I am trying to reduce the copper ions to copper metal with electricity. My Ideas was to use silver as the anode and a copper wire as the ...
- 521
4
votes
1
answer
340
views
Balancing Redox Equations - Half Reactions
How do I balance this using the half-reaction method: $$\ce{Zn(s) + HCl(aq) -> Zn^{2+} (aq) + H_2 (g)}$$
I would first split it up in its ionic components:
$\ce{Zn(s) + H^+ + Cl^- -> Zn^{2+} (...
- 415
4
votes
1
answer
234
views
How does a silver chloride electrode (Ag/AgCl) convert the potential in aqueous solution to the wire?
I am aware of the redox chemistry that happens at the electrode surface, but I'm not sure how exactly a change in electrical potential in the solution would change the potential in the electrode?
- 41
3
votes
2
answers
11k
views
Why would a solution of FeCl2 appear brown/yellow sort of like FeCl3?
If we prepare a solution of $\ce{FeCl2}$ by dissolving solid $\ce{FeCl2}$ powder in water, supposing the bottle of $\ce{FeCl2}$ was left open for sufficient time, is it possible for $\ce{FeCl2}$ to ...
- 318
3
votes
2
answers
441
views
Partial reactions in redox formation of rust
In the iron oxidation that results in rust, the first step is to steal 2 electrons from $\ce{Fe}$. The main thief is said to be the oxygen dissolved in water, witch uses the stolen electrons to form $\...
