All Questions
Tagged with aqueous-solution redox
68
questions
2
votes
2
answers
162
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Is acidified dichromate(VI) capable of oxidizing hydrogen sulfide to sulfur dioxide?
My textbook outlines reductive behaviour of $\ce{H2S}$ with the reaction
$$\ce{3H2S + K2Cr2O7 + 4H2SO4 -> 3S + Cr2(SO4)3 + K2SO4 + 7H2O}.\label{rxn:QR1}\tag{R1}$$
This reaction oxidizes $\ce{S^2-}$ ...
- 2,331
3
votes
4
answers
9k
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What gas are the bubbles that evolve in the redox reaction of copper(II) chloride and aluminum?
When aluminum (foil) is placed in an aqueous solution of copper(II) chloride, the aluminum atoms lose electrons to the copper(II) ions and replace them to form aluminum chloride, and to free up ...
- 1,201
6
votes
1
answer
315
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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
1
vote
3
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3k
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Copper metal with silver ion
My book states that $\ce{2AgNO3(aq) +Cu ->Cu(NO3^-)2(aq) +2Ag(s)}$. In addition to the formula, it also shows the following image:
As in the image it shows the salmon colored copper atoms are ...
- 435
1
vote
1
answer
9k
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How does chromium(III) react to form chromium(VI) with hydrogen peroxide?
$$\ce{2Cr(OH)3 + 4NaOH + 3H2O2 -> 2Na2CrO4 + 8H2O}$$
How does this reaction occur? We suddenly get sodium chromate in the place of chromium hydroxide. I can't understand it. We mix two hydroxides ...
- 3,276
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
9
votes
2
answers
1k
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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:
$$\ce{3NaNO3 + 8Al + 5NaOH + 18H2O -> 8Na[Al(OH)4] + 3NH3(...
- 3,276
2
votes
0
answers
154
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Will bases typically precipitate silver atoms from silver ions?
In class I learnt that one can dissolve many substances using acid and that this can be predicted using standard electrode potentials. For example,
$$\begin{align}
\ce{Zn &-> Zn^{2+} + 2e^-} ...
2
votes
1
answer
874
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Trying to displace iron from ferrous sulphate heptahydrate using aluminium foil but nothing has happened
I started by dissolving the sulphate into water and filtering it as I noticed there was a dirty residue lying at the bottom. (I am using ferrous sulphate that is commonly used in gardening.) I then ...
5
votes
1
answer
3k
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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 ...
2
votes
3
answers
8k
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How does salt concentration affect corrosion rate of iron?
I have conducted an experiment where I test the affect of $\ce{NaCl}$ concentration on corrosion rate of iron. I did this in an environment were all of the iron was submerged in water and the water ...
- 235
20
votes
3
answers
15k
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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
3
votes
2
answers
1k
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Adding powdered Pb and Fe to a solution
My book states that if we add powdered $\ce{Pb}$ (lead) and $\ce{Fe}$ (iron) to a solution containing $1\ \mathrm{M}$ each of $\ce{Pb^2+}$ and $\ce{Fe^2+}$ it would result in formation of more $\ce{Pb}...
- 780
-4
votes
2
answers
464
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Are aqueous solutions of oxidizing agents safe? [closed]
In the "reducing agent" article in Wikipedia it says
Good reducing agents are reagents that deliver $\ce{H2}$.
Wouldn't that make water unsafe to dissolve oxidizing agents?
- 4,265
4
votes
1
answer
340
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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