Leaching of copper using zinc
.everyoneloves__top-leaderboard:empty,.everyoneloves__mid-leaderboard:empty,.everyoneloves__bot-mid-leaderboard:empty{ margin-bottom:0;
}
$begingroup$
Why can we not use zinc for extracting copper from a solution containing $ce{Cu^2+}$ ions even though it is a better reducing agent than $ce{Fe}$?
I am studying metallurgy and I cannot understand why zinc cannot be used.
electrochemistry redox metallurgy
edited May 24 at 8:30
andselisk♦
21.9k8 gold badges77 silver badges147 bronze badges
asked May 24 at 6:24
Vikas BalaniVikas Balani
141 bronze badge
$endgroup$
add a comment |
$begingroup$
Why can we not use zinc for extracting copper from a solution containing $ce{Cu^2+}$ ions even though it is a better reducing agent than $ce{Fe}$?
I am studying metallurgy and I cannot understand why zinc cannot be used.
electrochemistry redox metallurgy
edited May 24 at 8:30
andselisk♦
21.9k8 gold badges77 silver badges147 bronze badges
asked May 24 at 6:24
Vikas BalaniVikas Balani
141 bronze badge
$endgroup$
$begingroup$
Just saying it, but many metallurgical process and reagents have an economic aspect to the choices made.
$endgroup$
– user79161
May 24 at 8:52
add a comment |
$begingroup$
Why can we not use zinc for extracting copper from a solution containing $ce{Cu^2+}$ ions even though it is a better reducing agent than $ce{Fe}$?
I am studying metallurgy and I cannot understand why zinc cannot be used.
electrochemistry redox metallurgy
edited May 24 at 8:30
andselisk♦
21.9k8 gold badges77 silver badges147 bronze badges
asked May 24 at 6:24
Vikas BalaniVikas Balani
141 bronze badge
$endgroup$
Why can we not use zinc for extracting copper from a solution containing $ce{Cu^2+}$ ions even though it is a better reducing agent than $ce{Fe}$?
I am studying metallurgy and I cannot understand why zinc cannot be used.
electrochemistry redox metallurgy
electrochemistry redox metallurgy
edited May 24 at 8:30
andselisk♦
21.9k8 gold badges77 silver badges147 bronze badges
asked May 24 at 6:24
Vikas BalaniVikas Balani
141 bronze badge
edited May 24 at 8:30
andselisk♦
21.9k8 gold badges77 silver badges147 bronze badges
asked May 24 at 6:24
Vikas BalaniVikas Balani
141 bronze badge
edited May 24 at 8:30
andselisk♦
21.9k8 gold badges77 silver badges147 bronze badges
edited May 24 at 8:30
andselisk♦
21.9k8 gold badges77 silver badges147 bronze badges
edited May 24 at 8:30
andselisk♦
21.9k8 gold badges77 silver badges147 bronze badges
21.9k8 gold badges77 silver badges147 bronze badges
asked May 24 at 6:24
Vikas BalaniVikas Balani
141 bronze badge
asked May 24 at 6:24
Vikas BalaniVikas Balani
141 bronze badge
asked May 24 at 6:24
Vikas BalaniVikas Balani
141 bronze badge
141 bronze badge
$begingroup$
Just saying it, but many metallurgical process and reagents have an economic aspect to the choices made.
$endgroup$
– user79161
May 24 at 8:52
add a comment |
$begingroup$
Just saying it, but many metallurgical process and reagents have an economic aspect to the choices made.
$endgroup$
– user79161
May 24 at 8:52
$begingroup$
Just saying it, but many metallurgical process and reagents have an economic aspect to the choices made.
$endgroup$
– user79161
May 24 at 8:52
$begingroup$
Just saying it, but many metallurgical process and reagents have an economic aspect to the choices made.
$endgroup$
– user79161
May 24 at 8:52
add a comment |
2 Answers
2
active
oldest
votes
$begingroup$
We can.
But I see few reasons why it is not used:
- Iron is much cheaper than zinc.
- There can be remaining residue of iron/zinc, coated by copper, or just being excessive. While copper can be melted away and iron stays, zinc would melt together with copper, causing unwanted impurity (unless wanted for making brass alloys)
- If we remove copper for environmental concerns, then by using zinc, we would just replace one evil by another. While both metals are essential for life in small amounts, both are toxic in larger amounts. ( So does iron, but at much higher level)
- Removing dissolved iron from waste is easier than removing zinc.
answered May 24 at 6:40
PoutnikPoutnik
4,1101 gold badge6 silver badges22 bronze badges
$endgroup$
add a comment |
$begingroup$
Do you know that the American Chemical Society has listed zinc as an "endangered" element? According to them, within hundred years the supply of zinc will be scarce. The best reducing agent in the world is the cathode of an electrolytic cell. Copper(II) is quite easy to reduce by electricity. Why waste an endangered element?
answered May 25 at 3:21
M. FarooqM. Farooq
5,5118 silver badges22 bronze badges
$endgroup$
$begingroup$
In fact, the similar is done during electrolytic copper purification on the industrial level.
$endgroup$
– Poutnik
May 25 at 7:41
$begingroup$
Time to properly process primary batteries and iron/steel with zinc anti-corrosive coating.
$endgroup$
– Poutnik
May 25 at 14:09
add a comment |
Your Answer
StackExchange.ready(function() {
var channelOptions = {
tags: "".split(" "),
id: "431"
};
initTagRenderer("".split(" "), "".split(" "), channelOptions);
StackExchange.using("externalEditor", function() {
// Have to fire editor after snippets, if snippets enabled
if (StackExchange.settings.snippets.snippetsEnabled) {
StackExchange.using("snippets", function() {
createEditor();
});
}
else {
createEditor();
}
});
function createEditor() {
StackExchange.prepareEditor({
heartbeatType: 'answer',
autoActivateHeartbeat: false,
convertImagesToLinks: false,
noModals: true,
showLowRepImageUploadWarning: true,
reputationToPostImages: null,
bindNavPrevention: true,
postfix: "",
imageUploader: {
brandingHtml: "Powered by u003ca class="icon-imgur-white" href="https://imgur.com/"u003eu003c/au003e",
contentPolicyHtml: "User contributions licensed under u003ca href="https://creativecommons.org/licenses/by-sa/3.0/"u003ecc by-sa 3.0 with attribution requiredu003c/au003e u003ca href="https://stackoverflow.com/legal/content-policy"u003e(content policy)u003c/au003e",
allowUrls: true
},
onDemand: true,
discardSelector: ".discard-answer"
,immediatelyShowMarkdownHelp:true
});
}
});
Sign up or log in
StackExchange.ready(function () {
StackExchange.helpers.onClickDraftSave('#login-link');
});
Sign up using Google
Sign up using Facebook
Sign up using Email and Password
Post as a guest
Required, but never shown
StackExchange.ready(
function () {
StackExchange.openid.initPostLogin('.new-post-login', 'https%3a%2f%2fchemistry.stackexchange.com%2fquestions%2f115850%2fleaching-of-copper-using-zinc%23new-answer', 'question_page');
}
);
Post as a guest
Required, but never shown
2 Answers
2
active
oldest
votes
2 Answers
2
active
oldest
votes
active
oldest
votes
active
oldest
votes
$begingroup$
We can.
But I see few reasons why it is not used:
- Iron is much cheaper than zinc.
- There can be remaining residue of iron/zinc, coated by copper, or just being excessive. While copper can be melted away and iron stays, zinc would melt together with copper, causing unwanted impurity (unless wanted for making brass alloys)
- If we remove copper for environmental concerns, then by using zinc, we would just replace one evil by another. While both metals are essential for life in small amounts, both are toxic in larger amounts. ( So does iron, but at much higher level)
- Removing dissolved iron from waste is easier than removing zinc.
answered May 24 at 6:40
PoutnikPoutnik
4,1101 gold badge6 silver badges22 bronze badges
$endgroup$
add a comment |
$begingroup$
We can.
But I see few reasons why it is not used:
- Iron is much cheaper than zinc.
- There can be remaining residue of iron/zinc, coated by copper, or just being excessive. While copper can be melted away and iron stays, zinc would melt together with copper, causing unwanted impurity (unless wanted for making brass alloys)
- If we remove copper for environmental concerns, then by using zinc, we would just replace one evil by another. While both metals are essential for life in small amounts, both are toxic in larger amounts. ( So does iron, but at much higher level)
- Removing dissolved iron from waste is easier than removing zinc.
answered May 24 at 6:40
PoutnikPoutnik
4,1101 gold badge6 silver badges22 bronze badges
$endgroup$
add a comment |
$begingroup$
We can.
But I see few reasons why it is not used:
- Iron is much cheaper than zinc.
- There can be remaining residue of iron/zinc, coated by copper, or just being excessive. While copper can be melted away and iron stays, zinc would melt together with copper, causing unwanted impurity (unless wanted for making brass alloys)
- If we remove copper for environmental concerns, then by using zinc, we would just replace one evil by another. While both metals are essential for life in small amounts, both are toxic in larger amounts. ( So does iron, but at much higher level)
- Removing dissolved iron from waste is easier than removing zinc.
answered May 24 at 6:40
PoutnikPoutnik
4,1101 gold badge6 silver badges22 bronze badges
$endgroup$
We can.
But I see few reasons why it is not used:
- Iron is much cheaper than zinc.
- There can be remaining residue of iron/zinc, coated by copper, or just being excessive. While copper can be melted away and iron stays, zinc would melt together with copper, causing unwanted impurity (unless wanted for making brass alloys)
- If we remove copper for environmental concerns, then by using zinc, we would just replace one evil by another. While both metals are essential for life in small amounts, both are toxic in larger amounts. ( So does iron, but at much higher level)
- Removing dissolved iron from waste is easier than removing zinc.
answered May 24 at 6:40
PoutnikPoutnik
4,1101 gold badge6 silver badges22 bronze badges
edited May 24 at 15:21
answered May 24 at 6:40
PoutnikPoutnik
4,1101 gold badge6 silver badges22 bronze badges
answered May 24 at 6:40
PoutnikPoutnik
4,1101 gold badge6 silver badges22 bronze badges
answered May 24 at 6:40
PoutnikPoutnik
4,1101 gold badge6 silver badges22 bronze badges
4,1101 gold badge6 silver badges22 bronze badges
add a comment |
add a comment |
$begingroup$
Do you know that the American Chemical Society has listed zinc as an "endangered" element? According to them, within hundred years the supply of zinc will be scarce. The best reducing agent in the world is the cathode of an electrolytic cell. Copper(II) is quite easy to reduce by electricity. Why waste an endangered element?
answered May 25 at 3:21
M. FarooqM. Farooq
5,5118 silver badges22 bronze badges
$endgroup$
$begingroup$
In fact, the similar is done during electrolytic copper purification on the industrial level.
$endgroup$
– Poutnik
May 25 at 7:41
$begingroup$
Time to properly process primary batteries and iron/steel with zinc anti-corrosive coating.
$endgroup$
– Poutnik
May 25 at 14:09
add a comment |
$begingroup$
Do you know that the American Chemical Society has listed zinc as an "endangered" element? According to them, within hundred years the supply of zinc will be scarce. The best reducing agent in the world is the cathode of an electrolytic cell. Copper(II) is quite easy to reduce by electricity. Why waste an endangered element?
answered May 25 at 3:21
M. FarooqM. Farooq
5,5118 silver badges22 bronze badges
$endgroup$
$begingroup$
In fact, the similar is done during electrolytic copper purification on the industrial level.
$endgroup$
– Poutnik
May 25 at 7:41
$begingroup$
Time to properly process primary batteries and iron/steel with zinc anti-corrosive coating.
$endgroup$
– Poutnik
May 25 at 14:09
add a comment |
$begingroup$
Do you know that the American Chemical Society has listed zinc as an "endangered" element? According to them, within hundred years the supply of zinc will be scarce. The best reducing agent in the world is the cathode of an electrolytic cell. Copper(II) is quite easy to reduce by electricity. Why waste an endangered element?
answered May 25 at 3:21
M. FarooqM. Farooq
5,5118 silver badges22 bronze badges
$endgroup$
Do you know that the American Chemical Society has listed zinc as an "endangered" element? According to them, within hundred years the supply of zinc will be scarce. The best reducing agent in the world is the cathode of an electrolytic cell. Copper(II) is quite easy to reduce by electricity. Why waste an endangered element?
answered May 25 at 3:21
M. FarooqM. Farooq
5,5118 silver badges22 bronze badges
edited May 25 at 14:16
answered May 25 at 3:21
M. FarooqM. Farooq
5,5118 silver badges22 bronze badges
answered May 25 at 3:21
M. FarooqM. Farooq
5,5118 silver badges22 bronze badges
answered May 25 at 3:21
M. FarooqM. Farooq
5,5118 silver badges22 bronze badges
5,5118 silver badges22 bronze badges
$begingroup$
In fact, the similar is done during electrolytic copper purification on the industrial level.
$endgroup$
– Poutnik
May 25 at 7:41
$begingroup$
Time to properly process primary batteries and iron/steel with zinc anti-corrosive coating.
$endgroup$
– Poutnik
May 25 at 14:09
add a comment |
$begingroup$
In fact, the similar is done during electrolytic copper purification on the industrial level.
$endgroup$
– Poutnik
May 25 at 7:41
$begingroup$
Time to properly process primary batteries and iron/steel with zinc anti-corrosive coating.
$endgroup$
– Poutnik
May 25 at 14:09
$begingroup$
In fact, the similar is done during electrolytic copper purification on the industrial level.
$endgroup$
– Poutnik
May 25 at 7:41
$begingroup$
In fact, the similar is done during electrolytic copper purification on the industrial level.
$endgroup$
– Poutnik
May 25 at 7:41
$begingroup$
Time to properly process primary batteries and iron/steel with zinc anti-corrosive coating.
$endgroup$
– Poutnik
May 25 at 14:09
$begingroup$
Time to properly process primary batteries and iron/steel with zinc anti-corrosive coating.
$endgroup$
– Poutnik
May 25 at 14:09
add a comment |
Thanks for contributing an answer to Chemistry Stack Exchange!
- Please be sure to answer the question. Provide details and share your research!
But avoid …
- Asking for help, clarification, or responding to other answers.
- Making statements based on opinion; back them up with references or personal experience.
Use MathJax to format equations. MathJax reference.
To learn more, see our tips on writing great answers.
Sign up or log in
StackExchange.ready(function () {
StackExchange.helpers.onClickDraftSave('#login-link');
});
Sign up using Google
Sign up using Facebook
Sign up using Email and Password
Post as a guest
Required, but never shown
StackExchange.ready(
function () {
StackExchange.openid.initPostLogin('.new-post-login', 'https%3a%2f%2fchemistry.stackexchange.com%2fquestions%2f115850%2fleaching-of-copper-using-zinc%23new-answer', 'question_page');
}
);
Post as a guest
Required, but never shown
Sign up or log in
StackExchange.ready(function () {
StackExchange.helpers.onClickDraftSave('#login-link');
});
Sign up using Google
Sign up using Facebook
Sign up using Email and Password
Post as a guest
Required, but never shown
Sign up or log in
StackExchange.ready(function () {
StackExchange.helpers.onClickDraftSave('#login-link');
});
Sign up using Google
Sign up using Facebook
Sign up using Email and Password
Post as a guest
Required, but never shown
Sign up or log in
StackExchange.ready(function () {
StackExchange.helpers.onClickDraftSave('#login-link');
});
Sign up using Google
Sign up using Facebook
Sign up using Email and Password
Sign up using Google
Sign up using Facebook
Sign up using Email and Password
Post as a guest
Required, but never shown
Required, but never shown
Required, but never shown
Required, but never shown
Required, but never shown
Required, but never shown
Required, but never shown
Required, but never shown
Required, but never shown
$begingroup$
Just saying it, but many metallurgical process and reagents have an economic aspect to the choices made.
$endgroup$
– user79161
May 24 at 8:52