Would sodium explode in salt water?
$begingroup$
I’ve seen the video etc of sodium being put into freshwater and the reaction of flames/small explosion but I wonder if the same reaction would occur if conducted in salt water such as the ocean.
inorganic-chemistry water aqueous-solution hydrogen
edited 7 hours ago
andselisk
14.8k649107
asked 7 hours ago
CarlyCarly
241
New contributor
Carly is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
$endgroup$
add a comment |
$begingroup$
I’ve seen the video etc of sodium being put into freshwater and the reaction of flames/small explosion but I wonder if the same reaction would occur if conducted in salt water such as the ocean.
inorganic-chemistry water aqueous-solution hydrogen
edited 7 hours ago
andselisk
14.8k649107
asked 7 hours ago
CarlyCarly
241
New contributor
Carly is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
$endgroup$
$begingroup$
chemistry.stackexchange.com/questions/2606/…
$endgroup$
– Mithoron
3 hours ago
add a comment |
$begingroup$
I’ve seen the video etc of sodium being put into freshwater and the reaction of flames/small explosion but I wonder if the same reaction would occur if conducted in salt water such as the ocean.
inorganic-chemistry water aqueous-solution hydrogen
edited 7 hours ago
andselisk
14.8k649107
asked 7 hours ago
CarlyCarly
241
New contributor
Carly is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
$endgroup$
I’ve seen the video etc of sodium being put into freshwater and the reaction of flames/small explosion but I wonder if the same reaction would occur if conducted in salt water such as the ocean.
inorganic-chemistry water aqueous-solution hydrogen
inorganic-chemistry water aqueous-solution hydrogen
edited 7 hours ago
andselisk
14.8k649107
asked 7 hours ago
CarlyCarly
241
New contributor
Carly is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
edited 7 hours ago
andselisk
14.8k649107
asked 7 hours ago
CarlyCarly
241
New contributor
Carly is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
edited 7 hours ago
andselisk
14.8k649107
edited 7 hours ago
andselisk
14.8k649107
edited 7 hours ago
andselisk
14.8k649107
14.8k649107
asked 7 hours ago
CarlyCarly
241
New contributor
Carly is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
asked 7 hours ago
CarlyCarly
241
asked 7 hours ago
CarlyCarly
241
241
New contributor
Carly is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
New contributor
Carly is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
Carly is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
$begingroup$
chemistry.stackexchange.com/questions/2606/…
$endgroup$
– Mithoron
3 hours ago
add a comment |
$begingroup$
chemistry.stackexchange.com/questions/2606/…
$endgroup$
– Mithoron
3 hours ago
$begingroup$
chemistry.stackexchange.com/questions/2606/…
$endgroup$
– Mithoron
3 hours ago
$begingroup$
chemistry.stackexchange.com/questions/2606/…
$endgroup$
– Mithoron
3 hours ago
add a comment |
2 Answers
2
active
oldest
votes
$begingroup$
Yes, sodium metal is also going to react exothermically with salt water or any other aqueous solution as long as it comes in contact with water:
$$ce{Na (s) + H2O -> Na+ (aq) + OH- (aq) + 0.5 H2 (g)}$$
eventually leading to explosion of hydrogen-oxygen mix forming near the water surface. Presence of sodium chloride in salt water isn't going to influence the reaction as it neither capable of shifting equilibrium to the left (gas formation), nor passivate sodium metal surface as it would do, for instance, some viscous oil.
answered 7 hours ago
andseliskandselisk
14.8k649107
$endgroup$
$begingroup$
According to this post, this is an incomplete explanation of the reason for explosion.
$endgroup$
– Ruslan
3 hours ago
1
$begingroup$
@Ruslan Of course it's incomplete because that's not what OP asked about. Thanks for providing the URL, now those who are also interested in how the detonation occurs, may quickly find the answer:)
$endgroup$
– andselisk
3 hours ago
add a comment |
$begingroup$
Sodium catches fire even in humid atmosphere. Salt water will make no difference. It will react with water in solution of salt in water, and the heat evolved will be very high and will vapourize sodium and it will fly away and may cause injuries. Do not do this at home.
$endgroup$
add a comment |
Your Answer
StackExchange.ifUsing("editor", function () {
return StackExchange.using("mathjaxEditing", function () {
StackExchange.MarkdownEditor.creationCallbacks.add(function (editor, postfix) {
StackExchange.mathjaxEditing.prepareWmdForMathJax(editor, postfix, [["$", "$"], ["\\(","\\)"]]);
});
});
}, "mathjax-editing");
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
});
}
});
Carly is a new contributor. Be nice, and check out our Code of Conduct.
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%2f108332%2fwould-sodium-explode-in-salt-water%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
$begingroup$
Yes, sodium metal is also going to react exothermically with salt water or any other aqueous solution as long as it comes in contact with water:
$$ce{Na (s) + H2O -> Na+ (aq) + OH- (aq) + 0.5 H2 (g)}$$
eventually leading to explosion of hydrogen-oxygen mix forming near the water surface. Presence of sodium chloride in salt water isn't going to influence the reaction as it neither capable of shifting equilibrium to the left (gas formation), nor passivate sodium metal surface as it would do, for instance, some viscous oil.
answered 7 hours ago
andseliskandselisk
14.8k649107
$endgroup$
$begingroup$
According to this post, this is an incomplete explanation of the reason for explosion.
$endgroup$
– Ruslan
3 hours ago
1
$begingroup$
@Ruslan Of course it's incomplete because that's not what OP asked about. Thanks for providing the URL, now those who are also interested in how the detonation occurs, may quickly find the answer:)
$endgroup$
– andselisk
3 hours ago
add a comment |
$begingroup$
Yes, sodium metal is also going to react exothermically with salt water or any other aqueous solution as long as it comes in contact with water:
$$ce{Na (s) + H2O -> Na+ (aq) + OH- (aq) + 0.5 H2 (g)}$$
eventually leading to explosion of hydrogen-oxygen mix forming near the water surface. Presence of sodium chloride in salt water isn't going to influence the reaction as it neither capable of shifting equilibrium to the left (gas formation), nor passivate sodium metal surface as it would do, for instance, some viscous oil.
answered 7 hours ago
andseliskandselisk
14.8k649107
$endgroup$
$begingroup$
According to this post, this is an incomplete explanation of the reason for explosion.
$endgroup$
– Ruslan
3 hours ago
1
$begingroup$
@Ruslan Of course it's incomplete because that's not what OP asked about. Thanks for providing the URL, now those who are also interested in how the detonation occurs, may quickly find the answer:)
$endgroup$
– andselisk
3 hours ago
add a comment |
$begingroup$
Yes, sodium metal is also going to react exothermically with salt water or any other aqueous solution as long as it comes in contact with water:
$$ce{Na (s) + H2O -> Na+ (aq) + OH- (aq) + 0.5 H2 (g)}$$
eventually leading to explosion of hydrogen-oxygen mix forming near the water surface. Presence of sodium chloride in salt water isn't going to influence the reaction as it neither capable of shifting equilibrium to the left (gas formation), nor passivate sodium metal surface as it would do, for instance, some viscous oil.
answered 7 hours ago
andseliskandselisk
14.8k649107
$endgroup$
Yes, sodium metal is also going to react exothermically with salt water or any other aqueous solution as long as it comes in contact with water:
$$ce{Na (s) + H2O -> Na+ (aq) + OH- (aq) + 0.5 H2 (g)}$$
eventually leading to explosion of hydrogen-oxygen mix forming near the water surface. Presence of sodium chloride in salt water isn't going to influence the reaction as it neither capable of shifting equilibrium to the left (gas formation), nor passivate sodium metal surface as it would do, for instance, some viscous oil.
answered 7 hours ago
andseliskandselisk
14.8k649107
edited 6 hours ago
answered 7 hours ago
andseliskandselisk
14.8k649107
answered 7 hours ago
andseliskandselisk
14.8k649107
answered 7 hours ago
andseliskandselisk
14.8k649107
14.8k649107
$begingroup$
According to this post, this is an incomplete explanation of the reason for explosion.
$endgroup$
– Ruslan
3 hours ago
1
$begingroup$
@Ruslan Of course it's incomplete because that's not what OP asked about. Thanks for providing the URL, now those who are also interested in how the detonation occurs, may quickly find the answer:)
$endgroup$
– andselisk
3 hours ago
add a comment |
$begingroup$
According to this post, this is an incomplete explanation of the reason for explosion.
$endgroup$
– Ruslan
3 hours ago
1
$begingroup$
@Ruslan Of course it's incomplete because that's not what OP asked about. Thanks for providing the URL, now those who are also interested in how the detonation occurs, may quickly find the answer:)
$endgroup$
– andselisk
3 hours ago
$begingroup$
According to this post, this is an incomplete explanation of the reason for explosion.
$endgroup$
– Ruslan
3 hours ago
$begingroup$
According to this post, this is an incomplete explanation of the reason for explosion.
$endgroup$
– Ruslan
3 hours ago
1
1
$begingroup$
@Ruslan Of course it's incomplete because that's not what OP asked about. Thanks for providing the URL, now those who are also interested in how the detonation occurs, may quickly find the answer:)
$endgroup$
– andselisk
3 hours ago
$begingroup$
@Ruslan Of course it's incomplete because that's not what OP asked about. Thanks for providing the URL, now those who are also interested in how the detonation occurs, may quickly find the answer:)
$endgroup$
– andselisk
3 hours ago
add a comment |
$begingroup$
Sodium catches fire even in humid atmosphere. Salt water will make no difference. It will react with water in solution of salt in water, and the heat evolved will be very high and will vapourize sodium and it will fly away and may cause injuries. Do not do this at home.
$endgroup$
add a comment |
$begingroup$
Sodium catches fire even in humid atmosphere. Salt water will make no difference. It will react with water in solution of salt in water, and the heat evolved will be very high and will vapourize sodium and it will fly away and may cause injuries. Do not do this at home.
$endgroup$
add a comment |
$begingroup$
Sodium catches fire even in humid atmosphere. Salt water will make no difference. It will react with water in solution of salt in water, and the heat evolved will be very high and will vapourize sodium and it will fly away and may cause injuries. Do not do this at home.
$endgroup$
Sodium catches fire even in humid atmosphere. Salt water will make no difference. It will react with water in solution of salt in water, and the heat evolved will be very high and will vapourize sodium and it will fly away and may cause injuries. Do not do this at home.
answered 7 hours ago
community wiki
Saurav Singh
add a comment |
add a comment |
Carly is a new contributor. Be nice, and check out our Code of Conduct.
Carly is a new contributor. Be nice, and check out our Code of Conduct.
Carly is a new contributor. Be nice, and check out our Code of Conduct.
Carly is a new contributor. Be nice, and check out our Code of Conduct.
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%2f108332%2fwould-sodium-explode-in-salt-water%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
$begingroup$
chemistry.stackexchange.com/questions/2606/…
$endgroup$
– Mithoron
3 hours ago