Would sodium explode in salt water?
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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 Jan 21 at 16:18
andselisk
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asked Jan 21 at 16:04
CarlyCarly
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add a comment |
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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 Jan 21 at 16:18
andselisk
15k649108
asked Jan 21 at 16:04
CarlyCarly
5913
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.
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1
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chemistry.stackexchange.com/questions/2606/…
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– Mithoron
Jan 21 at 19:42
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youtu.be/LmlAYnFF_s8?t=398
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– uhoh
Jan 21 at 23:51
1
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@uhoh: I believe youtu.be/e9AiK5zulf8 is a much more straightforward way to answer OP's question. :)
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– Quuxplusone
Jan 22 at 3:24
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@Quuxplusone yes that certainly sounds like a coulomb explosion!
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– uhoh
Jan 22 at 3:28
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 Jan 21 at 16:18
andselisk
15k649108
asked Jan 21 at 16:04
CarlyCarly
5913
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 Jan 21 at 16:18
andselisk
15k649108
asked Jan 21 at 16:04
CarlyCarly
5913
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 Jan 21 at 16:18
andselisk
15k649108
asked Jan 21 at 16:04
CarlyCarly
5913
New contributor
Carly is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
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edited Jan 21 at 16:18
andselisk
15k649108
edited Jan 21 at 16:18
andselisk
15k649108
edited Jan 21 at 16:18
andselisk
15k649108
15k649108
asked Jan 21 at 16:04
CarlyCarly
5913
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 Jan 21 at 16:04
CarlyCarly
5913
asked Jan 21 at 16:04
CarlyCarly
5913
5913
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.
1
$begingroup$
chemistry.stackexchange.com/questions/2606/…
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– Mithoron
Jan 21 at 19:42
$begingroup$
youtu.be/LmlAYnFF_s8?t=398
$endgroup$
– uhoh
Jan 21 at 23:51
1
$begingroup$
@uhoh: I believe youtu.be/e9AiK5zulf8 is a much more straightforward way to answer OP's question. :)
$endgroup$
– Quuxplusone
Jan 22 at 3:24
$begingroup$
@Quuxplusone yes that certainly sounds like a coulomb explosion!
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– uhoh
Jan 22 at 3:28
add a comment |
1
$begingroup$
chemistry.stackexchange.com/questions/2606/…
$endgroup$
– Mithoron
Jan 21 at 19:42
$begingroup$
youtu.be/LmlAYnFF_s8?t=398
$endgroup$
– uhoh
Jan 21 at 23:51
1
$begingroup$
@uhoh: I believe youtu.be/e9AiK5zulf8 is a much more straightforward way to answer OP's question. :)
$endgroup$
– Quuxplusone
Jan 22 at 3:24
$begingroup$
@Quuxplusone yes that certainly sounds like a coulomb explosion!
$endgroup$
– uhoh
Jan 22 at 3:28
1
1
$begingroup$
chemistry.stackexchange.com/questions/2606/…
$endgroup$
– Mithoron
Jan 21 at 19:42
$begingroup$
chemistry.stackexchange.com/questions/2606/…
$endgroup$
– Mithoron
Jan 21 at 19:42
$begingroup$
youtu.be/LmlAYnFF_s8?t=398
$endgroup$
– uhoh
Jan 21 at 23:51
$begingroup$
youtu.be/LmlAYnFF_s8?t=398
$endgroup$
– uhoh
Jan 21 at 23:51
1
1
$begingroup$
@uhoh: I believe youtu.be/e9AiK5zulf8 is a much more straightforward way to answer OP's question. :)
$endgroup$
– Quuxplusone
Jan 22 at 3:24
$begingroup$
@uhoh: I believe youtu.be/e9AiK5zulf8 is a much more straightforward way to answer OP's question. :)
$endgroup$
– Quuxplusone
Jan 22 at 3:24
$begingroup$
@Quuxplusone yes that certainly sounds like a coulomb explosion!
$endgroup$
– uhoh
Jan 22 at 3:28
$begingroup$
@Quuxplusone yes that certainly sounds like a coulomb explosion!
$endgroup$
– uhoh
Jan 22 at 3:28
add a comment |
2 Answers
2
active
oldest
votes
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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 Jan 21 at 16:14
andseliskandselisk
15k649108
$endgroup$
4
$begingroup$
According to this post, this is an incomplete explanation of the reason for explosion.
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– Ruslan
Jan 21 at 20:11
2
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@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:)
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– andselisk
Jan 21 at 20:16
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.
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add a comment |
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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 Jan 21 at 16:14
andseliskandselisk
15k649108
$endgroup$
4
$begingroup$
According to this post, this is an incomplete explanation of the reason for explosion.
$endgroup$
– Ruslan
Jan 21 at 20:11
2
$begingroup$
@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
Jan 21 at 20:16
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 Jan 21 at 16:14
andseliskandselisk
15k649108
$endgroup$
4
$begingroup$
According to this post, this is an incomplete explanation of the reason for explosion.
$endgroup$
– Ruslan
Jan 21 at 20:11
2
$begingroup$
@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
Jan 21 at 20:16
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 Jan 21 at 16:14
andseliskandselisk
15k649108
$endgroup$
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 Jan 21 at 16:14
andseliskandselisk
15k649108
edited Jan 21 at 16:19
answered Jan 21 at 16:14
andseliskandselisk
15k649108
answered Jan 21 at 16:14
andseliskandselisk
15k649108
answered Jan 21 at 16:14
andseliskandselisk
15k649108
15k649108
4
$begingroup$
According to this post, this is an incomplete explanation of the reason for explosion.
$endgroup$
– Ruslan
Jan 21 at 20:11
2
$begingroup$
@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
Jan 21 at 20:16
add a comment |
4
$begingroup$
According to this post, this is an incomplete explanation of the reason for explosion.
$endgroup$
– Ruslan
Jan 21 at 20:11
2
$begingroup$
@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
Jan 21 at 20:16
4
4
$begingroup$
According to this post, this is an incomplete explanation of the reason for explosion.
$endgroup$
– Ruslan
Jan 21 at 20:11
$begingroup$
According to this post, this is an incomplete explanation of the reason for explosion.
$endgroup$
– Ruslan
Jan 21 at 20:11
2
2
$begingroup$
@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
Jan 21 at 20:16
$begingroup$
@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
Jan 21 at 20:16
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 Jan 21 at 16:13
community wiki
Saurav Singh
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Carly is a new contributor. Be nice, and check out our Code of Conduct.
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1
$begingroup$
chemistry.stackexchange.com/questions/2606/…
$endgroup$
– Mithoron
Jan 21 at 19:42
$begingroup$
youtu.be/LmlAYnFF_s8?t=398
$endgroup$
– uhoh
Jan 21 at 23:51
1
$begingroup$
@uhoh: I believe youtu.be/e9AiK5zulf8 is a much more straightforward way to answer OP's question. :)
$endgroup$
– Quuxplusone
Jan 22 at 3:24
$begingroup$
@Quuxplusone yes that certainly sounds like a coulomb explosion!
$endgroup$
– uhoh
Jan 22 at 3:28