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How does sodium sulphate react with ammonium nitrate?
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Michael Davison
How does sodium sulphate react with ammonium nitrate?
Here's how to figure this kind of question out. Notice that both compounds are ionic and binary. Meaning each has cations and anions with balanced charges to make them neutral. So, when you are that, you predict a double replacement reaction.
AB + CD →AD + CB (not BC since B is an anion and cations are written first in a formula).
So, you can predict possible products in this case of sodium nitrate and ammonium sulfate. But just because you can logically predict the possible products doesn't mean they'll actually form. One type of double replacement will yield an unstable product that will produce a gas. Another will be an acid-base neutralization and produce a salt and water. And the third type would produce an insoluble product that will precipitate out of solution. So in each of those cases, two binary compounds in aqueous solution produce a different phase product, either a solid precipitate, liquid water, or a gas. If none of the above happens, no reaction will take place.
So, in this case you have a bicarbonate base and no acid, so it can't be acid-base neutralization. It has no gaseous molecules that could be formed, so the only possiblity is a precipitation reaction. But if one looks up the solubility in water of sodium nitrate, all sodium compounds are soluble, and of ammonium sulfate, and all ammonium compounds are soluble. So there is nothing to drive a reaction. So the answer is there's no reaction.
Here's how to figure this kind of question out. Notice that both compounds are ionic and binary. Meaning each has cations and anions with balanced charges to make them neutral. So, when you are that, you predict a double replacement reaction.
AB + CD →AD + CB (not BC since B is an anion and cations are written first in a formula).
So, you can predict possible products in this case of sodium nitrate and ammonium sulfate. But just because you can logically predict the possible products doesn't mean they'll actually form. One type of double replacement will yield an unstable product that will produce a gas. Another will be an acid-base neutralization and produce a salt and water. And the third type would produce an insoluble product that will precipitate out of solution. So in each of those cases, two binary compounds in aqueous solution produce a different phase product, either a solid precipitate, liquid water, or a gas. If none of the above happens, no reaction will take place.
So, in this case you have a bicarbonate base and no acid, so it can't be acid-base neutralization. It has no gaseous molecules that could be formed, so the only possiblity is a precipitation reaction. But if one looks up the solubility in water of sodium nitrate, all sodium compounds are soluble, and of ammonium sulfate, and all ammonium compounds are soluble. So there is nothing to drive a reaction. So the answer is there's no reaction.
Here's how to figure this kind of question out. Notice that both compounds are ionic and binary. Meaning each has cations and anions with balanced charges to make them neutral. So, when you are that, you predict a double replacement reaction.
AB + CD →AD + CB (not BC since B is an anion and cations are written first in a formula).
So, you can predict possible products in this case of sodium nitrate and ammonium sulfate. But just because you can logically predict the possible products doesn't mean they'll actually form. One type of double replacement will yield an unstable product that will produce a gas. Another will be an acid-base neutralization and produce a salt and water. And the third type would produce an insoluble product that will precipitate out of solution. So in each of those cases, two binary compounds in aqueous solution produce a different phase product, either a solid precipitate, liquid water, or a gas. If none of the above happens, no reaction will take place.
So, in this case you have a bicarbonate base and no acid, so it can't be acid-base neutralization. It has no gaseous molecules that could be formed, so the only possiblity is a precipitation reaction. But if one looks up the solubility in water of sodium nitrate, all sodium compounds are soluble, and of ammonium sulfate, and all ammonium compounds are soluble. So there is nothing to drive a reaction. So the answer is there's no reaction.
Here's how to figure this kind of question out. Notice that both compounds are ionic and binary. Meaning each has cations and anions with balanced charges to make them neutral. So, when you are that, you predict a double replacement reaction.
AB + CD →AD + CB (not BC since B is an anion and cations are written first in a formula).
So, you can predict possible products in this case of sodium nitrate and ammonium sulfate. But just because you can logically predict the possible products doesn't mean they'll actually form. One type of double replacement will yield an unstable product that will produce a gas. Another will be an acid-base neutralization and produce a salt and water. And the third type would produce an insoluble product that will precipitate out of solution. So in each of those cases, two binary compounds in aqueous solution produce a different phase product, either a solid precipitate, liquid water, or a gas. If none of the above happens, no reaction will take place.
So, in this case you have a bicarbonate base and no acid, so it can't be acid-base neutralization. It has no gaseous molecules that could be formed, so the only possiblity is a precipitation reaction. But if one looks up the solubility in water of sodium nitrate, all sodium compounds are soluble, and of ammonium sulfate, and all ammonium compounds are soluble. So there is nothing to drive a reaction. So the answer is there's no reaction.
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