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Why is sodium carbonate more frequently used in neutralising acid compared to sodium hydroxide despite being a weaker base?
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Monterino Overson
Why is sodium carbonate more frequently used in neutralising acid compared to sodium hydroxide despite being a weaker base?
Sodium hydroxide is found in drain cleaner. Antacids, which combat excess stomach acid, are comprised of bases such as magnesium hydroxide or sodium hydrogen carbonate. Various common bases and corresponding uses are given in Table 14.3. 2. Mix baking soda with water Baking soda can calm some episodes of heartburn by neutralizing your stomach acid. To do this, dissolve a teaspoon of baking soda in a glass of water and drink it slowly. In fact, you should drink everything slowly when you have heartburn.
Sodium hydroxide is found in drain cleaner. Antacids, which combat excess stomach acid, are comprised of bases such as magnesium hydroxide or sodium hydrogen carbonate. Various common bases and corresponding uses are given in Table 14.3. 2. Mix baking soda with water Baking soda can calm some episodes of heartburn by neutralizing your stomach acid. To do this, dissolve a teaspoon of baking soda in a glass of water and drink it slowly. In fact, you should drink everything slowly when you have heartburn.
OK, Na carbonate froths everywhere, but you know when you have added enough as the effervescence ceases.
If you add a slight excess the solution is not super basic and you can add a bit of acid to remove it. If you add it as a solid you can quickly decant the solution from any excess and then measure the pH.
With NaOH it is difficult to monitor the reaction. You need to constantly measure the pH and you can easily overshoot.
OK, Na carbonate froths everywhere, but you know when you have added enough as the effervescence ceases.
If you add a slight excess the solution is not super basic and you can add a bit of acid to remove it. If you add it as a solid you can quickly decant the solution from any excess and then measure the pH.
With NaOH it is difficult to monitor the reaction. You need to constantly measure the pH and you can easily overshoot.
Imagine this, if you added too much NaOH to the acid, then the resulting solution would become strongly basic. Remember, strong bases can be just as toxic and corrosive as strong acids. Your skin might become a potential victim as concentrated NaOH can hydrolyse esters (fats and phospholipids). Worse yet, NaOH is very soluble in water hence anything that’s left will be able to react as a base.
With Na2CO3, this won’t be much of a problem because Na2CO3 fizzes in acid. So you’d know when the acid has been completely neutralized (no more fizzing). Even if you added too much, Na2CO3 is not the most soluble base nor is it the strongest one. Hence, you won’t have to worry sick about your pipes getting potentially devoured by excess Na2CO3.
Imagine this, if you added too much NaOH to the acid, then the resulting solution would become strongly basic. Remember, strong bases can be just as toxic and corrosive as strong acids. Your skin might become a potential victim as concentrated NaOH can hydrolyse esters (fats and phospholipids). Worse yet, NaOH is very soluble in water hence anything that’s left will be able to react as a base.
With Na2CO3, this won’t be much of a problem because Na2CO3 fizzes in acid. So you’d know when the acid has been completely neutralized (no more fizzing). Even if you added too much, Na2CO3 is not the most soluble base nor is it the strongest one. Hence, you won’t have to worry sick about your pipes getting potentially devoured by excess Na2CO3.
CaCO3 (calcium carbonate, a.k.a. chalk) doesn't dissolve in water, so it doesn't behave like a base. All acids stronger than H2CO3 (provide their calcium salts dissolve well in water) react with calcium carbonate, yielding CO2. The free hydrogen ions are consumed resulting in decreased hydrogen ion activity. In other words calcium carbonate acts to neutralise or buffer the solution by consuming hydrogen ions [8].
CaCO3 (calcium carbonate, a.k.a. chalk) doesn't dissolve in water, so it doesn't behave like a base. All acids stronger than H2CO3 (provide their calcium salts dissolve well in water) react with calcium carbonate, yielding CO2. The free hydrogen ions are consumed resulting in decreased hydrogen ion activity. In other words calcium carbonate acts to neutralise or buffer the solution by consuming hydrogen ions [8].
Explanation: Both substances will neutralize sulfuric acid perfectly well. But solid sodium hydroxide is more corrosive to human skin than sodium hydrogen carbonate is. ... So, a spilled solution of sodium hydrogen carbonate will be less caustic than a solution of sodium hydroxide. Vinegar is about 5 to 7 percent acetic acid (ethanoic acid), CH3COOH. It is a weak acid, meaning that it ionizes to only a slight extent, but it will neutralize a base, in this case, sodium hydroxide.
Explanation: Both substances will neutralize sulfuric acid perfectly well. But solid sodium hydroxide is more corrosive to human skin than sodium hydrogen carbonate is. ... So, a spilled solution of sodium hydrogen carbonate will be less caustic than a solution of sodium hydroxide. Vinegar is about 5 to 7 percent acetic acid (ethanoic acid), CH3COOH. It is a weak acid, meaning that it ionizes to only a slight extent, but it will neutralize a base, in this case, sodium hydroxide.
Safety and convenience, mostly. You can have an open tray, bag or bucket of sodium carbonate. You can grab a handful of it barehanded. You can strew it on the floor and sweep it up with a broom. If you accidentally use way too much, nothing happens.
I wouldn’t recommend doing any of those things with sodium hydroxide.
Safety and convenience, mostly. You can have an open tray, bag or bucket of sodium carbonate. You can grab a handful of it barehanded. You can strew it on the floor and sweep it up with a broom. If you accidentally use way too much, nothing happens.
I wouldn’t recommend doing any of those things with sodium hydroxide.
Sodium hydroxide is found in drain cleaner. Antacids, which combat excess stomach acid, are comprised of bases such as magnesium hydroxide or sodium hydrogen carbonate. Various common bases and corresponding uses are given in Table 14.3. 2. Mix baking soda with water Baking soda can calm some episodes of heartburn by neutralizing your stomach acid. To do this, dissolve a teaspoon of baking soda in a glass of water and drink it slowly. In fact, you should drink everything slowly when you have heartburn.
Sodium hydroxide is found in drain cleaner. Antacids, which combat excess stomach acid, are comprised of bases such as magnesium hydroxide or sodium hydrogen carbonate. Various common bases and corresponding uses are given in Table 14.3. 2. Mix baking soda with water Baking soda can calm some episodes of heartburn by neutralizing your stomach acid. To do this, dissolve a teaspoon of baking soda in a glass of water and drink it slowly. In fact, you should drink everything slowly when you have heartburn.
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OK, Na carbonate froths everywhere, but you know when you have added enough as the effervescence ceases.
If you add a slight excess the solution is not super basic and you can add a bit of acid to remove it. If you add it as a solid you can quickly decant the solution from any excess and then measure the pH.
With NaOH it is difficult to monitor the reaction. You need to constantly measure the pH and you can easily overshoot.
OK, Na carbonate froths everywhere, but you know when you have added enough as the effervescence ceases.
If you add a slight excess the solution is not super basic and you can add a bit of acid to remove it. If you add it as a solid you can quickly decant the solution from any excess and then measure the pH.
With NaOH it is difficult to monitor the reaction. You need to constantly measure the pH and you can easily overshoot.
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That’s precisely it.
Imagine this, if you added too much NaOH to the acid, then the resulting solution would become strongly basic. Remember, strong bases can be just as toxic and corrosive as strong acids. Your skin might become a potential victim as concentrated NaOH can hydrolyse esters (fats and phospholipids). Worse yet, NaOH is very soluble in water hence anything that’s left will be able to react as a base.
With Na2CO3, this won’t be much of a problem because Na2CO3 fizzes in acid. So you’d know when the acid has been completely neutralized (no more fizzing). Even if you added too much, Na2CO3 is not the most soluble base nor is it the strongest one. Hence, you won’t have to worry sick about your pipes getting potentially devoured by excess Na2CO3.
That’s precisely it.
Imagine this, if you added too much NaOH to the acid, then the resulting solution would become strongly basic. Remember, strong bases can be just as toxic and corrosive as strong acids. Your skin might become a potential victim as concentrated NaOH can hydrolyse esters (fats and phospholipids). Worse yet, NaOH is very soluble in water hence anything that’s left will be able to react as a base.
With Na2CO3, this won’t be much of a problem because Na2CO3 fizzes in acid. So you’d know when the acid has been completely neutralized (no more fizzing). Even if you added too much, Na2CO3 is not the most soluble base nor is it the strongest one. Hence, you won’t have to worry sick about your pipes getting potentially devoured by excess Na2CO3.
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CaCO3 (calcium carbonate, a.k.a. chalk) doesn't dissolve in water, so it doesn't behave like a base. All acids stronger than H2CO3 (provide their calcium salts dissolve well in water) react with calcium carbonate, yielding CO2. The free hydrogen ions are consumed resulting in decreased hydrogen ion activity. In other words calcium carbonate acts to neutralise or buffer the solution by consuming hydrogen ions [8].
CaCO3 (calcium carbonate, a.k.a. chalk) doesn't dissolve in water, so it doesn't behave like a base. All acids stronger than H2CO3 (provide their calcium salts dissolve well in water) react with calcium carbonate, yielding CO2. The free hydrogen ions are consumed resulting in decreased hydrogen ion activity. In other words calcium carbonate acts to neutralise or buffer the solution by consuming hydrogen ions [8].
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Sodium carbonate is a whole lot safer than sodium hydroxide.
An acid spill doesn’t require a strong base for neutralization, so why would you use one if a safer (though weaker) base is available?
Sodium carbonate is a whole lot safer than sodium hydroxide.
An acid spill doesn’t require a strong base for neutralization, so why would you use one if a safer (though weaker) base is available?
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Explanation: Both substances will neutralize sulfuric acid perfectly well. But solid sodium hydroxide is more corrosive to human skin than sodium hydrogen carbonate is. ... So, a spilled solution of sodium hydrogen carbonate will be less caustic than a solution of sodium hydroxide. Vinegar is about 5 to 7 percent acetic acid (ethanoic acid), CH3COOH. It is a weak acid, meaning that it ionizes to only a slight extent, but it will neutralize a base, in this case, sodium hydroxide.
Explanation: Both substances will neutralize sulfuric acid perfectly well. But solid sodium hydroxide is more corrosive to human skin than sodium hydrogen carbonate is. ... So, a spilled solution of sodium hydrogen carbonate will be less caustic than a solution of sodium hydroxide. Vinegar is about 5 to 7 percent acetic acid (ethanoic acid), CH3COOH. It is a weak acid, meaning that it ionizes to only a slight extent, but it will neutralize a base, in this case, sodium hydroxide.
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Safety and convenience, mostly. You can have an open tray, bag or bucket of sodium carbonate. You can grab a handful of it barehanded. You can strew it on the floor and sweep it up with a broom. If you accidentally use way too much, nothing happens.
I wouldn’t recommend doing any of those things with sodium hydroxide.
Safety and convenience, mostly. You can have an open tray, bag or bucket of sodium carbonate. You can grab a handful of it barehanded. You can strew it on the floor and sweep it up with a broom. If you accidentally use way too much, nothing happens.
I wouldn’t recommend doing any of those things with sodium hydroxide.
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