Vivian Marlowe
Sodium bicarbonate and alcohol do not react with each other. This is because sodium bicarbonate is a weak base, formed by a weak base (sodium hydroxide) and a weak acid (carbonic acid). Alcohol can act as a weak acid or base, similar to water. Weak acids and bases do not react with each other. When sodium bicarbonate is added to a carboxylic acid solution, carbon dioxide gas is formed, and bubbles can be observed in the solution. On the other hand, when sodium bicarbonate is added to an alcohol solution, there will be no observable reaction, indicating that the liquid being tested is an alcohol.
| Characteristics | Values |
|---|---|
| Reaction | No observable reaction |
| Reason | Sodium bicarbonate is a weak base, and alcohol can act as a weak acid/base like water. Weak acids and bases don't react with each other. |
| Distinguishing factor | The presence or absence of bubbles can indicate whether a solution contains a carboxylic acid or an alcohol. |
| Alternative test | Sodium reacts with the -OH group in water even better than with the one in an alcohol. If you add a tiny piece of sodium to a neutral liquid free of water and get bubbles of hydrogen produced, then the liquid is an alcohol. |
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What You'll Learn
Sodium bicarbonate and alcohol do not react
When a slight disturbance is introduced to the system, the baking soda is briefly dislodged from the solution, allowing vinegar to react with it. This results in minor bubbling at the top, but the solution does not boil as it typically would. The addition of a small amount of vinegar to the IPA layer allows the acetic acid to permeate and react with the bicarb that has diffused into the IPA, creating carbon dioxide bubbles and further agitating the solution.
The reaction between sodium bicarbonate, isopropyl alcohol, and acetic acid (vinegar) is a multi-step process. Firstly, the isopropyl alcohol and vinegar are mixed, forming two layers due to their different densities. The vinegar, being denser, settles at the bottom. The two substances do not immediately combine, and a slight disturbance or jolt may be necessary to initiate a reaction.
When the solution is disturbed, the vinegar and isopropyl alcohol begin to mix, and the acetic acid in the vinegar reacts with the isopropyl alcohol, resulting in minor bubbling. This is because the acetic acid in vinegar is largely undissociated and can dissolve well in alcohol. Over time, the acetic acid permeates the IPA layer, and the carbon dioxide bubbles created further agitate the solution, leading to a more complete reaction.
In summary, while sodium bicarbonate and alcohol do not react directly, the addition of vinegar to the mixture can initiate a reaction. The reaction occurs in distinct layers, with the IPA forming an upper layer and the vinegar permeating and reacting with the IPA over time. The disturbance facilitates the reaction by temporarily dislodging the baking soda from the solution, allowing the vinegar to react with it.
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Sodium bicarbonate is a weak base
The chemical compound sodium bicarbonate, also known as baking soda or bicarbonate of soda, has the formula $NaHCO_{3}$. It is a crystalline white substance that often appears as a fine powder. It has a salty and alkaline taste, similar to washing soda (sodium carbonate). Sodium bicarbonate is a weak base.
When sodium bicarbonate is dissolved in water, the following hydrolysis reaction occurs:
$$\ce{NaHCO3 + H2O -> NaOH + H2CO3}$$
However,
$$\ce{H2CO3 -> H2O + CO2}$$
So, the actual reaction is:
$$\ce{NaHCO3 -> NaOH + CO2}$$
$\ce{CO2}$ escapes, so the reaction is irreversible, and all the $\ce{NaHCO3}$ is converted to $\ce{NaOH}$, which is a strong base. This reaction is demonstrated when vinegar (acetic acid) is added to a solution of sodium bicarbonate and water. The sodium bicarbonate acts as a base, receiving a proton from the acetic acid, which then decomposes to water and carbon dioxide.
Sodium bicarbonate can also act as an acid. When coupled with a strong base like sodium hydroxide, it can give a proton. Bicarbonate decomposes into carbonate, and hydroxide decomposes into water.
In addition, sodium bicarbonate reacts with ethanol, a type of alcohol. Ethanol is used to dissolve small quantities of waste sodium. The resulting solution can be washed away safely. When a small piece of sodium is dropped into ethanol, it reacts to produce bubbles of hydrogen gas and leaves a colourless solution of sodium ethoxide.
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Alcohol is a neutral compound
The term "alcohol" in chemistry originally referred to ethanol or ethyl alcohol, the primary alcohol that is used as a drug and is the main alcohol in alcoholic drinks. Alcohols are produced by hydroxylation, the installation of a hydroxy group using oxygen or a related oxidant. The suffix "-ol" appears in the chemical name of substances where the hydroxyl group is the functional group with the highest priority.
However, when alcohol is mixed with another strong base, such as NaOH, it becomes a base. This is the typical result for ethanol, indicating that it is more commonly used as a base than an acid. When alcohol reacts with other strong bases, it produces OH–, which is a basic compound. The alcohol phenol is an exception to this rule, as it cannot be basic.
The -OH group in alcohol is neutral, while it is acidic in carboxylic acid. The reason for this is that in carboxylic acid, the -OH group is joined to the electron-withdrawing carbonyl group. In contrast, alcohol has an alkyl group with a +I effect.
In terms of the reaction between sodium bicarbonate (baking soda) and alcohol, there is little to no mixing between isopropyl alcohol ("IPA") and the saturated aqueous bicarbonate solution. IPA is fully miscible with pure water but would be "salted out" of a saturated ionic solution. IPA, being less dense, would form an upper layer in the reaction vessel. One observation is that the alcohol is changing the water's ability to dissolve the baking soda, and when a slight jolt is added to the system, the baking soda is dislodged out of the solution long enough for vinegar to react with it.
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Carboxylic acids react with sodium bicarbonate to produce CO2 and bubbles
Carboxylic acids, such as acetic acid (vinegar), react with sodium bicarbonate (baking soda) to produce carbon dioxide (CO2) gas and bubbles. This reaction is often used in science experiments to demonstrate the concept of acid-base reactions and can even be employed to create a "volcano" effect.
When carboxylic acids and sodium bicarbonate come into contact, they undergo a chemical reaction due to the interaction of their bases and acids. This reaction results in the formation of carbonic acid, which then quickly breaks down into carbon dioxide and water. The carbon dioxide escapes as gas, creating the bubbles observed in the mixture.
The reaction between carboxylic acids and sodium bicarbonate is spontaneous and exothermic, meaning it releases energy in the form of heat. This is why the mixture may feel warm to the touch after the reaction occurs. The production of carbon dioxide gas and the release of heat can be visibly noticed through the bubbling and fizzing of the mixture.
To observe this reaction, one can perform a simple experiment by mixing vinegar (a carboxylic acid) with baking soda (sodium bicarbonate). The vinegar serves as the carboxylic acid, providing the acidic component necessary to trigger the reaction. The baking soda, on the other hand, contributes the sodium bicarbonate, which reacts with the acetic acid in the vinegar.
It is important to note that this reaction may differ when sodium bicarbonate reacts with other types of alcohols, such as isopropyl alcohol. In such cases, the alcohol may affect the water's ability to dissolve the baking soda, resulting in two layers that do not immediately mix. However, with carboxylic acids, the reaction produces a distinct fizzing and bubbling effect due to the rapid release of carbon dioxide gas.
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Ethanol can be used to dissolve sodium
The reaction between ethanol and sodium is relatively gentle compared to other alcohols, such as isopropyl alcohol (IPA), which exhibits little to no mixing with a saturated aqueous bicarbonate solution. However, it is important to ensure that there is no trace of water present, as sodium reacts more readily with the -OH group in water than in alcohol.
The solubility of sodium in ethanol is concentration-dependent. Ethanol can dissolve sodium hydroxide (NaOH) up to concentrations of 10 grams of NaOH per litre. At higher concentrations, an equilibrium reaction becomes important, and the solubility of NaOH in dry ethanol is nebulous.
The reaction between sodium and ethanol can be summarised by the following chemical equation:
\(\\ce{CH_3CH_2ONa}\)
This equation represents the formation of sodium ethoxide, which is strongly alkaline. Therefore, it is crucial to handle this solution with care and properly dispose of any waste.
In summary, ethanol can be used to dissolve small quantities of sodium, resulting in the formation of sodium ethoxide. This reaction produces hydrogen gas and a colourless solution, demonstrating the presence of an alcohol. However, it is important to take safety precautions due to the hazardous nature of sodium and the resulting alkaline solution.
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Frequently asked questions
There will be no observable reaction when sodium bicarbonate is added to an alcohol solution. This is because sodium bicarbonate is a weak base and alcohol can act as a weak acid or base, and weak acids and bases do not react with each other.
If a small piece of sodium is dropped into ethanol, it reacts steadily to give off bubbles of hydrogen gas and leaves a colorless solution of sodium ethoxide.
When sodium bicarbonate is added to vinegar (a carboxylic acid), CO2 gas is formed, and bubbles can be observed in the solution.
Everyone knows that baking soda (sodium bicarbonate) and vinegar (acetic acid) react vigorously when mixed together. The solution starts creating carbonic acid that decays into carbon dioxide, thus forming bubbles.
