In general, slow-moving oils are liquid at room temperature. Oils that are firm at room temperature will accelerate trace in soap. Examples of oils and butters that accelerate trace are palm oil , coconut oil , all butters, palm kernel flakes , beeswax , and castor oil. Click here to learn more about common soapmaking oils and butters. Choosing the right soapmaking oils is the first step to a successful swirled design. Some of the most popular slow moving oils are pure olive oil , canola oil , sweet almond oil , sunflower oil , avocado oil , apricot kernel oil , rice bran oil and chia oil.
Keep in mind some slow-moving oils are slower than others. For example, I would categorize rice bran oil as slow moving, but it does accelerate trace more than pure olive oil. From my experience the slowest-moving oils are canola oil , pure olive oil and sweet almond oil. To learn more about formulating your own cold process recipes, click here. Looking for some recipes that are suitable for swirls? Check out the tutorials below! Every soaper has their temperature preference, which may vary from recipe to recipe.
Many soapers prefer to soap at room temperature when making a complex swirled soap. Even adjusting your temperatures by just 10 degrees can make a huge difference in the texture of your soap batter. They emulsify oils and lye solution within minutes, or even seconds. But, stick blenders emulsify oils and lye so quickly that it can be easy to over-emulsify to a trace unsuited for swirls. Once you over-blend your soap, there is no way to get that lovely thin to medium trace back.
Stick blending your batter for too long can lead to a thick trace which inhibits the ability to swirl. Pulse the stick blender in short bursts. And remember, you can always stick blend more later! Once you reach a thin trace, I prefer to use a whisk to stir in my colorants. I also whisk in my fragrance oil last. This gives me the most time to work with my batter before it starts to thicken. After all, fragrance oils can be made up of hundreds of essential oils and aroma chemicals though most are made of a handful.
Adding them in the middle of the sopp making process can produce varying results. From separation to ricing, you can see some of the negative effects of misbehaving fragrance oil in the Soap Behaving Badly post. Luckily, Bramble Berry tests all fragrance oils thoroughly to make sure they behave well in cold process soap. If creating a swirled soap design, use a fragrance oil that does not accelerate trace. A fragrance that causes acceleration will thicken the soap batter once mixed in.
If the design requires a thick trace, an accelerating fragrance oil is great. Not sure how the fragrance oil behaves? Bramble Berry includes fragrance oil testing notes on each fragrance oil product page. My last swirling tip, and maybe the most important? A great example of this is the spin swirl technique above. With every batch of soap you learn and get better. Do you have any tips or tricks for creating swirled cold process soap?
Do you have a favorite swirl technique? Enter your email address below and you will receive all our new posts directly in your email inbox. Your spin swirls look amazing. I just completed my 4th and yet another failed batch!
So frustrating!!!! I thought it would look better if I planed the surface but nope! Spin swirling is a more advanced technique. How do the results in each cup look different?
Why do you think this is the case? Now, take cup number one and add one additional tablespoon of 3 percent hydrogen peroxide to the cup. Swirl the cup slightly to mix the solution.
What happens now? Looking at all your results, what do you think is the limiting factor for the catalase reaction in your cups? Extra: Repeat this activity, but this time do not add dish soap to all of the reactions.
What is different once you remove the dish soap? Do you still see foam formation? Extra: So far you have observed the effect of substrate H 2 O 2 concentration on the catalase reaction. What happens if you keep the substrate concentration constant but change the concentration of the enzyme? Try adding different amounts of yeast solution to three tablespoons of hydrogen peroxide, starting with one teaspoon.
Do you observe any differences, or does the concentration of catalase not matter in your reaction? Extra: What happens if the environmental conditions for the enzyme are changed?
Repeat the catalase reaction but this time vary conditions such as the pH by adding vinegar an acid or baking soda a base , or change the reaction temperature by heating the solution in the microwave. Can you identify which conditions are optimal for the catalase reaction? Are there any conditions that eliminate the catalase activity? Extra: Can you find other sources of catalase enzyme that you could use in this activity?
Research what other organisms, plants or cells contain catalase and try using these for your reaction. Do they work as well as yeast? Build a Cooler. Make a Potato Shrink--with Saltwater. Get smart. Sign up for our email newsletter. Sign Up. Support science journalism. Knowledge awaits.
See Subscription Options Already a subscriber? Create Account See Subscription Options. Extraction 2 Return the aqueous layer to the separatory funnel.
There is no need to wash the funnel in between extractions. Stopper the funnel, invert and shake with venting, then allow the layers to separate. At this step, there should be two layers in the separatory funnel. If two layers aren't present, it's likely that the wrong layer was added to the funnel in step 2 a common mistake. One way to test if this was the mistake is to add a bit of water from a squirt bottle.
If the layer returned to the separatory funnel is the organic layer incorrect , the squirt bottle water will not mix with the solution, and will instead fall as droplets to the bottom. If the organic layer incorrect was accidentally returned to the separatory funnel, there is no harm done, as the organic layer was simply diluted. Pour the liquid back into the flask designed for the organic layer, and instead add the aqueous solution to the funnel. Drain the bottom aqueous layer into an Erlenmeyer flask: it is acceptable to use the same flask that was used for the aqueous layer in the first extraction that may have been labeled "bottom aqueous layer".
Since it is most common to combine the organic layers in multiple extractions, the top organic layer can be poured out of the separatory funnel into the same flask that was used for the organic layer in the first extraction that may have been labeled "top organic layer".
Organic Layer is on the Bottom In this section are stepwise instructions on how to extract an aqueous solution with an organic solvent that is denser than water the organic layer will be on the bottom.
After allowing the layers to separate in the funnel, drain the bottom organic layer into a clean Erlenmeyer flask and label the flask, e. Do not drain the top aqueous layer from the funnel. Stopper the funnel, invert and shake gently for 1 minute with venting, then allow the layers to separate. Since it is most common to combine the organic layers in multiple extractions, the bottom organic layer can be drained from the separatory funnel into the same flask that was used for the organic layer in the first extraction that may have been labeled "bottom organic layer".
Stopper the funnel, invert and shake gently with venting, then allow the layers to separate. Troubleshooting This section descries common problems and solutions in extractions. There is Only One Layer The most common reason for having only one layer in a separatory funnel when there should be two as in when the procedure tells you to "separate the layers" , is to have made a mistake. There are Three Layers The most common reason for three layers in a separatory funnel is inadequate mixing Figure 4.
There is Insoluble Material at the Interface A small amount of insoluble film between two layers is not uncommon during an extraction. The Interface Cannot be Seen On occasion the compounds in a separatory funnel are so dark that they obscure the interface between the two layers. The Layers Don't Separate Well An Emulsion Formed Emulsions are when tiny droplets of one layer are suspended in the other layer, resulting in no distinct interface between the two layers Figure 4.
Emulsions can happen for several reasons: The density of each layer may be so similar that there is weak motivation for the liquids to separate. There may be soap-like compounds or other emulsifying agents present that dissolve some of the components in one another.
Nonetheless, if an emulsion does form, there are some ways to attempt to clarify them: For mild emulsions, gently swirl the layers and try to knock down suspended droplets with a glass stirring rod.
Allow the solution to sit for a period of time even until the next lab period if possible. With enough time, some solutions do settle out on their own. This of course may not be practical. For small volumes, use a centrifuge if one is available. A centrifuge hastens the process of letting an emulsion settle on its own. Remember that a centrifuge needs to be balanced or it may wobble off the benchtop. Divide the solutions equally, putting tubes of equal volume opposite one another inside the centrifuge.
If an emulsion is formed because the two layers have similar densities, try to alter the density of each layer to make them more different. To help clarify an emulsion, try to decrease the density of the top layer or increase the density of the bottom layer. Alternatively add additional ethyl acetate, which will dilute the organic layer and lower its density. As a last resort add some pentane, which will mix with the top organic layer and decrease its density pentane is one of the least dense organic solvents.
The addition of pentane is used as a final effort as it will negatively affect the ability of the organic layer to extract somewhat polar compounds. If an emulsion occurs with an aqueous solution top layer and dichloromethane bottom layer , add some water from a squirt bottle to dilute the top layer and decrease its density. This method worked well to clarify the emulsion in Figure 4. Try decreasing the solubility of one component in the other. The inversions were done very slowly in order to see the extractions stepwise.
With even gentle mixing the methyl red and thus color extracts rapidly. Mix the Solutions for microscale extraction Pour the contents to be extracted into a conical vial, or a glass tube with a tapered end e.
As these containers are prone to tip, use a beaker Figure 4. Methyl salicylate is a naturally occurring compound that we will use to produce salicylic acid, which will then be used to make the wonder drug aspirin acetylsalicylic acid. This is not the source of salicylic acid in the industrial synthesis of aspirin, but it is, nevertheless, a good one for laboratory use. Two different chemical techniques will be employed. First is hydrolysis, which is the breaking of a bond with water.
Esters are quite easily hydrolyzed into their two starting components, an acid and an alcohol. Then, we perform an ester synthesis for the formation of aspirin.
Equilibrium favors hydrolysis, but using acetic anhydride as the acid source prevents this backward reaction, since water is not produced during ester formation.
Both salicylic acid and aspirin are easily isolated. Methyl salicylate an ester can be hydrolyzed to produce salicylic acid. The two different functional groups on the aromatic ring are utilized in this lab. First, the free carboxylic acid group will be produced when we hydrolyze the methyl salicylate. Methanol is the alcohol which is released by hydrolysis.
Second, the hydroxyl group on salicylic acid will be used in ester formation to produce aspirin. When we performed an ester synthesis previously, we took special precautions to prevent water from being produced we included a dessicant in the reaction mixture and had a drying tube affixed on top of the reflux column.
Acetic anhydride will be used in this experiment so that when ester is formed, water is not produced. As a result, the thermodynamic equilibrium will now be for the formation of an ester instead of its hydrolysis. Before proceeding with the experiment you should review several items. First, you should be familiar with the ester functional group.
Esters are formed when an acid and an alcohol combine. You should be able to quickly identify an ester by looking at the structural formula. There are only three types of compounds which have an oxygen located between two carbons. These are ethers, esters and acid anhydrides.
Can you identify the differences? Second, we will perform a hydrolysis reaction. Hydrolysis occurs when water is used to break a bond. Hydrolysis can occur in either basic or acidic conditions. We will learn later the actual mechanisms, but in both cases we produce one chemical which is an alcohol and the other chemical will be a carboxylic acid when esters are hydrolyzed.
Third, we will produce an ester. It should be noted that ester formation cannot occur in the presence of base, only acid. During the first day of this lab, we will produce salicylic acid. This acid will then be used to make aspirin. The synthesis of aspirin is a multi-billion dollar a year chemical. While salicylic acid as some therapuetic value, it is not as effective as aspirin in reducing inflammation and other common medical conditions for which aspirin can be used.
Procedure This experiment is composed of two parts. The first involves the hydrolysis of methyl salicylate in order to produce salicylic acid Day 1.
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