Eggplant is often considered to be very bitter. One of the secrets chefs use to remove the bitterness is to coat the surface of the eggplant with salt. As the eggplant sits, it becomes wet and when the wetness is rinsed or wiped away the bitterness is gone. Explain what is happening to improve the flavor of the eggplant.

Short Answer

Expert verified
Salt draws water out of the eggplant through osmosis, removing bitter-tasting compounds in the process. Rinsing the eggplant then removes the extracted water and bitterness.

Step by step solution

01

Understanding Osmosis

The process that is occurring when salt is coated on the surface of the eggplant is known as osmosis. Osmosis is the movement of water through a semi-permeable membrane from an area of lower solute concentration to higher solute concentration.
02

Starting the Osmosis Process

When salt is applied to the eggplant's surface, it draws water out of the eggplant due to the higher concentration of salt (solute) outside. This is because water in the eggplant moves towards the higher concentration of salt to balance the solute levels on both sides of the eggplant's skin, which acts as a semi-permeable membrane.
03

Removal of Bitter Compounds

As water is drawn out, it also carries with it some of the bitter-tasting compounds that are soluble in water. These compounds are present within the flesh of the eggplant.
04

Rinsing Away the Bitterness

Once the eggplant has released the water and some of the bitter compounds, it is then rinsed or wiped off. This ensures that the extracted water and bitterness are completely removed from the surface, leaving the eggplant less bitter.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with Vaia!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Semi-Permeable Membrane
Imagine the skin of an eggplant. It is more than just a protective layer; it's what we describe as a semi-permeable membrane. This means that while it blocks certain substances from passing through, it allows others, like water, to move freely. In the kitchen, this characteristic is harnessed during food preparation.

When salt is sprinkled onto the surface of an eggplant, the semi-permeable nature of the skin comes into play. Water within the eggplant begins to move out towards the area where the salt concentration is higher, demonstrating the remarkable process of osmosis. This movement is selective; the membrane permits water to pass but retains most other substances inside the eggplant, including some that contribute to its bitter taste.
Solute Concentration
Understanding solute concentration is key to mastering culinary techniques like the reduction of bitterness in eggplants. By salting the eggplant, chefs take advantage of the concept that water naturally moves from a region of lower solute concentration—the inside of the eggplant—to a higher solute concentration—the salted surface.

Solutes are substances like salt or sugar that dissolve in solvents such as water. The interaction between solute and solvent on each side of the eggplant skin generates a concentration gradient. It's this gradient that provides the driving force for osmosis. Chefs exploit this scientific principle, effectively drawing out water and with it, some of the bitter tastes, thus improving the eggplant's flavor.
Removal of Bitter Compounds
Eggplants contain natural substances that can taste quite bitter to some people. These compounds, which are often water-soluble, can be reduced effectively through osmosis. The action of osmosis, induced by the salt, doesn't just remove water from the eggplant; it also pulls out these bitter compounds.

As osmosis continues due to the presence of salt, the bitter-tasting soluble substances are carried away within the water that escapes through the eggplant's semi-permeable skin. The subsequent step of rinsing removes any remaining salt and the water that contains the bitterness, resulting in a more palatable vegetable.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Calculate the grams of solute in each of the following solutions: (a) \(1.20 \mathrm{~L}\) of \(18 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) (b) \(27.5 \mathrm{~mL}\) of \(1.50 \mathrm{M} \mathrm{} \mathrm{KMnO}_{4}\) (c) \(120 \mathrm{~mL}\) of \(0.025 \mathrm{M} \mathrm{Fe}_{2}\left(\mathrm{SO}_{4}\right)_{3}\)

Calculate the molarity of the following solutions: (a) \(0.50 \mathrm{~mol}\) of solute in \(125 \mathrm{~mL}\) of solution (b) \(2.25 \mathrm{~mol}\) of \(\mathrm{CaCl}_{2}\) in \(1.50 \mathrm{~L}\) of solution (c) \(275 \mathrm{~g} \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\) in \(775 \mathrm{~mL}\) of solution (d) \(125 \mathrm{~g} \mathrm{MgSO}_{4} \cdot 7 \mathrm{H}_{2} \mathrm{O}\) in \(2.50 \mathrm{~L}\) of solution

A pot of chai tea has a volume of 600 . \(\mathrm{mL}\), a mass of 618 . \(\mathrm{g}\), and contains \(866 \mathrm{mg}\) of cinnamaldehyde \(\left(\mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}\right)\), the principal component of cinnamon. (a) What is the molarity of cinnamaldehyde in the tea? (b) What is the mass percent of cinnamaldehyde in the tea? (c) What is the mass/volume percent of cinnamaldehyde in the tea?

Automobile battery acid is \(38 \% \mathrm{H}_{2} \mathrm{SO}_{4}\) and has a density of \(1.29 \mathrm{~g} / \mathrm{mL}\). Calculate the molality and the molarity of this solution.

Some people have begun to formulate their own window-cleaning solutions using commonly available household chemicals. One formulation calls for mixing vinegar (dilute acetic acid, \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) ) with water and a small amount of detergent. A commonly used recipe contains \(14.3 \mathrm{~g}\) of acetic acid mixed with \(525.0 \mathrm{~g}\) of water and \(1.3 \mathrm{~g}\) of detergent. This recipe makes a total of \(540.0 \mathrm{~mL}\) of solution. (a) What is the mass percent of acetic acid in the window cleaner? (b) What is the molarity of acetic acid in the window cleaner?

See all solutions

Recommended explanations on Chemistry Textbooks

View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free