Sports drinks are designed to rehydrate the body after excessive fluid depletion. Electrolytes in particular promote normal rehydration to prevent fatigue during physical exertion. Are they a good choice for achieving the recommended fluid intake?
Are they performance and endurance enhancers like they claim? Who should drink them? Typically, eight ounces of a sports drink provides between fifty and eighty calories and 14 to 17 grams of carbohydrate, mostly in the form of simple sugars. Sodium and potassium are the most commonly included electrolytes in sports drinks, with the levels of these in sports drinks being highly variable. The American College of Sports Medicine says a sports drink should contain milligrams of sodium per 8 ounces as it is helpful in replenishing some of the sodium lost in sweat and promotes fluid uptake in the small intestine, improving hydration.
In the summer of , the assistant football coach of the University of Florida Gators requested scientists affiliated with the university study why the withering heat of Florida caused so many heat-related illnesses in football players and provide a solution to increase athletic performance and recovery post-training or game.
University of Florida football player Chip Hinton testing Gatorade in , pictured next to the leader of its team of inventors, Robert Cade. Each particle of the solute is surrounded by particles of the solvent, carrying the solute from its original phase. Describe what happens when an ionic solute like Na 2 SO 4 dissolves in a polar solvent. Describe what happens when a molecular solute like sucrose C 12 H 22 O 11 dissolves in a polar solvent.
Classify each substance as an electrolyte or a nonelectrolyte. Each substance dissolves in H 2 O to some extent. Each ion of the ionic solute is surrounded by particles of solvent, carrying the ion from its associated crystal.
Learning Objectives To describe the dissolution process at the molecular level. The Dissolution Process What occurs at the molecular level to cause a solute to dissolve in a solvent?
When a solute dissolves, the individual particles of solute become surrounded by solvent particles. Eventually the particle detaches from the remaining solute, surrounded by solvent molecules in solution. Ionic Compounds and Covalent Compounds as Solutes In the case of molecular solutes like glucose, the solute particles are individual molecules. Potassium chloride is an ionic compound; therefore, when it dissolves, its ions separate, making it an electrolyte. Fructose is a sugar similar to glucose.
In fact, it has the same molecular formula as glucose. Because it is a molecular compound, we expect it to be a nonelectrolyte. A chemical compound is made up of many identical molecules formed from atoms from more than one element, attached by chemical bonds. However, not all compounds are created equally. Different things happen to ionic compounds and covalent compounds when they dissolve in water. When ionic compounds dissolve in water they go through a process called dissociation, splitting into the ions that make them up.
However, when you place covalent compounds in water, they typically do not dissolve but form a layer on top of the water. Ionic compounds are molecules consisting of oppositely charged ions, which are ions with both negative and positive charges. Covalent compounds are non-metals bound together, made up of two electrons shared between two atoms. Ionic compounds have a high melting and boiling point, but covalent compounds have a comparatively lower melting and boiling point.
This is because ionic compounds need a very large amount of energy to break their ionic bonds and separate the positive and negative charges. Sodium bromide, calcium chloride and magnesium oxide are examples of ionic compounds, while ethanol, ozone, hydrogen and carbon dioxide are examples of covalent compounds. When ionic compounds dissolve in water, they break apart into the ions that make them up through a process called dissociation.
This is important. Don't include water as a reactant when compounds dissociate into their ions while dissolving in water. While there are a few exceptions to this rule, for most situations you should use aq to indicate an aqueous solution. Featured Video. Cite this Article Format. Helmenstine, Anne Marie, Ph. Dissociation Reaction Definition and Examples. List of the Strong Acids and Key Facts.
Properties of Ionic and Covalent Compounds. Arrhenius Acid Definition and Examples. Balanced Equation Definition and Examples. Covalent or Molecular Compound Properties. Chemical Reaction vs. Chemical Equation. Ionic vs Covalent Bonds - Understand the Difference. Your Privacy Rights. To change or withdraw your consent choices for ThoughtCo.
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