some dilute sulfuric acid H2S of forehead concentration of 4.90 gram /cubic decimeter what is its concentration in mol/cubic decimeter
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Book: ChemPRIME (Moore et al.)
3: Using Chemical Equations in Calculations
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3.11: Solution Concentrations
Last updated6 Nov 2020
3.10.4: Sports, Physiology, and Health- Muscle Energy from ATP
3.11.1: Biology- Solution Concentrations and Cells
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Contributed by Ed Vitz, John W. Moore, Justin Shorb, Xavier Prat-Resina, Tim Wendorff, & Adam Hahn
ChemPRIME at Chemical Education Digital Library (ChemEd DL)
In the laboratory, in your body, and in the outside environment, the majority of chemical reactions take place in solutions. Macroscopically a solution is defined as a homogeneous mixture of two or more substances, that is, a mixture which appears to be uniform throughout. On the microscopic scale a solution involves the random arrangement of one kind of atom or molecule with respect to another.
There are a number of reasons why solutions are so often encountered both in nature and in the laboratory. The most common type of solution involves a liquid solvent which dissolves a solid solute. (The term solvent usually refers to the substance present in greatest amount. There may be more than one solute dissolved in it.) Because a liquid adopts the shape of its container but does not expand to fill all space available to it, liquid solutions are convenient to handle. You can easily pour them from one container to another, and their volumes are readily measured using graduated cylinders, pipets, burets, volumetric flasks, or other laboratory glass-ware. Moreover, atoms or molecules of solids dissolved in a liquid are close together but still able to move past one another. They contact each other more frequently than if two solids were placed next to each other. This “intimacy” in liquid solutions often facilitates chemical reactions.