Explain The Importance Of The Mole As A Unit Of Measure In The Science Of Chemistry.

Why is the mole concept important in chemistry?

Because eventually every single thing you do in chemistry will relate back to it. Some are subtle and you don't even pay much attention to it. Think about a simple chemical reaction. When you write the chemical equation, you write the mole ratio between reactants and products, the stoichiometry. For instance, a simple acid base reaction.2NaOH + H2SO4 ---> Na2SO4 + 2H2OThis means 2 moles of NaOH will react with 1 mole of H2SO4 to make 1 mole of Na2SO4 and 2 moles of water.I can't possibly list all the areas where we use this concept.Most people tend to see chemistry as a measurement science. While it's much more than that, it's not very wrong in a sense. We do measure a lot of things and that's what the general public mostly hears about. Lead content in water, how much caffeine is in your coffee, alcohol percentage in a beer, minerals in water etc etc. But most importantly, molar mass is sort of conversion factor. If I say take 1 mole of Sodium Chloride, it wouldn't make much sense for someone who isn't very familiar with the concept of moles or molar mass. But if you do, you know that I'm telling you to take 58.44 grams of Sodium Chloride.

What does concentration measure in chemistry?

Generally speaking, concentration is the ratio between the amount of a solute and the amount of the solvent or solution in which that solute is contained. These amounts can be expressed in many different ways, depending on what you are going to use concentration for or on which means of measurement are available. Common ways to express concentration are grams of solute/liters of solution and ml of solute/ 100 ml of solution.In chemistry we usually need to know not the volume or the weight of a substance but the number of its particles. The number of particles is expressed by a unit called “mole”, so the most common way to express concentration in chemistry is ‘molar concentration’, that is, the number of moles per liter of solution (not solvent).So this is what concentration measures in chemistry: the number of particles per unit volume of a mixture.(There are several other ways to express concentration in chemistry, depending on the problem you are dealing with, but the basic concept is the same.)

Why is the concept of concentration so important in chemistry?

Concentration and its implications remain very important from the initial stages of chemistry all the way through the most advanced concepts. Concentration conceptually is very important for two, of many, reasons.First: concentrations are used for chemical reactions. It tells you how much you have, in how much volume. Without concentrations it's like trying to make a recipie without amounts. A chemical reaction that requires specific amounts of reagents may just not work without the proper concentrations. To work through a replicatable chemical reaction, you have to know concentration. In some cases not knowing can even be dangerous, as not knowing the concentration of some reagents can incur risk with strong acids and bases. Another great example is pharmaceuticals. Concentration is very important, and is related to the prescribed dosage of medicine. The wrong concentration (think of the body as the solvent!) can be a serious issue.A second major reason is related to chemical testing. Concentration is directly tied to determining information like how much heavy metal is in water, or how much pesticide ran off into a nearby water source, or how strong an instance of acid rain is. The list goes on. Without concentration usage, these types of analysis would be much more difficult or even impossible.Hope this helped!

Why do people still use the mole (unit) in chemistry?

"Why they don't simply express their quantity measurement per atom, per unit volume, per molecule or etc.?"Let's take a look at these:Why not mass?Masses don't work well because atoms have different masses.  Thus, instead of just knowing the molar ratios for a reaction you would have to know the mass ratios, which would be different for each reaction and a huge pain in the ass.  Instead of just tabulating the atomic masses on the periodic table and using that relate everything to moles, there would have to be a table of reactions and the masses required for each reaction.Why not volume?It's basically the same problem as using mass.  Different compounds have different numbers of molecules/atoms per unit volume.  Also, how are you going to use volume for solids?  Would there be some combination of volume and mass? Also a huge pain in the ass.Why not molecules?This is probably the most reasonable approach.  However, chemists work with massive amounts of molecules/atoms. A single gram of hydrogen has 6,02000000000000000000000 hydrogen atoms.  We can express that in scientific notation to make it more manageable, 6X10^23 atoms, but this is clearly not convenient for bookkeeping and calculations.Why not etc.?I'm not sure what this would be.  Furloughs?  Bushels? Baker's dozens?  The mole is a very convenient way to express chemical reactions.  It incorporates the most important measurement of a chemical reaction, number of molecules/atoms, while eliminating the need for dealing with cumbersomely large numbers. If you're just now learning about moles, it might not click as to why this is the best unit for reactions. If you go on to do some work where you're dealing with lots of chemicals, you'll eventually be thankful that someone invented the convention of the mole.

What is a mole in chemistry?

The mole is the unit of measurement in the International System of Units (SI) for amount of substance. It is defined as the amount of a chemical substance that contains as many elementary entities, e.g., atoms, molecules, ions, electrons, or photons, as there are atoms in 12 grams of carbon-12 (12C), the isotope of carbon with relative atomic mass12 by definition. This number is expressed by the Avogadro constant, which has a value of 6.022140857(74)×10[math]^{23}[/math] mol−1. The mole is one of the base units of the SI, and has the unit symbol mol.Think of moles as a "chemist's dozen". Just as 12 eggs is a dozen eggs, 6.02 × 10[math]^{23}[/math] eggs is a mole of eggs. 6.02 × 10[math]^{23}[/math]molecules of oxygen is a mole of oxygen.The number of grams in a mole is different from substance to substance. If you're like most students, it's this that's confusing you. Picture it this way: a dozen elephants have a different weight than a dozen rabbits- but in each case, you have a dozen animals. Similarly, a mole of oxygen gas has a different weight than a mole of water- but in each case, you have 6.02×10[math]^{23}[/math] molecules.Why use moles? You often want to know how many molecules you have in a sample of a substance. Counting the molecules individually would be completely impractical. Even if you had a way to see the individual molecules, there are just too many, even in a tiny sample. Moles were defined to solve the problem of counting large numbers of molecules. With moles, you count the number of molecules in the sample by weighing it.bigAuthor: Fred Senese senese@antoine.frostburg.edu