PH/acid-base information
http://www.morrisonlabs.com/ph_study_guide.htm
http://acid-base.com/index.php
http://www.101science.com/PH.html
http://www.shodor.org/UNChem/basic/ab/
SHIT FROM WIKIPEDIA:
-A mole is the amount of substance of a system which contains as many elementary entities as there are atoms in 12 grams of carbon 12, where the carbon 12 atoms are unbound, at rest and in their ground state.[1] The number of atoms in 12 grams (or, 0.012 kilograms) of carbon 12 is known as Avogadro's number. The currently accepted value is 6.022 1415(10) × 1023 mol-1 (2002 CODATA).
-Avogadro's number, also called Avogadro's constant (NA), named after Amedeo Avogadro, is the number of atoms in a mole of a monatomic element or the number of molecules in a mole of a compound. Avogadro's number is formally defined in the SI as the number of carbon-12 atoms in 12 grams (0.012 kg) of unbound carbon-12 in its rest-energy electronic state. The accepted value is 6.0221415×1023 atoms/mole. In the nineteenth century physicists measured the mass of one atom of hydrogen to be about 1/(6.023x1023) grams; they were trying to evaluate how many molecules of an ideal gas would fit in 1 cubic centimeter [1]. Carbon-12 was chosen as the reference substance over hydrogen because its atomic mass could be measured more accurately.
-The relationship of the atomic mass unit to Avogadro's number means that a mole can also be defined as: That quantity of a substance whose mass in grams is the same as its atomic weight. For example, iron has an atomic weight of 55.845, so a mole of iron weighs 55.845 grams. This notation is very commonly used by chemists and physicists.
-However, most chemical engineers as well as many other engineers and scientists differentiate between gram moles and kilogram moles (kgmol or kmol): 55.845 grams in a gram mole of iron and 55.845 kilograms in a kilogram mole of iron. Similarly, engineers and scientists in the United States use the pound mole (lbmol): 55.845 pounds in a pound mole of iron.
-The name mole (German Mol) is attributed to Wilhelm Ostwald who introduced the concept in the year 1902. It is an abbreviation for molecule (German Molekül), which is in turn derived from Latin moles "mass, massive structure". He used it to express the gram molecular weight of a substance. So, for example, 1 mole of hydrochloric acid (HCl) has a mass of 36.5 grams (atomic weights Cl: 35.5 u, H: 1.0 u).
-The mole is useful in chemistry because it allows different substances to be measured in a comparable way. Using the same number of moles of two substances, both amounts have the same number of molecules or atoms. The mole makes it easier to interpret chemical equations in practical terms. Thus the equation:
2H2 + O2 → 2H2O
can be understood as "two moles of hydrogen plus one mole of oxygen yields two moles of water."
Moles are useful in chemical calculations, because they enable the calculation of yields and other values when dealing with particles of different mass.
Number of particles is a more useful unit in chemistry than mass or weight, because reactions take place between atoms (for example, two hydrogen atoms and one oxygen atom make one molecule of water) that have very different weights (one oxygen atom weighs almost 16 times as much as a hydrogen atom). However, the raw numbers of atoms in a reaction are not convenient, because they are very large; for example, just one mL of water contains over 3×1022 (or 30,000,000,000,000,000,000,000) molecules.
I'LL MAKE IT PRETTY AFTER REPRO CLASS WHEN I'M NOT AT THE COMPUTER LAB OKAY
http://acid-base.com/index.php
http://www.101science.com/PH.html
http://www.shodor.org/UNChem/basic/ab/
SHIT FROM WIKIPEDIA:
-A mole is the amount of substance of a system which contains as many elementary entities as there are atoms in 12 grams of carbon 12, where the carbon 12 atoms are unbound, at rest and in their ground state.[1] The number of atoms in 12 grams (or, 0.012 kilograms) of carbon 12 is known as Avogadro's number. The currently accepted value is 6.022 1415(10) × 1023 mol-1 (2002 CODATA).
-Avogadro's number, also called Avogadro's constant (NA), named after Amedeo Avogadro, is the number of atoms in a mole of a monatomic element or the number of molecules in a mole of a compound. Avogadro's number is formally defined in the SI as the number of carbon-12 atoms in 12 grams (0.012 kg) of unbound carbon-12 in its rest-energy electronic state. The accepted value is 6.0221415×1023 atoms/mole. In the nineteenth century physicists measured the mass of one atom of hydrogen to be about 1/(6.023x1023) grams; they were trying to evaluate how many molecules of an ideal gas would fit in 1 cubic centimeter [1]. Carbon-12 was chosen as the reference substance over hydrogen because its atomic mass could be measured more accurately.
-The relationship of the atomic mass unit to Avogadro's number means that a mole can also be defined as: That quantity of a substance whose mass in grams is the same as its atomic weight. For example, iron has an atomic weight of 55.845, so a mole of iron weighs 55.845 grams. This notation is very commonly used by chemists and physicists.
-However, most chemical engineers as well as many other engineers and scientists differentiate between gram moles and kilogram moles (kgmol or kmol): 55.845 grams in a gram mole of iron and 55.845 kilograms in a kilogram mole of iron. Similarly, engineers and scientists in the United States use the pound mole (lbmol): 55.845 pounds in a pound mole of iron.
-The name mole (German Mol) is attributed to Wilhelm Ostwald who introduced the concept in the year 1902. It is an abbreviation for molecule (German Molekül), which is in turn derived from Latin moles "mass, massive structure". He used it to express the gram molecular weight of a substance. So, for example, 1 mole of hydrochloric acid (HCl) has a mass of 36.5 grams (atomic weights Cl: 35.5 u, H: 1.0 u).
-The mole is useful in chemistry because it allows different substances to be measured in a comparable way. Using the same number of moles of two substances, both amounts have the same number of molecules or atoms. The mole makes it easier to interpret chemical equations in practical terms. Thus the equation:
2H2 + O2 → 2H2O
can be understood as "two moles of hydrogen plus one mole of oxygen yields two moles of water."
Moles are useful in chemical calculations, because they enable the calculation of yields and other values when dealing with particles of different mass.
Number of particles is a more useful unit in chemistry than mass or weight, because reactions take place between atoms (for example, two hydrogen atoms and one oxygen atom make one molecule of water) that have very different weights (one oxygen atom weighs almost 16 times as much as a hydrogen atom). However, the raw numbers of atoms in a reaction are not convenient, because they are very large; for example, just one mL of water contains over 3×1022 (or 30,000,000,000,000,000,000,000) molecules.
I'LL MAKE IT PRETTY AFTER REPRO CLASS WHEN I'M NOT AT THE COMPUTER LAB OKAY