Here is a glossary of the terms used throughout this website
Bronsted-Lowry theory: All bases are (H+) Proton acceptors. All acids are (H+) Proton Donors.
Arrhenius Theory: All bases dissolve in water to produce (OH-) Ions. All acids dissolve in water to produce (H+) Ions
Lewis Theory: All bases are electron pair donors. All acids are electron pair acceptors.
Acid:a substance that is a (H+) proton donor, dissolve in water to produce (H+) ions and are electron pair acceptors.
Base: All bases are (H+) Proton acceptors, dissolve in water to produce (OH-) Ions, and are electron pair donors
Alkali: A base that will dissolve in water
Conjugate acid: The acid created when a base receives a proton from an acid
Conjugate base: The base created when an acid looses a proton and gives it to a base.
Litmus Paper: A piece of paper that will change color depending on the solution its dipped into being an acid or base
pH paper: A indicator that will tell you the pH of a solution
Phenolphthalein: Indicator that turns colorless acidic and neutral solution and pink in basic solutions
Buffers: A solution whose pH will always stay the same, even if it is mixed in with a strong acid or strong base
Strength: The amount that a solution dissociates to form hydrogen ions depending whether it is an acid or base.
Concentration: The amount of moles per unit volume in a solution
Molarity = moles of solute/liters of solution
Neutralization theory: When equal amounts of both acid and base are added together, salt and water are created.
Titration: A technique that is used to determine the concentration of an unknown solution by using a solution that you do know the concentration to.
Rough titration: A titration that is preformed before the exact titration to determine the amount of acid that must be put in the flask of base
Regular titration: The step after the rough titration that gives you the exact amount of acid that is put into the flask of base to make it neutral
pOH + pH = 14
[H+] = 2nd log (-pH)
[OH-] = 2nd log (-pOH)pH = - log ([H+])
pOH = -log ([OH-])
Arrhenius Theory: All bases dissolve in water to produce (OH-) Ions. All acids dissolve in water to produce (H+) Ions
Lewis Theory: All bases are electron pair donors. All acids are electron pair acceptors.
Acid:a substance that is a (H+) proton donor, dissolve in water to produce (H+) ions and are electron pair acceptors.
Base: All bases are (H+) Proton acceptors, dissolve in water to produce (OH-) Ions, and are electron pair donors
Alkali: A base that will dissolve in water
Conjugate acid: The acid created when a base receives a proton from an acid
Conjugate base: The base created when an acid looses a proton and gives it to a base.
Litmus Paper: A piece of paper that will change color depending on the solution its dipped into being an acid or base
pH paper: A indicator that will tell you the pH of a solution
Phenolphthalein: Indicator that turns colorless acidic and neutral solution and pink in basic solutions
Buffers: A solution whose pH will always stay the same, even if it is mixed in with a strong acid or strong base
Strength: The amount that a solution dissociates to form hydrogen ions depending whether it is an acid or base.
Concentration: The amount of moles per unit volume in a solution
Molarity = moles of solute/liters of solution
Neutralization theory: When equal amounts of both acid and base are added together, salt and water are created.
Titration: A technique that is used to determine the concentration of an unknown solution by using a solution that you do know the concentration to.
Rough titration: A titration that is preformed before the exact titration to determine the amount of acid that must be put in the flask of base
Regular titration: The step after the rough titration that gives you the exact amount of acid that is put into the flask of base to make it neutral
pOH + pH = 14
[H+] = 2nd log (-pH)
[OH-] = 2nd log (-pOH)pH = - log ([H+])
pOH = -log ([OH-])