Glossary:
Acid - Proton donor, produces H+ ions in water, electron pair acceptor.
Aq (Aqueous) - Containing water
Base- Proton donor, produced OH- ions in water, electron pair doner.
Buffer - A substance that resists a change of pH
Concentration - Amount of substance per unit volume.
The Bronsted-Lowry theory : An acid is a proton donor and a base is a proton accepter
The Arrhenius theory: Acids are substances which produce hydrogen ions in solution. Bases are substances which produce hydroxide ions in solution.
The Lewis theory: An acid can accept a pair of electrons and a base can donate a pair of electrons.Conjugate acid- A base that recieves a proton
Electrolyte - Any liquid that conducts electricity.
Corrosive - A corrosive substance in one that can cause damage to another substance. (Acid can corrode a metal)
Conjugate base- A acid that donates a proton.
Conjugate acid - A base that gains a proton.
Proton - A positively charged particle (H+ is a proton)
pH meter - A electronic devise used to measure the pH of a solution.
Alkali - A base that dissolves in water
pH - Scale of strength of acids and bases from 0-14. Potential of H+ ions.
pOH - Scale of strength of acids and bases from 14-0. Potential of OH- ions.
M(mole) - A unit to measure an amount of chemical substance.
Ionic compound - Anything with positive and negative ions.
Salt - Any neutral ionic compound.
Indicator- Are substances that change color at a certain pH.
Blue litmus paper - An indicator that turns red in an acid and stays blue in a base or neutral solution.
Red litmus paper - An indicator that turns blue in a base and stays red in a acid or neutral solution.
Universal indicator - A versatile substance with combination of various indicators that can determine the pH of a solution.Strong Acid - Can dissociate in water to form more H+ ions then a weak acid.
Strong base - Can dissociate in water to form more OH- ions then a weak base.
Strong acid - Can dissociate in water to form more H+ ions then a weak acid.
Rough titration - A titration preformed to determine about the amount of acid added to the base in order to neutralize the solution.
Exact titration - A titration preformed to determine the exact amount of acid added to the base in order to neutralize the solution.
Meniscus - The bottom or the top of the curve of a liquid due to its container. (Always read results from eye level at the center of the meniscus.
Aq (Aqueous) - Containing water
Base- Proton donor, produced OH- ions in water, electron pair doner.
Buffer - A substance that resists a change of pH
Concentration - Amount of substance per unit volume.
The Bronsted-Lowry theory : An acid is a proton donor and a base is a proton accepter
The Arrhenius theory: Acids are substances which produce hydrogen ions in solution. Bases are substances which produce hydroxide ions in solution.
The Lewis theory: An acid can accept a pair of electrons and a base can donate a pair of electrons.Conjugate acid- A base that recieves a proton
Electrolyte - Any liquid that conducts electricity.
Corrosive - A corrosive substance in one that can cause damage to another substance. (Acid can corrode a metal)
Conjugate base- A acid that donates a proton.
Conjugate acid - A base that gains a proton.
Proton - A positively charged particle (H+ is a proton)
pH meter - A electronic devise used to measure the pH of a solution.
Alkali - A base that dissolves in water
pH - Scale of strength of acids and bases from 0-14. Potential of H+ ions.
pOH - Scale of strength of acids and bases from 14-0. Potential of OH- ions.
M(mole) - A unit to measure an amount of chemical substance.
Ionic compound - Anything with positive and negative ions.
Salt - Any neutral ionic compound.
Indicator- Are substances that change color at a certain pH.
Blue litmus paper - An indicator that turns red in an acid and stays blue in a base or neutral solution.
Red litmus paper - An indicator that turns blue in a base and stays red in a acid or neutral solution.
Universal indicator - A versatile substance with combination of various indicators that can determine the pH of a solution.Strong Acid - Can dissociate in water to form more H+ ions then a weak acid.
Strong base - Can dissociate in water to form more OH- ions then a weak base.
Strong acid - Can dissociate in water to form more H+ ions then a weak acid.
Rough titration - A titration preformed to determine about the amount of acid added to the base in order to neutralize the solution.
Exact titration - A titration preformed to determine the exact amount of acid added to the base in order to neutralize the solution.
Meniscus - The bottom or the top of the curve of a liquid due to its container. (Always read results from eye level at the center of the meniscus.