Acid
Compound that gives off H+ ions in solution.
Base
Substance which gives off hydroxide ions (OH-) in solution.
Definitions of back breakers and fts
Arrhenius
acid: generates [H+] in solution
radix: generates [OH-] in solution
normal Arrhenius equation: acid + plant saltiness + water
object lesson: HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)
Brønsted-Lowery:
acid: anything that donates a [H+] (proton donor)
foundation: anything that accepts a [H+] (proton acceptor)
normal Brønsted-Lowery equation: acid + base acid + base
example: HNO2(aq) + H2O(aq) NO2-(aq)+ H3O+(aq)
Each acid has a coupled base and each base has a fuse acid. These conjugate pairs only differ by a proton. In this example: NO2- is the conjugate base of the acid HNO2 and H3O+ is the conjugate acid of the base H2O.
Lewis:
acid: accepts an electron pair
base: donates an electron pair
The advantage of this surmisal is that many more reactions can be considered acid-base reactions because they do non have to occur in solution
A salt is form when an acid and a base atomic number 18 mixed and the acid releases H+ ions while the base releases OH- ions.
This process is called hydrolysis. The pH of the salt depends on the strengths of the original acids and bases:
These salts are acidic or basic due to their acidic or basic ions. When weak acids or weak bases react with water, they make strong conjugate bases or conjugate acids, respectively,
which determines the pH of the salt
Strong Acids: These acids completely ionize in solution so they are always stand for in chemical equations in their ionized form. There are only seven (7) strong acids:
HCl, HBr, HI, H2SO4, HNO3, HClO3, HClO4
Weak Acids: These are the most common type of acids. They follow the equation:
HA(aq) H+(aq) + A-(aq)If you destiny to get a full essay, order it on our website: Orderessay
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