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Acid/Base Review Sheet Name: Key ROA
Chemistry I
1. What is the difference between the Arrhenius definition and the
Bronsted-Lowry definition of an acid and a base?
° Arrehenivs definition fas the acid jbase 17
Atids increase Cut] and bases increase Lon-J
* BL atids are proten donors, bases are
Protn acceptors
2: Identify the acid, base, conjugate acid and conjugate base in the following:
a. HF + HO = F + H30*
A B CB CA
b. HaSOs- + H20 << H2S04 + OH
8 A CA CB
3. Define the following terms:
Arrhenius Acid- Substance that in Creases [H7] in Sslutron
. = } utrory
Arrhenius Base- substance that increases Low] in sal
Bronsted-Lowry Acid - Proten donor
(Hr)
Bronsted-Lowry Base- prefon ac ceptor
CH’)
; : 0
Monoproticacid- an acid with one proforr ex. HC), HN®3
Diproticacid- an acid with two — proors EX. Hy S04
Solu hon.
\
\
Triproticacid~ 9, gerd with three Protons ex: H3Pby
PH- @ measure of the concentration of Ha9* (hydrorian)
Neutralization- gQ reaction belween an acid and base
to produce a Salt and 120
Titration —
& Jaboratery technique used # determine the
@oncentrotion of a Solutarn
Indicator -
Q Substance sensitive Charges in pH
Endpoint- when the indicater Changes color during a
titra horn
4. Know the names and formulas for the common acids and bases.
¥ du mote’
5. Calculate the pH for the following:
a. [H30*] = 3.25x 10-9 pH 8.49
b. [H30"] = 157x103 pH > 9.80
c [HsO'}= 950x104" pH = }0.04
da [OH] = 3.25x10° — ngH = 5.44 pH= 8.5/1
e. [OH] = 575x10% pow = 7.84 pH? G-Tb