Names
Acids & Bases
Acids & Bases
Ca(OH)2
Calcium hydroxide
This is the species formed after an acid has donated its proton.
Conjugate Base
Calculate the pH when 100 mL of 0.1 M HCl is mixed with 100 mL of 0.1 M NaOH.
7 (neutral)
Potassium Hydroxide
KOH
These are the two primary products typically formed when an Arrhenius acid reacts with an Arrhenius base.
salt and water
HBr
Hydrobromic Acid
This is the conjugate acid of the common solvent H2O.
H3O+ (Hydronium ion)
If a solution's [H+] concentration is 1.0 x 10^-2 M, is the solution acidic, basic, or neutral?
Acidic
Strontium Hydroxide
Sr(OH)2
This is the specific chemical formula of the salt produced by the reaction of HCl and NaOH
NaCl
HClO2
Chlorous Acid
In the reaction NH3 + H2O <--> NH4+ + OH-, this species acts as the conjugate acid.
NH4+ (ammonium ion)
This is the [H+] concentration of a solution with a pH of 9.
1.0 x 10^-9 M
Nitrous Acid
HNO2
When Magnesium Hydroxide, a base found in antacids, reacts with stomach acid (HCl), this salt is formed.
MgCl2
H2Cr2O7
Dichromic acid
The conjugate base of the hydrogen sulfate ion, HSO4-.
sulfate ion (SO4)
If a solution has an [OH-] of 4.8 x 10-3 M, this is its corresponding [H+] concentration.
2.1 x 10-12 M
Tartaric Acid
H2C4H4O6 or C4H6O6
The following reaction needs to be neutrally balanced. Add the correct subscripts where needed
HSO4 + BeOH --> 2H2O + BeSO4
H2SO4 + Be(OH)2 --> 2H2O + BeSO4
Hydroxide accepts a proton to become _______
water
H2O
When nitric acid loses a proton, it forms this specific ion, which serves as its conjugate base.
NO3
Calculate the pOH of a solution where
[H+] = 9.87 x 10-3 M.
2.01
(2 if rounded)
Thiosulfuric Acid
H2S2O3
The following reaction needs to be fully balanced. Add the correct subscripts and coefficients where needed.
CaOH + HPO4 -> CaPO4 + H2O
3Ca(OH)2 + 2H3PO4 -> Ca3(PO4)2 + 6H2O