Chapter 14-15 Worksheet: True & False
The larger the number of acidic protons a compound has, the more acidic the compound.
false
The larger the pH, the more acidic the solution.
false
The pH at the equivalence point for all titrations at 25˚C is 7.0.
false
The pH at the equivalence point for titrations of strong monoprotic acids using strong base at 25˚C is always less then 7.0.
false
The pH at the equivalence point for titrations of weak acids using strong base at 25˚C is always less then 7.0.
false
The pH of a 0.1 M solution of HF is 1.0.
false
The pH of a 0.1 M solution of NH3 is 1.0.
false
The pH of a 0.1 M solution of NaOH is 1.0.
false
The pH of a neutral solution is always 7.0
false
The pH of pure water is always 7.0.
false
The pOH of a 0.1 M solution of HCl is 1.0.
false
The pOH of a 0.1 M solution of HF is 1.0.
false
The pOH of a 0.1 M solution of NH3 is 1.0.
false
The stronger the X-H bond, the stronger the acid.
false
All organic acids are weak acids.
true
Buffers are composed of an acid and its conjugate base.
true
CH3NH2 is a weak base.
true
Co(OH)2 is more soluble in an acidic solution than in pure water.
true
For a neutral solution the following is always true: [H+]=[OH- ].
true
For a neutral solution the following is always true: pH = pOH.
true
For acid base titrations, a strong acid or strong base is always used as a titrant.
true
For all aqueous solutions at 25˚C, [H+][OH-] = 10^-14
true
For all aqueous solutions at 25˚C, pH+pOH = 14.
true
For oxoacids, only those hydrogen bound to oxygen are acidic.
true
For oxoacids, the more electronegative the central atom, the more acidic the compound.
true
For oxoacids, the more oxygen bound to the central atom, the more acidic the compound.
true
Given the acid dissociation constant of an acid at room temperature, you should be able to determine the base dissociation constant of its conjugate base.
true
Given the hydrogen ion concentration of an aqueous solution at room temperature, you should always be able to determine the hydroxide concentration.
true
Hydrochloric acid is a strong acid.
true
If a compound behaves as a Bronsted-Lowry acid in a reaction, it necessarily is behaving as a Lewis acid.
true
If a solution of Co(OH)2 is at equilibrium and a strong acid is added, more Co(OH)2 will dissolve.
true
In an acid-base reaction, the side with the weaker acid will always be at higher concentration at equilibrium.
true
In an acid-base reaction, the side with the weaker acid will always have the weaker base.
true
In some reactions water behaves like a base, in other reactions water behaves like an acid.
true
Indicators used for acid base titrations are composed of an acid and its conjugate base.
true
Nonmetal oxides tend to form acidic solutions.
true
The conjugate bases of strong acids are neutral.
true
The hydrogen ion (H+) and hydronium ion (H3O+) mean the same thing.
true
The larger the pOH, the more acidic the solution.
true
The more polar the H-X bond, the stronger the acid.
true
The pH at the equivalence point for titrations of strong monoprotic acids using strong base at 25˚C is always 7.0.
true
The pH at the equivalence point for titrations of weak bases using strong acids at 25˚C is always less then 7.0.
true
The pH of a 0.1 M solution of HCl is 1.0.
true
The pOH of a 0.1 M solution of NaOH is 1.0.
true
The stronger the acid, the weaker its conjugate base.
true
If a compound behaves as a Lewis acid in a reaction, it necessarily is behaving as a Bronsted-Lowry acid.
false
If compound A is a stronger acid than compound B, than compound B is a stronger base than compound A.
false
Alkali metal oxides tend to form acidic solutions.
false
All bases contain the hydroxide ion.
false
Any acid and conjugate base pair will form a buffer.
false
Because of the common ion effect, BaSO4 is more soluble in sulfuric acid than in pure water.
false
For a polyprotic acid Ka1 is always less than Ka2.
false
For a polyprotic acids Ka1 is always less than Ka2.
false
Hydrofluoric acid is a strong acid.
false
If a compound A has a higher Ksp then compound B, then compound A is necessarily more soluble then compound B.
false
