Chapter 18 true and false
The larger the pH, the more acidic the solution.
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 is1.0.
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
the larger the number of acidic protons a compound has, the more acidic the compound.
false
All organic acids are weak acids.
true
CH3NH2 is a weak base.
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 all aqueous solutions at 25C, pH+pOH=14
true
For all aqueous solutions at 25C,[H+][OH-]=10^(-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
In an acid-base reaction, the side with the weaker acid will always be at higher concentration at equilibrium.
true
In some reactions water behaves like a base, in other reactions water behaves like an acid.
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 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 compound A is a stronger acid than compound B, than compound B is a stronger base than compound A.
false
If a compound behaves as a Lewis acid in a reaction, it necessarily is behaving as a Bronsted-Lowry acid.
false
Alkali metal oxides tend to form acidic solutions.
false
All bases contain the hydroxide ion.
false
For a polyprotic acid Ka1 is always less than Ka2.
false
Hydrofluoric acid is a strong acid.
false
