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WorksheetsAcid Base reactions
Total questions: 27
Worksheet time: 19mins
HA(aq) + H2O ↔ H3O+ + A-
If there is a lot of product, what does that tell you about the acid?
The following statement is true for arrhenius acid and base EXCEPT
Arrhenius acid produces H+ ions
Arrhenius base produces OH- ions
H2O need to be present for Arrhenius acid base to dissociate
Hydrogen atoms make the solution acidic
Which of the following shows the correct conjugate acid base pair?
CH3COOH (acid) / H2O (conjugate base)
CH3COOH (acid) / CH3COO- (conjugate base)
H2O (base) / H+(conjugate acid)
H2O (base) / CH3COOH (conjugate acid)
The Ka, acid dissociation constant, for an acid is 9 x 10-4 at room temperature. At this temperature, what is the approximate percent dissociation of the acid in a 1.0 M solution?
0.03%
0.09%
3%
5%
9%
Phenol, C6H5OH, has a Ka =1.0 x 10-10. What is the pH of a 0.010 M solution of phenol?
between 3-7
10
2
between 7-10
7
When sodium nitrate is dissolved in water
the solution is acidic because of the hydrolysis of the sodium ion
the solution is neutral
The solution is basic because of hydrolysis of the sodium ion
The solution is acidic because of hydrolysis of the NO2- ion
What mass of sodium cyanide must be added to 250. mL of water in order to obtain a solution having a pH of 10.50? [Ka(HCN) = 4.9 x 10–10]
240 g
0.032 g
0.059 g
0.94 g
How is a given chemical equation of any generic monoprotic weak acid written?
AH
HA
HGA
HG
What is the name of this ion: [H3O+]?
Hydroxide ion
Hydronium ion
Helium ion
Helium oxide ion
What happens to the pH of the acidic solutions when you add NaOH?
Increases
Decreases
Stays at equilibrium
It floats
A (a) contains lots of a weak acid or base and its conjugate which neutralizes added acid or base to maintain pH.
The tendency of a common ion to decrease the ionization of a weak acid
Le Chatelier's Principle
Common ion effect
Buffer
Ionization
A buffer will maintain pH over a range of
pKa ± 10
Ka ± 1
pH ± 1
pKa ± 1
Which combination would not make an effective buffer solution?
A weak acid and its conjugate base.
A weak base and its conjugate acid.
Equal concentrations of a strong acid and a strong base.
Equal concentrations of a weak acid and a weak base.
Which of the following pairs can form a buffer solution?
HCl and NaCl
NH 3 and NH 4 Cl
NaOH and H 2 O
H 2 SO 4 and Na 2 SO 4
Buffer capacity
Increases as the concentration of buffer components decreases
Decreases as the concentration of buffer components increases
Never changes
Increases as the concentration of buffer components increases
What is the primary function of a buffer solution?
To change the color of the solution based on its pH.
To conduct electricity more efficiently.
To maintain a relatively constant pH when small amounts of acid or base are added.
To increase the reaction rate of chemical reactions.
