Self Test 7-A
Which is the conjugate base of HCO3-? H2CO3 OH- H3O+ (CO3)-2
(CO3)-2
Which of the following cannot be a Bronsted-Lowry acid? H2CO3 NH3 (SO4)-2 NH4+
(SO4)-2
What is the molarity of a solution that contains 4 grams of NaOH in 500 mol solution? (Formula mass of NaOH=40 u)
.2 M
If 10 mL of HCl neutralizes 15 mL of .4 M solutions of NaOH, the molarity of the HCl is
.60
Which water solution has the highest concentration of H3O+ ions?
1 M H2SO4
If [OH-]= 1 x 10^-4 at 298 K for a given solution, the [H+] of the solution is equal to
1 x 10^-10
Phenolphthalein will be pink in a solution whose H3O+ ion concentration in moles per liter is
1 x 10^-9
Which solution contains exactly .5 mol of H2SO4? (1.0 L of .50 M solution)
1.0 L of .50 M solution
What is the pOH of a solution whose hydronium ion concentration is .ooo1 M?
10
Which value for Ki describes the ionization of the strongest acid?
10^-1
Which group contains elements whose hydroxides are strong bases?
1A
In the reaction H3PO3 + 2OH- --> HPO3-2 + 2HOH, the number of protons donated per molecule of H3PO3
2
The pH of a .001 M solution of HCl (aq) is approximately
3
What is the missing coefficient for OH- In the following reaction? H3PO4 + __OH- --> (PO4)-3 + __HOH
3
How many moles of sodium hydroxide (NaOH) are required to exactly neutralize 2 mol of sulfuric acid (H2SO4)?
4
When one mole of (NH4)3PO4 dissolves in water, the number of moles of ions formed is
4
How many mL of .80 M HCl are required to exactly neutralize 50 mL of .4 M KOH?
40
Equal volumes of .1 M solutions of KOH and HNO3 are mixed. The pH of the resulting solution is closest to
7
Which reaction illustrates amphoterism? (H2O + H2O --> H3O+ + OH-)
H2O + H2O --> H3O+ + OH-
In the reaction HS- + H2O <--> H3O+ + S-2, the two Bronsted-Lowry bases are
H2O and S-2
When NaOH reacts w HC2H3O2 in water solution, which ion or molecule acts as the Bronsted-Lowry strong acid?
H3O+
Which Bronsted-Lowry acid has a conjugate base that has amphoteric properties?
H3O+
Which formula represents a hydrated proton?
H3O+
Which pair of ions is present in the greatest quantity in a solution of nitric acid?
H3O+, NO3-
Which of the following is the weakest Bronsted acid? HBr HI HCl HF
HF
Which acid is almost completely ionized in a dilute solution at 298 K?
HNO3
Which substance is nearly 100% ionized in water soln?
HNO3
Which of the following has amphoteric properties? HCl HNO3 H3O+ HSO4-
HSO4-
In a rxn between NaOH and HCL in water solution, which ion is a spectator ion?
Na+
The ionization of acetic acid at equilibrium may be represented by HC2H3O2 (aq) + H2O (l) <--> H3O (aq) + + C2H3O2- (aq) The addition of which ion will cause an increase in the concentration of C2H3O2-(aq)?
OH-
In the reaction S-2 + HSO4- <--> HS- + (SO4)-2, the two Bronsted-Lowry bases are
S-2 and (SO4)-2
Which of the following reacts with HCl solution to produce H2 gas?
Zn
In a solution of acetic acid (whose formula may be written HC2H3O2 or CH3COOH), which relationship is correct?
[CH3COOH] > [CH3COO-] x [H+]
In the reaction NH3 (g) + HCl (g) <--> NH4Cl (s), the NH3 acts as
a proton acceptor
According to the Arrhenius theory, a substance that yields Hydrogen ions as the only positive ion in an aqueous solution is
an acid
A solution at 25 degrees C with a pH of 7 contains
an equal number of H3O+ and OH- ions
A water solution of K2SO4 contains
both H3O+ and OH- ions
When hydrochloric acid is neutralized by sodium hydroxide, the salt formed is sodium
chloride
A water solution of NaCl and a water solution of HCl are similar in that both solutions
contain H3O+ ions
As .1 mol Ba(OH)2 (s) dissolves in 1 L of .1 M H2SO4, the conductivity of the solution
decreases
As excess HCl soln is added to a beaker containing NaOH solution, the pH of the mixture in the beaker
decreases continuously past 7
The rxn between OH- and H3O+ to form H2O is
exothermic
In pure water, ionization increases as temperature increases. At temperatures greater than 25 degrees C, the value for Kw is
greater than 1.0 x 10^-14
In pure water, ionization increases as temperature increases. At temperatures greater than 25 degrees C, the value for [H3O+] is
greater than 1.0 x 10^-7
An acid that has an ionization constant of 2.0 x 10^-7 is stronger than
hydrosulfuric acid
If the pH of a solution is 5, the number of hydronium ions per liter of this solution is greater than the number of
hydroxide ions
A water solution of NaC2H3O3 has a pH > 7 because the solution contains more
hydroxide than hydronium ions
As conjugate acid strength decreases, the strength of conjugate bases
increases
Weak electrolytes in aqueous solutions attain equilibrium between
ions and undissociated molecules
All solutions that conduct electric current contain
ions which are free to move
When pH = 4.25, the value for [H3O+] is
less than 1.0 x 10^-4
Which term is applied to any reaction between hydroxide and hydronium ions in a water solution?
neutralization
Compared to its conjugate base, a Bronsted-Lowry acid possesses
one more proton
The best way to increase the pH of an aqueous solution is to add
potassium hydroxide
The Kw value for a sample of water at 1 atm and 298 K will be most likely to change when there is an increase in the
temperature
Compared to its conjugate base, a conjugate Bronsted-Lowry acid possesses
the same number of electrons
In the rxn (CO2)-2 + H2O <--> HCO3- + OH-, the water molecule serves as a
weak acid
