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WorksheetsAcids and Bases/Equilibrium Quiz
Total questions: 35
Worksheet time: 25mins
Neutral
Life
What pH is the strongest base?
1
7
4
14
A Bronsted-Lowry acid:
donates H+ to another substance
accepts H+ from another substance
produces OH- to another substance
accepts OH- from another substance
In the equation below, which of the following are conjugate acid-base pairs?
HCl + NH3 → Cl- + NH4+
HCl & NH3
NH4+ & HCl
NH4+ & Cl-
HCl & Cl-
In the equation below, what is the Bronsted-Lowry base?
HCl + NH3 → Cl- + NH4+
HCl
NH3
Cl-
NH4+
HSO4- + H2O → H3O+ +SO42-
Identify the Bronsted-Lowry acid in the above reaction.
HSO4-
H2O
H3O+
SO42-
For a solution at 25oC, pH + pOH =
7
14
1.0 x 10-14
-log (1.0 x 10 -14)
If the pH of a solution is 4.0, what is the pOH?
4.0
10.0
1.0 x 10 -4
cannot be determined from the information
The pH of a solution is 8.43. What is the [H3O+] concentration?
3.7 x 10 -9 M
1.0 x 10-5.57 M
2.7 x 10-6 M
1.0 x 10-14 M
If the molarity of a Ca(OH)2 solution is 1.4 x 10-4 M, the pH of the solution is
10.45
4.00
3.55
10.00
What is the pH of a 0.075 M HF solution, assuming 5.00% dissociation in water?
2.42
11.57
1.12
12.88
What type of solution do you have if [OH-] = 3.41 x 10-4 M?
acidic
basic
neutral
explosive
Oranges have a [H3O+] of 1.70 x 10-2 M. Their pOH is
1.77
12.23
10.91
3.09
A solution of KOH is 2.5 x 10-5 M. What is the [H+] concentration?
4.60 M
9.40 M
3.98 x 10-10 M
1.0 x 10-4.60 M
What is the main purpose of acid-base titrations?
To test if reactants react.
To calculate the concentration of unknown analyte.
To calculate the concentration of known analyte.
To test quality of reactants.
What is the role of an indicator in a reaction?
To help reactants react successfully.
To bind to the analyte to form a products.
To show when the reaction has reached or past the equivalence point.
To provide a surface for the reaction to occur.
What is an equivalence point?
It is the point when enough analyte has been added.
It is the point when the amount of added titrant is equal to the amount of analyte in the solution.
It is the point when the volume of titrant is equivalent the volume of analyte.
It is the point when the concentration of titrant added is equivalent to the volume of analyte.
4.42mL
3.63mL
4.36mL
When adding base to acid the phenolphthalein indicator changes color from ... to ... at the end of the titration.
Colorless to Pink
Pink to Colorless
Red to Yellow
Colorless to Yellow
What volume of a 0.200 M KOH solution is required to titrate 50.0 mL of a 0.250 M HNO3 solution?
12.5 mL
25.0 mL
40.0 mL
62.5 mL
In a titration, a sample of H2SO4 solution having a volume of 15.00 mL required 36.42 mL of 0.147 M NaOH solution for complete neutralization. What is the molarity of the H2SO4 solution? (Make sure you check your mole ratio!)
0.178 M
0.356 M
0.0178 M
0.0356 M
A chemist prepares a solution of hydrochloric acid that is approximately 0.100 M and wants to determine its precise concentration. A 25.00 mL aliquot of the HCl solution is transferred to a flask, and after a drop of indicator is added, the HCl solution is titrated with 0.0775 M standard NaOH solution. The titration requires exactly 37.46 mL of the NaOH solution to reach the end point. What is the molarity of the HCl solution?
2.93 M
0.232 M
0.116 M
0.293 M
Which of the following shows the correct equation for the dissolution of BaCl2?
Ba 2+(aq) + Cl2-(aq) <-> BaCl2(s)
BaCl2(aq) <-> Ba 2+(aq) + 2Cl-(aq)
BaCl2(s) <-> Ba 2+(aq) + 2Cl-(aq)
Ba 2+(aq) + 2Cl-(aq) <-> BaCl2(s)
What is the Ksp expression for Cu3(PO4)2?
Ksp = [Cu+2]3[PO4-3]2
Ksp = [Cu+2]2[PO4-3]3
Ksp = [Cu+2][PO4-3]
Ksp = [Cu+2]3[PO4-3]
Which of the following is a neutralization reaction?
2Na + Cl2 → 2NaCl
CH4 + 2O2 → CO2 + 2H2O
HCl + KOH → KCl + H2O
CaCO3 → CO2 + CaO
What is the pH of a reaction between a strong acid and strong base?
0
5
10
7
HCO3- + H2O → H3O+ + CO32-
Water is acting as
a Bronsted-Lowry base
a Bronsted-Lowry acid
a strong acid
a weak acid
What is the conjugate base of H2SO4?
SO42-
H3SO4+
HSO3-
HSO4-
Which of the following statements is true?
If the H+ ion concentration in a solution increases by a factor of 10, the pH of the solution increases by 1
If the H+ ion concentration in a solution increases by a factor of 10, the pH of the solution decreases by 1
Which of the following is the correct definition for a weak acid?
Partially dissociates into hydroxide ions when dissolved in water
Fully dissociates into hydroxide ions when dissolved in water
Fully dissociates into hydronium ions when dissolved in water
Partially dissociates into hydronium ions when dissolved in water
The Ksp value for AgI is 1.5 x 10-16. This indicates that:
AgI is almost completely insoluble in water.
AgI is slightly soluble in water.
AgI is highly soluble in water.
AgI dissociates completely in water.
The products for the reaction of Ba(OH)2 and HClO4 are:
BaClO and H2Cl
BaClO4 and HOH
Ba(ClO4)2 and H2O
BaCl2 and HCO2
