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WorksheetsAcids and Bases F22
Total questions: 12
Worksheet time: 33mins
Which of these is a strong acid solution?
0.10 M HClO3(aq)
0.10 M HF(aq)
0.010 M HBr(aq)
0.10 M HNO2(aq)
0.10 M HClO(aq)
Which solution would have the lowest pH?
0.10 M NaOH(aq)
0.10 M HCOOH(aq)
0.010 M HBr(aq)
0.10 M HI(aq)
Which solution would have the highest pH?
0.10 M HF(aq)
0.10 M NaOH(aq)
0.10 M Ba(OH)2(aq)
0.050 M KOH(aq)
If a solution has a [H+] of 1.0 x 10 -5 M, the [OH-] is ____ and the solution is ______.
1.0 x 10 -9 M, acidic
1.0 x 10 -5 M, acidic
1.0 x 10 -9 M, basic
1.0 x 10 -5 M, basic
9.00, acidic
What is the pH of a 2.5 x 10-5 M HBr(aq) solution?
4.60
5.00
2.50
9.40
What is the pH of a 0.010 M Ca(OH)2 solution?
2.00
1.70
12.30
12.00
Which statement(s) are false if two different 0.10 M weak acid solutions are compared? Select all that apply.
The weaker acid will have a lower pH value.
The stronger acid will have a larger Ka value.
The stronger acid will have a higher % ionization.
The weaker acid is a better proton donor.
Use the checkboxes to select all the true statements.
A strong acid always has a lower pH reading than a weak acid.
As the concentration of a weak base decreases, pH decreases.
As the concentration of a weak acid decreases, pH decreases.
You don’t need a Ka value to calculate the pH for a strong acid.
What is the pH for a 0.25 M HCOOH(aq) (Ka = 1.8 x 10-4)?
0.60
2.18
4.35
11.82
Calculate the Kb for a weak base solution, B(aq) if the pH = 11.35 for a 0.020 M solution of B(aq).
2.5x10-4
1.1x10-1
2.2x10-3
2.8x10-4
An acidic salt usually has a _______ cation and a ________ anion.
acidic cation, basic anion
acidic cation, neutral anion
basic cation, acidic anion
neutral cation, basic anion
neutral cation, acidic anion
Which of these would be a basic salt solution?
NaBr(aq)
NH4Cl(aq)
Ba(ClO)2(aq)
Ca(NO3)2(aq)
FeCl3(aq)
