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Titration
Calculations
Properties/Theories
pH
100
In a titration, what is the solution with the unknown concentration?
What is the analyte
100
The Ka value for an acid is 1.0×10^–12. What is the Kb value for its conjugate base?
What is 1.0×10^–2
100
What is the relationship between Ka and pKa?
What is pKa = –log Ka
100
What is the concentration of OH– ions in an aqueous solution in which [H+] = 2.0×10^–3 mol dm^–3?
What is 5.0×10^–12 mol dm^-3
200
What is a buffer solution?
What is a solution that resists pH change and maintains a nearly constant pH when small amounts of acid or alkali are added
200
Ammonia has a pKb value of 4.75. What is the pH of a 1.00 x 10^-2 mol dm^-3 solution of ammonia at 298K?
What is 5.625
200
An acid-base indicator has a pKa value of 4.0. At what pH will this indicator change color?
What is 4
200
What is the hydroxide ion concentration and pH for a solution of NaOH of concentration 0.010 mol dm^–3?
What is [OH–] = 1.0×10^–2 mol dm^–3 and pH = 12.00
300
An aqueous solution of ammonia was titrated with a solution of sulfuric acid of concentration 0.150 mol dm^–3, 25.0 cm^3 of the ammonia solution required 20.1 cm^3 of the sulfuric acid solution for neutralization. What is the concentration of the ammonia solution?
What is 0.241 mol dm^–3
300
The acid dissociation constant of a weak acid has a value of 1.0×10–5 mol dm^–3. What is the pH of a 0.10 mol dm^–3 aqueous solution of that acid?
What is 3
300
What is a molecule that can either donate or accept a proton
What is amphiprotic
300
10 cm^3 of 0.01 mol dm^–3 nitric acid (HNO3) is diluted with 90 cm^3 of water. What is the pH of the resulting solution?
What is 3
400
Methyl Orange is red while in the presence of?
What is an acid
400
The Ka for an acid is 1.0×10^–2. What is the value of Kb for its conjugate base?
What is 1.0×10^–12
400
pKw for water at 283K is 14.54. What is the pH of water at this temperature?
What is 7.27
400
Determine the pOH of 0.121 mol dm–3 aqueous ammonia (pKb = 4.75)
What is 2.83
500
What is the stage of titration at which half of the amount of weak acid has been neutralized?
What is the half-equivalence point
500
For CH3COOH, Ka = 1.8×10^–5 mol dm^–3.What is the value of [H+] in a buffer solution in which [CH3COOH] = 2.0 mol dm^–3 and [CH3COO–]= 1.0 mol dm^–3?
What is 3.6×10^–5
500
what is the Kb expression for the reaction of Ammonia with water?
What is [NH4+][OH-]/[NH3]
500
Calculate the pH of a mixture of 50.0 cm^3 of 0.100 mol dm^–3 aqueous ammonia and 50.0 cm^3 of 0.0500 mol dm^–3 hydrochloric acid solution.
What is 9.25