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Split the class into two teams, and one-by-one you will represent your team.
Choose your answer.
If it’s correct, your team gets 2 points.
If it’s incorrect, the other team can steal for 1 point.
To move to the next question click the flask.
Double Jeopardy- collaborate with your team mates and present an answer with
the points you want to wager.
7. A final 5 point bonus question will be up for grabs!!
8. The team with the most points wins the game.
Which reaction is a neutralization reaction?
Ca(OH) 2 (aq) + 2NaCl(aq) CaCl 2 (aq) + 2NaOH(aq)
Ca(NO 3 ) 2 (aq) +2KOH(aq) Ca(OH) 2 (S)
+2KNO 3 (aq)
H 2 SO 4 (aq) + Mg(s)  MgSO 4 (aq) + H 2 (g)
Mg(OH) 2 (aq) + 2HCl(aq)  MgCl 2 (aq) + 2H 2 O(l)
AgNO 3 (aq) + NaCl(aq)  AgCl(s) + NaNO 3 (aq)
Which statement about the titrant in a titration is true?
It is an acid
Measured with a pipette
It has an [unknown]
It’s poured in the burette
Which statement about all acid-base indicators is true?
They can be mixed together to make a universal indicator
They change colour in response to changes in pH
They are synthetic
They are toxic
What is the pH of a solution with [H+] = 2.88 x 10-4
10.46
4.45
3.54
0.459
I’m titrating with a base with a concentration of
0.87mol/L, where should I put it?
Burette
Pipette
Beaker
How sure are you in your
inner chemist?
Wager your points
accordingly!
Question
You’ve just completed a titration and found that you
added 26.7mL of 0.73mol/L NaOH to 25mL of HCl.
What is the concentration of
the HCl?
Hint – Balanced
eq’n
You’ve just completed a titration and found that you
added 26.7mL of 0.73mol/L NaOH to 25mL of HCl.
NaOH(aq) + HCl(aq)  H2O(l) + NaCl(aq)
What’s your answer?
NaOH(aq) + HCl(aq)  H2O(l) + NaCl(aq)
V = 26.7mL
n = 0.73 mol
C = 0.0195mol/L V = 25.0mL
n = 0.73 mol
C = 0.78mol/L
1:1 ratio
Therefore, the moles are the same
What is the concentration of hydrogen ions and
hydroxide ions in a solution that has a pH of 5.7?
What is the concentration of hydrogen ions and
hydroxide ions in a solution that has a pH of 5.7?
pH = 5.7
[H+] = 10-5.7 = 1.99 x 10-6
pOH = 8.3 [OH-] = 10-8.3 = 5.01 x 10-9
Write out the equation and identify and acid, base,
conjugate acid and conjugate base.
CH3COO-(aq) + H2O(l)  CH3COOH(aq) + OH-(aq)
Answer
What is the difference
between a strong base
and a weak base?
Answer
What is the net ionic equation for a
reaction with potassium hydroxide and
hydrochloric acid?
Answer
Are you more confident now?
What will you wager this time?
Question
Suppose that you are titrating an acid and base using
phenolphthalein indicator. Does it matter whether
you put the acid or the base in the Erlenmeyer flask?
Explain.
Answer
According to Arrhenius theory, how does hydrogen chloride
act when it is dissolved in water?
As a source of H +
As a source of Cl As a source of OH As a solvent
A student is doing a titration to determine the [acid]. The
student puts a base with a [known] in the burette. The
while doing the titration, the student washes the base
down the side of the Erlenmeyer flask with a small
amount of water. How will the results be affects?
The [calculated] of the acid will be higher.
The [calculated] of the acid will be lower.
The [base] will decrease during the titration.
The [acid] will not be affected.
Approximately 12mol of a substance is dissolved in 1L of
water. Analysis of a sample of the solution indicated that
the solution has a hydroxide ion concentration of 12mol/L
What is the solution?
A concentrated strong acid
A dilute weak acid
A dilute strong base
A concentrated weak base
Calculate the pH of a solution formed by diluting 50mL of
0.43mol/L HCl to a final volume of 1.0L
1.66
0.667
12.34
0.952
These questions are getting
harder!
How much to wager now?
Question
A student performed a titration on a drain cleaner that
contained sodium hydroxide. The student titrated
35.0mL of the drain cleaner and added 50.08mL of
0.409mol/L HCl to reach the equivalence point. What is
the concentration of sodium hydroxide in the drain
cleaner? What safety precautions should the student
take?
Answer
Calculate the pH of a solution with
[OH-] = 3.98 x 10-11mol/L
10.4
0.6
13.4
3.6
Which is stronger?
Explain your choice.
HClO 4
HClO 3
Be careful! Don’t
wager too
much now!
Three trials for a titration between potassium hydroxide solution and
carbonic acid are shown below. The concentration of the acid is 0.266
mol/L and 24.50 ml of acid was required to reach the endpoint. Write a
balanced equation and determine the concentration of the potassium
hydroxide solution.
Answer