Titrations Group Activity Worksheet
Name: ______Date: ______Period: _____
Titration Group Activity Worksheet
Individual
1) Write the balanced chemical reaction for the neutralization of HCl by NaOH in water.
2) When a strong acid or a strong base dissociates in water they do so completely so that the [H+] and the [OH-] equal the concentrations of the acid or base.
- What is the concentration of [H+] in a solution of 0.10 M HCl?
- What is the concentration of [OH-] in s solution of 0.050 M NaOH?
3) What is the pH of each solution? (Show the equation and work)
4) What is the number of moles of H+ in 20.0 mL of a 0.10 M solution of HCl? (Show your calculation)
5) In order to neutralize 20.0 mL of 0.10 M HCl an equal amount of moles of hydroxide ions (OH-) must be added. What volume of 0.050 M NaOH would be required to neutralize the acid? (Show your calculation)
Name: ______Date: ______Period: _____
Titration Group Activity Worksheet
Individual
1) Write the balanced chemical reaction for the neutralization of HCl by NaOH in water.
2) When a strong acid or a strong base dissociates in water they do so completely so that the [H+] and the [OH-] equal the concentrations of the acid or base.
- What is the concentration of [H+] in a solution of 0.10 M HCl?
- What is the concentration of [OH-] in s solution of 0.050 M NaOH?
3) What is the pH of each solution? (Show the equation and work)
4) What is the number of moles of H+ in 20.0 mL of a 0.10 M solution of HCl? (Show your calculation)
5) In order to neutralize 20.0 mL of 0.10 M HCl an equal amount of moles of hydroxide ions (OH-) must be added. What volume of 0.050 M NaOH would be required to neutralize the acid? (Show your calculation)
6) What is the pH of the neutralized solution?______What is the [H+] of the neutralized solution? ______
7) What is the volume of the .050M NaOH is required to neutralize 200.0 mL of the 0.10 M HCl?
Solve with your group…but what if you didn’t have enough?
8) Suppose you added 50.0 mL of 0.25 M NaOH to 200.0 mL of 0.10 M HCl.
- Would the solution be neutral?
- How many moles of OH- have been added? (Show your calculation)
- How many moles of H+ have been added? (Show your calculation)
9) Which is the limiting reagent? Which is in excess?
10) How many moles of the excess reactant are left after the reaction is complete? (Show your calculation)
moles un-reacted excess reactant = (initial moles excess reactant) – (moles reacted excess reactant)
11) Calculate the [H+] and the pH of the solution that exists after the reaction is complete. (Show your calculation)
[H+] = __mole un-reacted H+__ total volume of solution = initial vol + added volume
total volume of solution
6) What is the pH of the neutralized solution?______What is the [H+] of the neutralized solution? ______
7) What is the volume of the .050M NaOH is required to neutralize 200.0 mL of the 0.10 M HCl?
Solve with your group…but what if you didn’t have enough?
8) Suppose you added 50.0 mL of 0.25 M NaOH to 200.0 mL of 0.10 M HCl.
- Would the solution be neutral?
- How many moles of OH- have been added? (Show your calculation)
- How many moles of H+ have been added? (Show your calculation)
9) Which is the limiting reagent? Which is in excess?
10) How many moles of the excess reactant are left after the reaction is complete? (Show your calculation)
moles un-reacted excess reactant = (initial moles excess reactant) – (moles reacted excess reactant)
11) Calculate the [H+] and the pH of the solution that exists after the reaction is complete. (Show your calculation)
[H+] = __mole un-reacted H+__ total volume of solution = initial vol + added volume
total volume of solution