2. If 358 mL of H2SO4 is neutralized with 60.0 mL of 1.50 M NAOH, what is the initial concentration of the acid?

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Fection 2 - Titrations Lesson 5
1. 0.200 M HCI is used to neutralize 20.0 mL of 0.350 M NaOH.
a. How many moles of OH- are present?
b. How many moles of H+ are needed to neutralize the OH-?
c. What volume of 0.200 M HCl is needed?
2. If 358 mL of H2SO4 is neutralized with 60.0 mL of 1.50 M NaOH, what is
the initial concentration of the acid?
3. 78.0 mL of 2.50 M phosphoric acid is neutralized with 500.0 mL of
potassium hydroxide. What is the concentration of the base?
4. When titrating 0.150 M HC with a calcium hydroxide solution of unknown
concentration. 35.0 mL of acid are required to neutralize 25.0 mL of the
base.
Transcribed Image Text:Fection 2 - Titrations Lesson 5 1. 0.200 M HCI is used to neutralize 20.0 mL of 0.350 M NaOH. a. How many moles of OH- are present? b. How many moles of H+ are needed to neutralize the OH-? c. What volume of 0.200 M HCl is needed? 2. If 358 mL of H2SO4 is neutralized with 60.0 mL of 1.50 M NaOH, what is the initial concentration of the acid? 3. 78.0 mL of 2.50 M phosphoric acid is neutralized with 500.0 mL of potassium hydroxide. What is the concentration of the base? 4. When titrating 0.150 M HC with a calcium hydroxide solution of unknown concentration. 35.0 mL of acid are required to neutralize 25.0 mL of the base.
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