Review Titrations

Which point on the titration curve corresponds to the point at which the moles of the added strong base are equal to the moles of the weak acid initially present?

• Q

• R

• S

• T

What is the endpoint of a titration

• [OH^-] = [H₃O⁺]

• when the indicator changes color

• when there is only acid remaining

• when there is only base remaining

what is the reading on this burette?

• 4.40mL
• 3.50mL
• 3.60mL
• 4.50mL

HCl + NaOH → 

• NaH + ClOH
• NaCl + H₂
• NaCl + H₂O
• NaCl + Cl₂

30.0 ml of NaOH is neutralized by 12.3 ml of 0.20 M HCl. What is the concentration of the NaOH?

• 82 mol/l

• 0.82 mol/l

• 0.49 mol/l

• 0.082 mol/l

H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O

How many moles of H₂SO₄ will neutralize 14.2 ml of 0.010 M NaOH? 

• 1.42 x 10⁴ mol

• 7.1 x 10^-5 mol

• 1.42 x 10^-4 mol

• 7.1 x 10⁵ mol

Answer explanation

Each mole of H₂SO₄ neutralises 2 moles of NaOH

Tags

moles = conc x vol

reacting ratio

H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O

What volume of 2.00 M H₂SO₄ solution will neutralize

36.20 ml of 2.00 M NaOH solution?

• 36.20 ml

• 18.1 ml

• 0.04 ml

• 0.02 ml

Answer explanation

Each mole of H₂SO₄ neutralises 2 moles of NaOH

Tags

moles = conc x vol

vol = moles / conc

reacting ratio

H₃PO₄ + 3NaOH → Na₃PO₄ + 3H₂O

What is the concentration of the NaOH solution,

if 36.00 ml of it neutralises 25.0 ml of 2.4 M H₃PO₄ solution?

• 2.16 x 10^-3 M

• 4.5 x 10^-3 M

• 5.0 M

• 7.2 x 10^-4 M

Answer explanation

Each mole of H₃PO₄ neutralises 3 moles of NaOH

Tags

conc = moles / vol

reacting ratio

moles = conc x vol

acids as monoprotic/diprotic/triprotic

I am titrating 1.0 M HCl with 1.0 M NaOH.  I have 25mL of HCl. How much NaOH will I need?

• 2.5mL
• 5mL
• 25mL
• 50mL

If it takes 25 mL of 0.05 M HCl to neutralize 345 mL of NaOH solution, what is the concentration of the NaOH solution?

• 0.0036 M NaOH

• 0.00125 M NaOH

• 3.62 M NaOH

• 1.25 M NaOH