Acid Base Calculations

30cm³ of NaOH is neutralised by 12.3cm³ of 0.2mol/l HCl. What is the concentration of the NaOH.

• 82 mol/l

• 0.82 mol/l

• 0.49 mol/l

• 0.082 mol/l

What is the endpoint of a titration

• Where the amount of acid and alkali are balanced according to the equation

• Where the colour changes

• At the end

what is the reading on this burette?

• 4.4cm³

• 3.5cm³

• 3.6cm³

• 4.5cm³

A(n) ___________ is a procedure in which a solution of known concentration is used to determine the concentration of an unknown solution.

• experiment

• titration

• chemistry

• reaction

What is the concentration of the NaOH solution, if 20.0cm³ of it is neutralised by 25.00cm³ of 0.1 mol/dm³ H₂SO₄ solution?

• 0.75 mol/dm³

• 1.0 mol/dm³

• 1.25 mol/dm³

• 0.25 mol/dm³

Answer explanation

Each mole of H₂SO₄ reacts with 2 moles of NaOH

Tags

conc = moles / vol

reacting ratio

moles = conc x vol

acids as monoprotic/diprotic/triprotic

What is the concentration of the H₂SO₄ solution, if 40.0cm³ of it is neutralised by 20.00cm³ of 0.1 mol/dm³ NaOH solution?

• 0.025 mol/dm³

• 4.00 x 10^-5 mol/dm³

• 0.03 mol/dm³

• 25.00 mol/dm³

Tags

conc = moles / vol

reacting ratio

moles = conc x vol

acids as monoprotic/diprotic/triprotic

Write a balanced chemical equation for the reaction of the following acid and base:

___ H₂SO₄ + ___KOH -->

Evaluate responses using AI:

OFF

Tags

NGSS.HS-PS1-1

Write a balanced chemical equation for the reaction of the following acid and base:

___ Al(OH)₃ + ___HCl -->

Evaluate responses using AI:

OFF

I have 25mL of 1.0 mol/L HCl which neutralises 20mL of NaOH. What is the concentration of the NaOH?

• 0.8 mol/L

• 1 mol/L

• 1.25 mol/L

A 25.0 mL sample of HCl was titrated to the endpoint with 15.0 mL of 2.0 mol/L NaOH. What is the concentration of HCl?

• 1.6 mol/L

• 0.03 mol/L

• 0.6 mol/L

• 1.2 mol/L