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3.4 Using concentrations of solutions in mol/dm3

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Question 3
H

In a titration, 25.0 cm3 of sodium hydroxide solution needed 20.0 cm3 of 0.150 mol/dm3 hydrochloric acid for complete neutralisation. The equation is NaOH+HCl→NaCl+H2O\text{NaOH} + \text{HCl} \rightarrow \text{NaCl} + \text{H}_2\text{O}NaOH+HCl→NaCl+H2​O. What is the concentration of the sodium hydroxide solution?

[1]
A

0.120 mol/dm30.120\ \text{mol/dm}^30.120 mol/dm3

B

0.150 mol/dm30.150\ \text{mol/dm}^30.150 mol/dm3

C

0.188 mol/dm30.188\ \text{mol/dm}^30.188 mol/dm3

D

0.240 mol/dm30.240\ \text{mol/dm}^30.240 mol/dm3

Markscheme

3.4 Using concentrations of solutions in mol/dm3 Questions

  1. GCSE
  2. /Chemistry
  3. /3.4 Using concentrations of solutions in mol/dm3

40 exam-style questions on AQA GCSE Chemistry 3.4 Using concentrations of solutions in mol/dm3, covering 3.4.1 Concentration in mol/dm3. Each one has a worked solution and a mark scheme showing where the marks go.

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