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Using Concentrations Of Solutions In Mol/dm 3 (chemistry Only) (ht Only) (GCSE Chemistry)

The following is a GCSE Chemistry test covering 'Using Concentrations Of Solutions In Mol/dm 3 (chemistry Only) (ht Only)' from the broader topic Quantitative Chemistry. The test is geared towards the AQA exam board style syllabus.
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A pipette delivers 20.0 cm3 of acid into a flask. The acid concentration is 0.500 mol/dm3. How many moles of acid were delivered?
You dissolve 2.50 g of solid KCl (Mr = 74.6) in water and make the volume up to 500 cm3. What is the concentration in mol/dm3?
A 100 cm3 volumetric flask is filled to the mark with solution containing 0.0200 mol of solute. What is the concentration in mol/dm3?
In a reaction 25.0 cm3 of 0.200 mol/dm3 HCl reacts exactly with 15.0 cm3 of NaOH. What is the concentration of NaOH in mol/dm3? (HCl + NaOH ? NaCl + H2O)
A 250 cm3 solution contains 0.015 mol of NaOH. What is the concentration in mol/dm3?
In a titration, 25.0 cm3 of H2SO4 requires 30.0 cm3 of 0.100 mol/dm3 NaOH to reach the endpoint for H2SO4 + 2 NaOH ? Na2SO4 + 2 H2O. What is the concentration of H2SO4 in mol/dm3?
A solution labelled 0.100 mol/dm3 KOH is diluted by adding 100 cm3 of water to 100 cm3 of the solution. What is the new concentration?
You need 0.250 mol of solute for a reaction. You have 125 cm3 of 2.00 mol/dm3 stock solution. Do you have enough?
A sample contains 0.250 g of dissolved NaCl in 50.0 cm3. What is the concentration in g/dm3 and in mol/dm3? (Mr NaCl = 58.44)
What mass of NaOH (Mr = 40.0) is needed to prepare 250 cm3 of 0.200 mol/dm3 solution?
During a titration the concordant titres are 23.45, 23.55 and 23.50 cm3. Which value should be used for calculations and why?