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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 student titrates 25.0 cm3 of HCl with 0.100 mol/dm3 Ba(OH)2. The balanced equation is 2 HCl + Ba(OH)2 ? BaCl2 + 2 H2O. If the end point requires 23.50 cm3 Ba(OH)2, what is the concentration of HCl in mol/dm3?
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)
When preparing 1.00 dm3 of 0.100 mol/dm3 solution, a weighing error gives 0.105 mol of solute instead of 0.100 mol. What is the actual concentration (mol/dm3)?
A 0.200 mol/dm3 solution is prepared by dissolving solute in 500 cm3. How many moles were needed?
A graduated cylinder reads to ±0.10 cm3. You use it to measure 25.0 cm3 for a titration. Which uncertainty should you quote for that volume?
You prepare 500 cm3 of 0.0100 mol/dm3 AgNO3. How many moles of AgNO3 are needed?
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?
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 mass of 4.20 g of an acid (Mr = 60.0) is dissolved in water to give 250 cm3. What is the concentration in mol/dm3?
What mass of NaOH (Mr = 40.0) is needed to prepare 250 cm3 of 0.200 mol/dm3 solution?
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)