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

A solution labelled 0.250 mol/dm3 is found experimentally to have 0.243 mol/dm3. What is the percentage error?

You have 0.120 mol of solute in 300 cm3. If you add water until the concentration is 0.0600 mol/dm3, what volume in cm3 will the solution be?

A student dilutes 10.0 cm3 of 1.00 mol/dm3 HCl to a total volume of 250 cm3. 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?

You titrate 25.00 cm3 of unknown acid and use 15.00 cm3 of 0.100 mol/dm3 NaOH. If the acid is monoprotic, what is its concentration?

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?

In an experiment you need 0.0200 mol of Na2CO3. How many cm3 of 0.100 mol/dm3 solution do you use?

During a titration the concordant titres are 23.45, 23.55 and 23.50 cm3. Which value should be used for calculations and why?

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)

You have 0.250 dm3 of 0.120 mol/dm3 CaCl2. How many grams of CaCl2 (Mr = 110.98) are present?