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

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 0.200 mol/dm3 solution is prepared by dissolving solute in 500 cm3. How many moles were needed?

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?

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

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 student finds the mean titre is 23.50 cm3 with a burette uncertainty of ±0.10 cm3 and a pipette uncertainty of ±0.02 cm3. Which is the best combined uncertainty to quote for the titre in cm3?

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?

You prepare 500 cm3 of 0.0100 mol/dm3 AgNO3. How many moles of AgNO3 are needed?

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