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Titrations (chemistry Only) (GCSE Chemistry)

The following is a GCSE Chemistry test covering 'Titrations (chemistry Only)' from the broader topic Chemical Changes. The test is geared towards the AQA exam board style syllabus.
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Below a typical questions that will be covered in this test. You final score will be logged on your account

You titrate 50.0 cm3 of 0.120 mol/dm3 H2SO4 with 0.100 mol/dm3 NaOH. What volume of NaOH is needed? (Equation: H2SO4 + 2 NaOH ? Na2SO4 + 2 H2O)
To reduce random error in titration timings and mixing, the best practice is to:
Which procedure increases accuracy when preparing a standard solution by weighing a solid?
Which indicator would be most suitable for a titration of a strong acid with a strong base?
A titration of 25.0 cm3 of an acid required 30.0 cm3 of 0.100 mol/dm3 NaOH. How many moles of acid were present if the reaction is HA + NaOH ? NaA + H2O?
You titrate 20.0 cm3 of 0.250 mol/dm3 sodium carbonate (Na2CO3) with 0.100 mol/dm3 hydrochloric acid. Which balanced equation is needed to calculate the concentration of HCl?
A back titration is most useful when:
In a titration calculation you find the moles of titrant used and want moles of analyte. Which information must you use next?
A student titrates 25.00 cm3 of hydrochloric acid with 0.100 mol/dm3 sodium hydroxide and uses 20.00 cm3 of the base to reach the end-point. What is the concentration of the hydrochloric acid in mol/dm3?
Which calculation step is correct to find concentration (mol/dm3) of an acid when moles of acid and volume in cm3 are known?
A titration uses 0.0250 mol of acid which reacts 1:1 with the base. If the titre of base used was 25.00 cm3, what was the concentration of the base in mol/dm3?