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NSWChemistryQuick questions
Module 5: Equilibrium and Acid Reactions
Quick questions on Acid-base titrations and indicators explained: HSC Chemistry Module 5
7short Q&A pairs drawn directly from our worked dot-point answer. For full context and worked exam questions, read the parent dot-point page.
What are titration basics?Show answer
A titration is a volumetric analysis in which a solution of known concentration (the titrant, usually in the burette) is added gradually to a solution of unknown concentration (the analyte, usually in a conical flask) until the reaction is complete.
What are comparing titration curves?Show answer
The shape of a titration curve depends on the strengths of the acid and base involved. The table below traces pH against the fraction of titrant added (acid being titrated with base), making the differences explicit.
What is indicator selection rule?Show answer
Choose an indicator whose colour change range straddles the equivalence pH. If the equivalence pH is 8.7 (weak acid / strong base), phenolphthalein (8.3-10.0) brackets it; methyl orange (3.1-4.4) would change far too early.
What is weak acid / weak base?Show answer
No sharp transition. No indicator gives a reliable end point. Not used quantitatively in HSC.
What is q1?Show answer
Define the equivalence point and the end point of a titration, and state the criterion for choosing an indicator that makes them coincide. [3 marks]
What is q2?Show answer
A 25.0 mL sample of is titrated to equivalence with 32.50 mL of 0.150 mol L NaOH. Calculate the concentration of the sulfuric acid. [3 marks]
What is q3?Show answer
A weak acid HA of unknown concentration is titrated with 0.100 mol L NaOH. The pH at the half-equivalence point is 4.74 and the equivalence point pH is 8.72. (a) State the of HA.
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