2. Two 10.0 mL samples of the same acid were titrated with a 0.11 M solution of

Question

2. Two 10.0 mL samples of the same acid were titrated with a 0.11 M solution of KOH. The titration curves for these two samples appear below. Select all of the following statements that are true about these titrations. Sample 1 Sample 2 800 200 200 0.02 Volume of titrant added Volume of titrant addecd Both solutions are weak acids. Sample 2 is more concentrated than sample 1. Sample 1 is more concentrated than sample 2. Sample 1 requires more moles of OH ions in order to reach the equivalence point. The two solutions start with a different number of moles of H30+ ions present Both solutions are strong acids. Sample 1 is a weak acid and Sample 2 is a strong acid.

Explanation / Answer

intial PH of both sample is very low (for sample 1 PH = 0.5 and for sample 2 PH = 1), it means both are strong acids.

now intial PH of both sample is different it means two solution start with a different number of moles of H3O+.

solution having large number of H+ ions (i.e. low value of PH) will have more concentration it means sample 1 is more concentrated than sample 2 (because sample 1 is having less PH)

also solution with large concentration, will require more no. of OH- ions in order to reach equivalence point so sample 1 requires more moles of OH- in order to reach the equivalence point.

so correct options are

option (3) Sample 1 is more concentrated than sample 2.

option (4) Sampple 1 requires more moles of OH- in order to reach the equivalence point.

option(5) The two solutions start with a different number of moles of H3O+ ions present.

option (6) Both solutions are strong acids.

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