A 28.1 mL sample of 0.264 M ethylamine, C₂H5NH₂, is titrated with 0.230 M hydrobromic acid. (1) Before the addition of any hydrobromic acid, the pH is (2) After adding 14.2 mL of hydrobromic acid, the pH is (3) At the titration midpoint, the pH is (4) At the equivalence point, the pH is (5) After adding 51.6 mL of hydrobromic acid, the pH is Use the Tables link on the toolbar for any equilibrium constants that are required.

You are given the following acidbase titration data, where each point on the graph represents the pH after adding a given volume of titrant (the substance being added during the titration). a What substance is being titrated, a strong acid, strong base, weak acid, or weak base? b What is the pH at the equivalence point of the tiration? c What indicator might you use to perform this titration? Explain.

The three flasks shown below depict the titration of an aqueous NaOH solution with HCl at different points. One represents the titration prior to the equivalence point, another represents the titration at the equivalence point, and the other represents the titration past the equivalence point. (Sodium ions and solvent water molecules have been omitted for clarity.) a Write the balanced chemical equation for the titration. b Label each of the beakers shown to indicate which point in the titration they represent. c For each solution, indicate whether you expect it to be acidic, basic, or neutral.

Determine the pH during the titration of 18.9 mL of 0.253 M hydrobromic acid by 0.205 M potassium hydroxide at the following points: (1) Before the addition of any potassium hydroxide (2) After the addition of 11.7 mL of potassium hydroxide (3) At the equivalence point (4) After adding 28.7 mL of potassium hydroxide