Save Question 9 (10 points) If the NaOH had been in the beaker and the acetic ac

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Save Question 9 (10 points) If the NaOH had been in the beaker and the acetic acid in the burette, how would that affect the titration? O The pH at the equivalence would be different The initial pH would be basic. O It would not change anything about the titration. O It would require a different indicator Save Question 10 (10 points) How is an indicator chosen for a titration? It is chosen based on your favorte color. O It is chosen based on how much acid is used. O It is chosen based on how much base is used. O It is chosen based on the expected equivalence point. Save Go to Submit Quiz Save All Responses

Explanation / Answer

9) NaOH is in the beaker while acetic acid is in the buret. Since NaOH is a strong base, the concentration of OH-, i.e, [OH-] is high and consequently, pOH = -log [OH-] is low. We know that pH + pOH = 14; therefore, pH = 14 – pOH and hence, pH will be high. A compound having pH of < 7 is said to be acidic while a compound having pH > 7 is basic. Hence, the initial pH is basic.

All the other statements are wrong. The pH at the equivalence point is determined by the concentration of sodium acetate formed and hence, shall remain the same. The equivalence point will be different, since the acid is now run into the base. The same acid-base indicator is used in the reaction.

10) An indicator signals the end point or equivalence point of an acid-base titration by changing its color. An acid-base indicator has distinctly different colors in acidic and basic media and the color of the indicator depends on the pH at the equivalence point. Hence, an acid-base indicator is chosen based on the expected equivalence point, more specifically on the expected pH at the equivalence point.

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