Acid-base indicators need to have very intense colors so that a very low concent

Question

Acid-base indicators need to have very intense colors so that a very low concentration is visible. Calculate there be a problem in using too much indicator? a. No, the colors would just be darker. b. No, indicators are inert. c. Yes, more indicator requires more extreme pH values to change color. d. Yes, the indicator could affect the acid-base chemistry being measured. e. No, the colors would just be sharper. The most suitable acid-base indicator for a titration of acetic acid with NaOH has _____ a. a pK_in = pK_a of the acid. b. a pK_in = pK_b of the base. c. pK_in = pH of a sodium acetate solution. d. pK_in = pH of an acetic acid solution. c. pK_in = 7.0.

Explanation / Answer

(8) (d)

the indicator may affect the acid base chemistry being measured if too much indicator is added.

(9)

(c) pKin = pH of sodium acetate solution

An appropriate indicator for and acid base titration will change colour at the same pH as the equivalence point of the acid base reaction. That is the end point of the reaction as indicated by the indicator must be the same as the equivalence point of the acid - base reaction.

At an equivalence point sodium acetate, the salt of weak acid and strong base is formed so, the resulting solution will have pH > 7.00, so, the indicators that change their colors at more than pH 7 are suitable.

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