A 50.0 ml of acidic solute (K. = 1.20 x 10-2) is titrated with a 2.50 mL of x 10-5 M NaOH solution. 1.00 Which of the following indicators would be best ?for this titration Indicator methyl orange methyl red bromocresol purple bromthymol blue thymol blue phenolpthalein Methyl red Bromocresol purple O Bromthymol blue O Phenolpthalein Methyl orange

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A 50.0 mL of acidic solute (K.
= 1.20 x 10-2) is titrated with a
2.50 mL of
x 10-5 M NaOH solution. 1.00
Which of the following
indicators would be best
?for this titration
Indicator
methyl orange
methyl red
bromocresol purple
bromthymol blue
thymol blue
phenolpthalein
Methyl red
Bromocresol purple O
Bromthymol blue O
Phenolpthalein
Methyl orange
Transcribed Image Text:A 50.0 mL of acidic solute (K. = 1.20 x 10-2) is titrated with a 2.50 mL of x 10-5 M NaOH solution. 1.00 Which of the following indicators would be best ?for this titration Indicator methyl orange methyl red bromocresol purple bromthymol blue thymol blue phenolpthalein Methyl red Bromocresol purple O Bromthymol blue O Phenolpthalein Methyl orange
Expert Solution
Step 1

Given: Ka of acid solute = 1.20 X 10-2 

Volume of acid solution = 50.0 mL = 0.050 L                             (Since 1 L = 1000 mL)

Concentration of NaOH used = 1.00 X 10-5 M

And volume of NaOH solution used = 2.50 mL.

 

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