An analytical chemist is titrating 168.8mL of a 1.100M solution of cyanic acid HCNO with a 0.7700M solution of KOH. The pKa of cyanic acid is 3.46. Calculate the pH of the acid solution after the chemist has added 282.6mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places.

Question
Asked Oct 26, 2019

An analytical chemist is titrating 168.8mL of a 1.100M solution of cyanic acid HCNO with a 0.7700M solution of KOH. The pKa of cyanic acid is 3.46. Calculate the pH of the acid solution after the chemist has added 282.6mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places.

 

check_circleExpert Solution
Step 1

Number of moles of HCNO is:

1.100шо
х.
L
-168.8mLx
-0.1856mol
L
1000mL
0.770 шоl
-х.
-0.217602 mol
L
Number of OH
added= 282.6mLx.
1000mL
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Image Transcriptionclose

1.100шо х. L -168.8mLx -0.1856mol L 1000mL 0.770 шоl -х. -0.217602 mol L Number of OH added= 282.6mLx. 1000mL

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Step 2

Then,

...
>CNO HH20
HCNOЮH -
Imol)
Cmo .18560-0.18560 t0.185660
0.1856 0.2176
Е(mо)
0
0.032
0.18560
help_outline

Image Transcriptionclose

>CNO HH20 HCNOЮH - Imol) Cmo .18560-0.18560 t0.185660 0.1856 0.2176 Е(mо) 0 0.032 0.18560

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