3. Suppose 10-6 mol HCIO4 (perchloric acid, a very strong acid) is dissolved in 1000 L of water. This gives (H°] =(10-6 mol)/(1000 L) = 10-9 M. Finally, the pH is calculated: pH = -logro[H*]= -log-o{10 °) = 9.0, which correspondsto an alkaline solution! What is wrong?%3D%3D!!!3!4. Calculate the pH of a 0.15 M solution of acetic acid, CH;COOH (K. = 1.8 x 109).

We have to find pH of given solution

Süppose 10 mol HCIO4 (perchloric acid, a very strong acid) is dissolved in 1000 L of water. This gives (H*) = (10-6 mol)/(1000 L) = 10-9 M. Finally, the pH is calculated: pH = -log 10[H*] = -log10( 10 °) = 9.0, which corresponds to an alkaline solution! What is wrong?

Süppose 10 mol HCIO4 (perchloric acid, a very strong acid) is dissolved in 1000 L of water. This gives (H) = (10-6 mol)/(1000 L) = 10-9 M. Finally, the pH is calculated: pH = -log 10[H] = -log10( 10 °) = 9.0, which corresponds to an alkaline solution! What is wrong?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 25QAP: Find [OH-] and the pH of the following solutions. (a) 0.25 g of Ba(OH)2 dissolved in enough water to...

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Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

3. Suppose 10-6 mol HCIO4 (perchloric acid, a very strong acid) is dissolved in 1000 L of water. This gives (H°] =
(10-6 mol)/(1000 L) = 10-9 M. Finally, the pH is calculated: pH = -logro[H*]= -log-o{10 °) = 9.0, which corresponds
to an alkaline solution! What is wrong?
%3D
%3D
!!
!3!
4. Calculate the pH of a 0.15 M solution of acetic acid, CH;COOH (K. = 1.8 x 109).

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