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?
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
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.
![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?
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4. Calculate the pH of a 0.15 M solution of acetic acid, CH;COOH (K. = 1.8 x 109).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3f37f6ac-ba46-47be-9428-b46bb2c1ac09%2Fa7371695-b7b8-43b6-a042-7cdf0b2bffa2%2Fboelx9h_processed.jpeg&w=3840&q=75)
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