Can you please further explain to me what I have to do to find the theoretical pH? I've prepared a 0.1 M Acetic acid by measuring out 5.0 mL, of 1.0 acetic aci and 45 mL of deionized water. Plus a additional of 1.00 mL of 1.0 M
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.
We know weak acids are not completely dissociated into ions so their pH is mainly determined by some calculations considering acid dissociation constant as summarised below:
To calculate the pH of a weak acid solution:
- Write the balanced dissociation equation.
- Set up an ICE table to track concentrations.
- Write the equilibrium expression (Ka).
- Plug in equilibrium concentrations.
- solve for x.
- Calculate [H+] at equilibrium.
- Find pH with the formula: pH = -log([H+]).
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