A solution of acetic acid is 2.0% dissociated at 25.0°C. What was the original concentration (in M) of the acetic acid solution? The Ka at 25.0 °C for acetic acid is 1.8 × 10^-5.
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.
- A solution of acetic acid is 2.0% dissociated at 25.0°C. What was the original concentration (in M) of the acetic acid solution? The Ka at 25.0 °C for acetic acid is 1.8 × 10^-5.
- A solution of ammonia is 3.2% ionized at 25.0°C. What was the original concentration (in M) of the ammonia solution? The Kb at 25.0°C for ammonia is 1.8×10^-5.
- Calculate the pOH of 0.716 M anilinium hydrochloride (C6H5NH3Cl) solution in water, given that Kb for aniline is 3.83 × 10^-4.
- The acid-dissociation constant of hydrocyanic acid (HCN) at 25.0°C is 4.9 × 10^-10. What is the pH of an aqueous solution of 0.080 M sodium cyanide (NaCN)?
- The base-dissociation constant of ethylamine (C2H5NH2) is 6.4 × 10^-4 at 25.0 °C. The [H+] in a 1.6 × 10^-2 M solution of ethylamine is __________ M.
- The acid-dissociation constants of phosphoric acid (H2PO3) are Kal = 7.5 × 10^-3, Ka2 = 6.2 × 10^-8, and Ka3 = 4.2 × 10^-13 at 25.0°C. What is the pH of a 2.5 M aqueous solution of phosphoric acid?
- What is the pH of a sodium formate solution prepared by adding 0.680 grams of sodium formate to 100.0 ml of water at 25.0°C? The Ka at 25.0°C for formic acid is 1.8 × 10^-4.
- Calculate the pH of a buffer that contains 0.270 M hydrofluoric acid (HF) and 0.180 M cesium fluoride (CsF). The Ka of hydrofluoric acid is 6.80 × 10^-4.
- The Kb of ammonia is 1.76 × 10^-5. The pH of a buffer prepared by combining 45.0 mL of 0.180 M ammonia and 40.0 mL of 0.205 M ammonium nitrate is __________.
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
