Base your answer to the question on the information below and on your knowledge of chemistry. A company produces a colorless vinegar that is 5.0% HC,H0z in water. One sample of vinegar has a pH value of 2.4. In water, the following occurs to produce hydromium ion. HC2H,O2 + H2O =H;O* + C¿H3O2° Using thymol blue as an indicator, a student titrates a 15.0-milliliter sample of the vinegar with 43.1 milliliters of a 0.30 M NAOH(aq) solution until the acid is neutralized. 3. State the pH value of a sample that has ten times fewer hydronium ions than an equal volume of a vinegar sample with a pH value of 2.4. 4. Determine the number of significant figures the concentration of the base used in this titration is expressed to.
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.
![Base your answer to the question on the information below and on your knowledge of chemistry.
A company produces a colorless vinegar that is 5.0% HC;H0; in water. One sample of vinegar has a pH value of
2.4. In water, the following occurs to produce hydromium ion.
HC2H;O2 + H2O = H;O* + C¿H;O2°
Using thymol blue as an indicator, a student titrates a 15.0-milliliter sample of the vinegar with 43.1 milliliters of a
0.30 M NaOH(aq) solution until the acid is neutralized.
3. State the pH value of a sample that has ten times fewer hydronium ions than an equal volume of a vinegar sample
with a pH value of 2.4.
4. Determine the number of significant figures the concentration of the base used in this titration is expressed to.
5. Explain, in terms of ions, why the colorless vinegar is classified as an Arrhenius acid.
6. State the Bronsted-Lowry base and its conjugate acid in the chemical reaction happening inside 5.0% vinegar.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe3e2759e-7875-4206-9c94-eb84e9608fb1%2F8980a690-78b8-4f17-b10e-71e57a72886a%2Fm89hfhd_processed.jpeg&w=3840&q=75)
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