cetic acid (HC2H3O2) is an important component of vinegar. A 10.00-mL sample of vinegar is titrated with 0.5052 M NaOH, and 16.88 mL are required to neutralize the acetic acid that is present. Write a balanced equation for this neutralization reaction. What is the molarity of the acetic acid in this vinegar

The molarity of the acetic acid in this vinegar is 0.853 M

Explanation:

Step 1: Data given

Volume of vinegar sample = 10.00 mL

Concentration of NaOH = 0.5052 M

16.88 mL are required to neutralize the acetic acid

Step 2: The reaction

HC2H3O2(aq) + NaOH(aq) ⇔ NaC2H3O2(aq) + H2O(l)

Step 3: Calculate molarity of cetic acid (HC2H3O2)

C1*V1 = C2*V2

⇒with C1 = the molarity ofHC2H3O2= TO BE DETERMINED

⇒with V1 = the volume of HC2H3O2 = 10.00 mL = 0.01 L

⇒with C2 = the molarity of NaOH = 0.5052 M

⇒with V2 = the volume of NaOH = 16.88 mL = 0.01688L

C1 = (C2*V2)V1

C1 = (0.5052 * 0.01688 ) / 0.01

C1 = 0.853 M

The molarity of the acetic acid in this vinegar is 0.853 M

212121212121212122121212121121212122121212121212121212121n i think

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.