A 0.1393-g sample of an unknown monoprotic acid was dissolved in 29.0 mL of water and titrated with 0.0627 M NaOH solution. The volume of base required to bring the solution to the equivalence point was 18.2 mL. (a) Calculate the molar mass of the acid. (b) After 10.4 mL of base had been added during the titration, the pH was determined to be 5.35. What is the Ka of the unknown acid

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.

the answer to this question is 3.