Reference no: EM13161643

Hydrogen peroxide (H2O2) behaves like an acid in water. It has a Ka value equal to 1.778x 10-12. When sold in stores, solutions of H2O2 are often 3.00% H2O2 by mass. The solution also contains a small amount of phosphoric acid (0.001% by mass) which stabilizes the solution as hydrogen peroxide easily decomposes. Since both hydrogen peroxide and phosphoric acid behave like acids in water, both acids will contribute H+ ions to the solution. The Ka for phosphoric acid is equal to 7.2 x 10-3. (HINT: assume the density of the solution is 1.000 g/ml). The two reactions that you will need are given below: (8 pts) a.) Determine the concentration (M) of H2O2 and H3PO4 from their provided mass percents. Assume 1.00 L of solution (Hint, review how a mass % is determined - it will help you identify the units and their respective locations before you convert). H2O2 (aq) + H2O (l) ? H3O+1 (aq) + HO2-1 (aq) H3PO4 (aq) + H2O (l) ? H3O+1(aq) + H2PO4-1 (aq) b.) Mathematically determine which acid contributes a larger concentration of H3O+ ions into the solution, be sure to report the H3O+ concentrations for both, label them clearly, and identify which substance creates a larger concentration?