Please help... Please solve thisproblem step by step I don't know where to start I never solvedthose kinds of problems. Thanks a lot I appreciate yourhelp...
Hydrogen peroxide (H2O2) behaves like anacid in water. It has a Ka value equal to 1.778x10-12. When sold in stores, solutions ofH2O2 are often 3.00%H2O2 by mass. The solutions also contain asmall amount of phosphoric acid (0.001% by mass) which stabilizesthe solution as hydrogen peroxide easily decomposes. Since bothhydrogen peroxide and phosphoric acid behave like acids in water,both acids will contribute H+ ions to the solution. TheKa for phosphoric acid is equal to 7.2 x10-3. Which acid contributes a larger concentration ofH3O+ ions into the solution if you assume1.00 L (HINT: assume the density of the solution is 1.000 g/ml).The two equations that you will need are given below:
H2O2 (aq) + H2O (l) H3O+1(aq) +HO2-1(aq)
H3PO4 (aq) + H2O(l) H3O+1(aq) + H2PO4-1(aq)
Please help... Please solve thisproblem step by step I don't know where to start I never solvedthose kinds of problems. Thanks a lot I appreciate yourhelp...
Hydrogen peroxide (H2O2) behaves like anacid in water. It has a Ka value equal to 1.778x10-12. When sold in stores, solutions ofH2O2 are often 3.00%H2O2 by mass. The solutions also contain asmall amount of phosphoric acid (0.001% by mass) which stabilizesthe solution as hydrogen peroxide easily decomposes. Since bothhydrogen peroxide and phosphoric acid behave like acids in water,both acids will contribute H+ ions to the solution. TheKa for phosphoric acid is equal to 7.2 x10-3. Which acid contributes a larger concentration ofH3O+ ions into the solution if you assume1.00 L (HINT: assume the density of the solution is 1.000 g/ml).The two equations that you will need are given below:
H2O2 (aq) + H2O (l) H3O+1(aq) +HO2-1(aq)
H3PO4 (aq) + H2O(l) H3O+1(aq) + H2PO4-1(aq)
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