ChemistryWiki | Answer To 2015-2016 Review HW For Acid | RecentChanges | Preferences
Part I
1. S2-, sulfide, Hydrosulfuric acid, Weak acid (also weak electrolyte)
2. Selenide, Se2-, H2Se, weak acid (weak electrolyte)
3. SO42-, sulfate, Sulfuric acid, strong acid (strong electrolyte)
4. sulfite, SO32-, H2SO3 weak acid (weak electrolyte)
5. Ca2+, OH1-, Calcium hydroxide, Strong base (strong electrolyte)
6. Phosphate, PO43-, H3PO4, weak acid (weak electrolyte)
7. NH3, Strong base (strong electrolyte)
8. Carbon dioxide, non-electrolyte
9. Ba2+, ClO2, Barium chlorite, strong electrolyte (it is a salt)
10. NO21-, nitrite, Nitrous acid, weak acid (weak electrolyte)
Part II
1. HF is the only weak acid (so it does not ionize 100%) and since all acids have the same mole of acid compound per volume, it will have least amount of H+. Sulfuric acid will have the highest Molarity of H+ since it produces two mole of H+ per mole of acid molecule. HCl only produces 1 mole of H+ per mole of acid compound.
2. It indicates pH and does it by changing from one color to another. The specific pH that it changes color is called the pH indicator.
3. To know when to stop adding in the strong acid or base (called titrating) to the reaction bucket. If you properly choose the pH indicator (so the Endpoint of the pH indictor = Equilvance point of the solution), the solution will be at the Equilvance point of the solution and that allows you to do Stoichiometry calculations.
4. pH = -log [H=], H+ and pH are inversely proportional to each other, it is the "-" sign in the equation since the log (and 10x) are power term so the "-" sign changes the power to a negative (small number).
Part III
1. pH = 1.988
2. [Ca(OH)2] = 3.62E-4 M
3. pH = 10.72
4. 2.74L of NaOH solution