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Part I
1. H2CO3, weak acid
2. Potassium hydroxide, strong base
3. NH3
, weak base
4. S1O3, non
5. Sulfuric acid, strong acid
6a. pH = 0.00
6b. [OH1-] = 9.82E-3 M, pOH = 2.008
6c. pOH = 13.793
7a. 2 K1(OH)1 (aq) + 1 H2SO4 (aq) --> 2 H2O1 (l) + 1 K2SO4 (aq)
7b. [K1(OH)1] = 2.70M
8. Equivalence point of the solution = Endpoint of the pH indicator
9a. HNO2
9b. CH3NH31+
10a. Weak acid and the salt of its conjugate base
10b. The pH of the solution does not change significantly with the addition of an strong acid or a strong base. It has a specie that will react with the H1+ so that OH1- do not have to be used in this neutralization. Also in the solution is a specie that will do a similar action if an OH1- is added to the solution. Remember, pH (and also pOH) scale only keep track of [H1+] concentration not acid molecule concentration.