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D. Miller Solutions to Review Problems for Acid/Base Chemistry 7. If 0.050 mL of 6.0 M NaOH is added to 400 mL of 10-5 M HCl, what is the
The added NaOH reacts with the HCl.
mol NaOH added = (6.0 mol/L)(0.000050 L) = 0.00030 mol
init mol H3O+ = (10-5 mol/L)(0.400 L) = 0.000004 mol init mol
mol after rxn OH- + H3O+ 6 2H2O
0 The HCl is completely neutralized and you are left with a solution of a strong
[OH-] = 0.000296 mol/0.40005 L = 7.4 x 10-4 M
pOH = 3.13 Y pH = 10.87 (Notice that the pH of this unbuffered solution increased by almost 6 pH units
with this small addition of base . Adding 100 times this volume of base to a
buffer (Prob. 4) changed the buffer pH by only 0.35 unit.) Chem 102
D. Miller Solutions to Review Problems for Acid/Base Chemistry 8. Characterize the solution formed (strong acid, strong, base, weak acid, weak
base, buffer or neutral) when equal volumes of the following are mixed. Explain.
0.5 M NaOH + 0.5 M HC2H3O2
The following reaction...
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This document was uploaded on 03/06/2014 for the course CHEM 102 at CSU Northridge.
- Fall '10