Part 1.)
Consider the titration of 50.0 mL of 0.0500 M
C2H5NH2 (a weak base;
Kb = 0.000640) with 0.100 M HBrO4. Calculate
the pH after the following volumes of titrant have been
added:
(a) 0.0 mL pH = |
(b) 6.3 mL pH = |
(c) 12.5 mL pH = |
(d) 18.8 mL pH = |
(e) 25.0 mL pH = |
(f) 42.5 mL pH = |
Part 2.)
A solution of Na3PO4 is added dropwise to a solution that is 0.0613 M in Ag+ and 0.00490 M in Cu2+.
The Ksp of Ag3PO4 is
8.89e-17.
The Ksp of Cu3(PO4)2 is
1.4e-37.
(a) What concentration of PO43- is necessary
to begin precipitation? (Neglect volume changes.)
___ [PO43-] = M.
(b) Which cation precipitates first?
___ Ag+Cu2+
(c) What is the concentration of PO43- when
the second cation begins to precipitate?
___ [PO43-] = M.
Part 1.) Consider the titration of 50.0 mL of 0.0500 M C2H5NH2 (a weak base; Kb = 0.000640) with 0.100 M HBrO4. Calculat...
A solution of Na3PO4 is added dropwise to a solution that is 0.0810 M in Ag+ and 0.00171 M in Cu2+. The Ksp of Ag3PO4 is 8.89e-17. The Ksp of Cu3(PO4)2 is 1.4e-37. (a) What concentration of PO43- is necessary to begin precipitation? (Neglect volume changes.) [PO43-] = M. (b) Which cation precipitates first? Ag+ Cu2+ (c) What is the concentration of PO43- when the second cation begins to precipitate? [PO43-] = M.
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Consider the titration of 40.0 mL of 0.0600 M CH3NH2 (a weak base; Kb = 0.000440) with 0.100 M HBrO4. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mL (b) 6.0 mL pH = (C) 12.0 mL pH = pH = 11.8 * x (d) 18.0 ml (e) 24.0 ml (f) 43.2 ml pH = pH = pH =
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