17.46 Consider the titration of 30.0 mL of 0.050 M NH3 with 0.025 M HCI. Calculate the pH after the following volumes of titrant have been added: (a) 0 mL, (b) 20.0 mL, (c) 59.0 mL, (d) 60.0 mL, (e) 61.0 mL, (f) 65.0 mL.
17.46 Consider the titration of 30.0 mL of 0.050 M NH3 with 0.025 M HCI. Calculate the pH after the following volumes of titrant have been added: (a) 0 mL, (b) 20.0 mL, (c) 59.0 mL, (d) 60.0 mL, (e) 61.0 mL, (f) 65.0 mL.
17.46 Consider the titration of 30.0 mL of 0.050 M NH3 with 0.025 M HCI. Calculate the pH after the following volumes of titrant have been added: (a) 0 mL, (b) 20.0 mL, (c) 59.0 mL, (d) 60.0 mL, (e) 61.0 mL, (f) 65.0 mL.
Transcribed Image Text:DAExercises
761
strong acid
g of the ti-
ng acid. (c)
which acid
17.43 A 20.0-mL sample of 0.200 M HBr solution is titrated with
tsl0.200 M NaOH solution. Calculate the pH of the solu-
tion after the following volumes of base have been added:
(a) 15.0 mL, (b) 19.9 mL, (c) 20.0 mL, (d) 20.1 mL, (e) 35.0 mL.
17.44 A 20.0-mL sample of 0.150 M KOH is titrated with 0.125 M
ere are both
HCIO4 solution. Calculate the pH after the following vol-
umes of acid have been added: (a) 20.0 mL, (b) 23.0 mL,
(c) 24.0 mL, (d) 25.0 mL, (e) 30.0 mL.
17.45 A 35.0-mL sample of 0.150 M acetic acid (CH3COOH) is ti-
trated with 0.150 M NaOH solution. Calculate the pH after
the following volumes of base have been added: (a) 0 mL,
(b) 17.5 mL, (c) 34.5 mL, (d) 35.0 mL, (e) 35.5 mL, (f) 50.0 mL.
17.46 Consider the titration of 30.0 mL of 0.050 M NH3 with
0.025 M HCI. Calculate the pH after the following volumes
of titrant have been added: (a) 0 mL, (b) 20.0 mL, (c) 59.0
mL, (d) 60.0 mL, (e) 61.0 mL, (f) 65.0 mL.
bile
17.47 Calculate the pH at the equivalence point for titrating
H;COOH(aq)
0.200 M solutions of each of the following bases with 0.200
M HBr: (a) sodium hydroxide (NaOH), (b) hydroxylamine
A (NH2OH), (c) aniline (C,H5NH2).
atements con-
17.48 Calculate the pH at the equivalence point in titrating 0.100
ed to reach the
103.
M solutions of each of the following with 0.080 M NaOH:
(a) hydrobromic acid (HBr), (b) chlorous acid (HCIO2),
(c) benzoic acid (C,HsCOOH).
HNO, titration
alence point in
Solubility Equilibria and Factors Affecting
Solubility (Sections 17.4 and 17.5)
ndicator for both
17.49 For each statement, indicate whether it is true or false.
(a) The solubility of a slightly soluble salt can be expressed
in units of moles per liter.
statements con-
rue or false.
(b) The solubility product of a slightly soluble salt is simply
the square of the solubility.
(c) The solubility of a slightly soluble salt is independent of
the presence of a common ion.
(d) The solubility product of a slightly soluble salt is inde-
pendent of the presence of a common ion.
titrations will be
entially the same
dicator for both
and MZ2, is the same, 4 x 10 mol/L. (a) Which has the
larger numerical value for the solubility product constant?
(b) In a saturated solution of each salt in water, which has
the higher concentration of M²*? (c) If you added an equal
volume of a solution saturated in MA to one saturated in
MZ2, what would be the equilibrium concentration of the
cation, M2+?
17.50 The solubility of two slightly soluble salts of M²*, MA
ach of the following
HCO3 titrated with
I titrated with HBr.
of each of the fol-
H 7: (a) formic acid
oxide titrated with
th nitric acid.
17.51 Write the expression for the solubility-product con-
stant for each of the following ionic compounds: Agl,
thymol blue has two
l generally be more
hase?
True or false: "solubility" and "solubility-product con-
na number for a given compound. (b) Write
WNI product constant for each
UntOH), and
SrSO4, Fe(OH)2, and Hg,Br2.
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