Question

1.)What is the pH of a buffer system prepared by dissolving
10.70 grams of NH_{4}Cl and 25mL of 12 M NH_{3} in
enough water to make 1.00L of solution?
K_{b}=1.80x10^{-5} for NH_{3}. Calculate
the change in pH after addition of 50.0mL of 0.15M NaOH.

2.)What mass of Na_{2}SO_{4} (molar mass=142.0
g/mol) must be added to 350mL of 0.16M Ag^{+} to initiate
precipitation of Ag_{2}SO_{4}? The K_{sp}
of Ag_{2}SO_{4} is 1.2x10^{-5}. Assume no
volume change occurs upon addition of
Na_{2}SO_{4}.

3.)What is the pH of a sturated solution of Fe(OH)_{2}?
K_{sp}=4.87x10^{-17}.

Answer #1

what is the pH of a buffer system prepared by dissolving 10.70
grams of NH4Cl and 25.00 mL of 12 M NH3 in enough water to make
1.000 L of solution? Kb=1.80 x 10^-5 for NH3. calculate the change
in pH after addition of 50.0 mL of 0.15M NaOH.

What is the pH of a buffer system prepared by dissolving 10.70
grams of NH4Cl and 25.00 mL of 12M NH3 in enough water to make
1.000 L of solution? Kb= 1.80 x 10^-5 for NH3. Calculate the change
in pH after addition of 50.00 mL of 0.15 NaOH.

1.) A buffer solution contains 0.455 M
NH4Cl and
0.295 M NH3
(ammonia). Determine the pH
change when 0.085 mol
NaOH is added to 1.00 L of the
buffer.
pH after addition − pH before addition = pH change
=
2.)
Determine the pH change when
0.044 mol HNO3 is
added to 1.00 L of a buffer solution that is
0.462 M in HF and
0.218 M in F-.
pH after addition − pH before addition = pH change
=

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