50.0 ml of 0.200 M AgNO3 is mixed with 50.0 ml of
0.050 M NaCl. Calculate...
50.0 ml of 0.200 M AgNO3 is mixed with 50.0 ml of
0.050 M NaCl. Calculate the concentration of Ag + and Cl- in the
resulting solution, assuming the volumes are additive.
75.0 mL of 0.200 M AgNO3 is combined with 125.0 mL of 0.100 M
Nacl. solid AgCl forms.
a) what mass of AgCl forms ?
b) what is the concentration of each of the 4 ions in the final
solution ? assume that volumes are additive. note.... none of the
concentration will be zero.'
-Ag , Na , NO3 and Cl
Calculate the pH for each case in the titration of 50.0 mL of
0.200 M HClO(aq)0.200 M HClO(aq) with 0.200 M KOH(aq).0.200 M
KOH(aq). Use the ionization constant for HClO.
What is the pH before addition of any KOH?
pH=
What is the pH after addition of 25.0 mL KOH?
pH=
What is the pH after addition of 35.0 mL KOH?
pH=
What is the pH after addition of 50.0 mL KOH?
pH=
What is the pH after addition of...
Calculate the pH for each case in the titration of 50.0 mL of
0.200 M HClO(aq)0.200 M HClO(aq) with 0.200 M KOH(aq).0.200 M
KOH(aq). Use the ionization constant for HClO.HClO.
What is the pH before addition of any KOH?KOH?
pH=pH=
What is the pH after addition of 25.0 mL KOH?25.0 mL KOH?
pH=pH=
What is the pH after addition of 35.0 mL KOH?35.0 mL KOH?
pH=pH=
What is the pH after addition of 50.0 mL KOH?50.0 mL KOH?
pH=pH=
What...
50 mL of 0.060 M K2CrO4 is mixed with 50
mL of 0.080 M AgNO3. Calculate the following:
a. The solubility of Ag2CrO4
(Ksp = 1.9 X 10-12) in the solution in moles
per liter.
b. The concentrations of the following ions Ag+,
CrO4-2, K+, and
NO3-.
50 mL of 0.060 M K2CrO4 is mixed with 50
mL of 0.080 M AgNO3. Calculate the following:
a. The solubility of Ag2CrO4
(Ksp = 1.9 X 10-12) in the solution in moles
per liter.
b. The concentrations of the following ions Ag+,
CrO4-2, K+, and
NO3-.
25.0 mL of 0.200 M solution of HBr are mixed with 25.0 mL of
0.200 M solution of NaOH in a constant pressure calorimeter. The
temperature increases from 23.00 °C to 24.37 °C. Assume that the
specific heat of the solution is the same as that of pure water
(4.18 J/(g•°C)) and that the density is the same as pure water
(1.00 g/mL). Calculate ΔH per mole of reaction for the below
chemical reaction.
HBr (aq) + NaOH (aq) →...
A 50.0 mL sample of 0.0645 M AgNO3(aq) is added to 50.0 mL of
0.100 M NaIO3(aq). Calculate the [Ag+] at equilibrium in the
resulting solution. The Ksp value for AgIO3(s) is 3.17 × 10-8.
[Ag+] =____ mol/L
Part A
A 50.0-mL sample of 0.200 M sodium hydroxide is
titrated with 0.200 M nitric acid.
Calculate the pH of the solution, after you add a total of 51.9
mL 0.200 M HNO3.
Express your answer using two decimal places.
Part B
A 39.0
mL
sample of 0.146
M
HNO2
is titrated with 0.300
M
KOH.
(Ka
for
HNO2
is 4.57×10−4.)
Determine the pH at the
equivalence point for the titration of
HNO2
and
KOH
.
Consider the titration of 50.0 mL of 0.100 M HN3 (Ka=1.9X10^-5)
with 0.200 M CSOH. Calculate the PH after addition of
A) at initial point
B) 12.50 ml CSOH
C) 50.0 ml CSOH
D) 60.0 mL of CSOH
If 85.00 mL of 0.100 M HCl is mixed with 25.00 mL of 0.200 M
H2SO4 and 50.00 mL of 0.400 M NaOH. What is the resulting pH of the
final solution?
Please show all work and how the formulas are derived if
modified.