14.7 mL of a 0.384 M NaCl stock solution must be diluted to make
a 0.0925 M NaCl for use in a hospital. What volumn of the dilute
solution must be made? What volumn
of water needs to be added to the stock solution to make the
dilute solution?
50.0 mL of a 0.100 -M HoAc solution is titrated with a 0.100 -M
NaOH solution. Calculate the pH at each of the following
points.
Volume of NaOH added: 0, 5, 10, 25, 40 ,45 , 50 , 55 , 60 , 70 ,
80 , 90 , 100
A 77.0-mL sample of a 0.203 M lithium sulfate solution is mixed
with 55.0 mL of a 0.226 M lead(II) nitrate solution and this
precipitation reaction occurs:
Li2SO4(aq) +
Pb(NO3)2(aq) ⟶ 2
LiNO3(aq) + PbSO4(s)
The solid PbSO4 is collected, dried, and found to have a
mass of 4.71 g. Determine the percent yield. 1 mole
PbSO4 = 303.26 g
Group of answer choices
A.) 64.7 %
B.) 71.9 %
C. 98.5 %
D.) 80.0 %
25.0 mL of a 0.100 M HCN solution is titrated with
0.100 M KOH. Ka of HCN=6.2 x 10^-10.
a)What is the pH when 25mL of KOH is added (this is the equivalent
point).
b) what is the pH when 35 mL of KOH is added.
A 20.00 mL solution of 0.100 M HCOOH (formic) was titrated with
0.100 M KOH. The Ka for the weak acid formic is 1.40 x 10-5. a.
Determine the pH for the formic prior to its titration with KOH. b.
Determine the pH of this solution at the ½ neutralization point of
the titration. c. Identify the conjugate acid-base pair species at
the ½ neutralization point.
You are titrating 25.00 mL of a 0.100 M solution of a weak acid
with a 0.250 M solution of potassium hydroxide. Assume the pKa of
the weak acid is 5.6.
A. What is the pH after adding 3.0 mL of 0.250 M potassium
hydroxide?
B. What is the pH at the midpoint of the titration?
C. What is the pH at the equivalence point of the titration?
A 77.0 mL sample of 0.0400 M
HNO3 is titrated with 0.0800 M
CsOH solution. Calculate the pH after the following
volumes of base have been added.
(a) 10.0
mL
pH =
(b) 37.3
mL
pH =
(c) 38.5
mL
pH =
(d) 39.3
mL
pH =
(e) 65.1
mL
pH =
A 5.00 M stock solution of HCl is serially diluted three times,
starting with 10.00 mL and adding it to 90.00 mL of water each
time. What is the final concentration of HCl in mol/L, after the
third dilution?
a.You have 40.0 mL of a 0.100 M solution of HClO, with a
Ka of 3.0 x 10-8. b. What is the pH of the
solution after the addition of 30.0 mL of 0.200 M NaOH?
You are titrating 0.100 L of 0.100 M carbonic acid (shown below)
with 0.500 M NaOH.
What will the pH be when 23.0 mL of NaOH have been added? pkas:
6.05 and 10.64