-If 35.00 mL of 0.0200 M aqueous HCl is required to titrate
30.00 mL of an aqueous solution of NaOH to the equivalence point,
the molarity of the NaOH solution is Blank 1 M.
-20.00 mL of 0.510 M NaOH is titrated with 0.740 M
H2SO4. Blank 1 mL of
H2SO4 are needed to reach the end point.
A 71.0 mL sample of 0.0400 M HIO4 is titrated with 0.0800 M RbOH
solution. Calculate the pH after the following volumes of base have
been added.
(a) 10.3 mL
pH =
(b) 34.4 mL
pH =
(c) 35.5 mL
pH =
(d) 36.2 mL
pH =
(e) 63.9 mL
pH =
A 83.0 mL sample of 0.0200 M HIO4 is titrated with 0.0400 M CsOH
solution. Calculate the pH after the following volumes of base have
been added. (
a) 11.6 mL
pH =
(b) 40.7 mL
pH =
(c) 41.5 mL
pH =
(d) 43.6 mL
pH =
(e) 75.5 mL
pH =
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 =
If 9.89 mL of 0.106 M sodium hydroxide is required to titrate
the acetylsalicylic acid in an aspirin tablet, how many milligrams
of acetylsalicylic acid are in the tablet? (MW acetylsalicylic acid
= 180.157 g/mol)
a. What volume of 0.085 M HCl is required to titrate 25.00 mL of
a 0.100 M NH3 solution to the equivalence point?
b. What is the pH at the equivalence point?
A 0.400 g sample of toothpaste was boiled with a 25 ml solution
TISAB buffer to extract the fluoride. After cooling, the solution
was diluted to exactly 100.0ml with more TISAB solution. The
potential of fluoride ion-selective electrode/reference electrode
in an aliquot of the sample was measured to be 186.6 mV. This value
corresponding to a log[F-] of -3.5016 on a working curve of mV
versus log [F-]. Calculate the weight percent F- and NaF in the
toothpaste sample.
100 mL of a river water sample took 9.30 mL of 0.01005 M Ag+ to
titrate. Calculate the concentration of Cl- in ppm (μg/mL or mg/L)
for the river water.
Part A: How many milliliters of 0.120 M NaOH are required to
titrate 50.0 mL of 0.0998 M butanoic acid to the equivalence point?
The Ka of butanoic acid is 1.5 x 10^-5.
Part B: What is the pH at the equivalence point?
Assume you mix (1.25x10^2) mL of 0.400 M HCl with the same
volume of 0.400 M NaOH in a coffee-cup calorimeter (as will be done
in the lab). The temperature of the solution before the mixing was
25.10 deg. C; after mixing and allowing the reaction to occur, the
temperature is 27.78 Deg. C. What is the enthalpy of neutralization
of the acid. Assume the densities of all the solutions are 1.00
g/mL and their specific heat capacities are 4.18...