A25.0 mL sample of 0.100 M NaOH is titrated with a 0.100 M HNO3
solution. Calculate the pH after the addition of 0.0, 4.0, 8.0,
12.5, 20.0, 24.0, 24.5, 24.9, 25.0, 25.1, 26.0, 28.0, and 30.0 of
the HNO3.
50.0 ml of an acetic acid (CH3COOH) of unknown
concentration is titrated with 0.100 M NaOH. After 10.0 mL of the
base solution has been added, the pH in the titration flask is
5.30. What was the concentration of the original acetic acid
solution? (Ka(CH3COOH) = 1.8 x
10-5)
What is the pH of a solution obtained by adding 50.0 mL of 0.100
M NaOH (aq) to 60.0 mL of 0.100 M HCl (aq)?
Select one:
a. 11.96
b. 2.04
c. 3.11
d. 7.00
QUESTION 2
What is the pH of a solution prepared by dissolving 5.86 grams
of propanoic acid, CH3CH2COOH (l),
and 1.37 grams of NaOH (s) in enough water to make exactly
250.0 mL of solution. pKa = 4.87 for propanoic
acid?
Select one:
a. 4.58...
A 25 mL aliquot of an HCl solution is titrated with 0.100 M
NaOH. The equivalence point is reached after 21.27 mL of the base
were added. Calculate 1) the concentration of the acid in the
original solution, 2) the pH of the original HCl solution and the
original NaOH solution, 3) the pH after 10.00 mL of NaOH have been
added, 4) the pH at the equivalence point, and 5) the pH after
25.00 mL of NaOH have been...
A 40.0 mL sample of 0.100 M HCl is titrated with 0.100 M NaOH.
Calculate the pH after the addition of each of the following
volumes of NaOH: (a) 0.0 mL, (b) 10.0 mL, (c) 20.0 mL, (d) 40.0 mL,
(e) 60.0 mL. A plot of the pH of the solution as a function of the
volume of added titrant is known as a pH titration curve. Using the
available data points, plot the pH titration curve for the above...
Consider a mixture of 50.0 mL of 0.100 M HCl and 50.0 mL of
0.100 M acetic acid. Acetic acid has a Ka of 1.8 x 10-5.
a. Calculate the pH of both solutions before mixing.
b. Construct an ICE table representative of this mixture.
c. Determine the approximate pH of the solution.
d. Determine the percent ionization of the acetic acid in this
mixture
50.0 mL of 0.100 M H2SO3 is titrated with
0.150 M KOH soluion.
a) What is the initial pH of the sulfurous acid?
b) How much titrant is needed to reach the equivalence points?
What is the pH at each equivalence point?
c) What is the pH of the solution after the following points of
the titration (with 0.150 M KOH)? (20.0 mL, 33.3 mL, 60.0 mL, 70.0
mL, 100.0 mL, 120.0 mL, 130.0 mL)?
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.
A 25.0 mL sample of 0.100 M acetic acid is titrated with a 0.125
M NaOH solution. Calculate the pH of the mixture after 10, 20, and
30 ml of NaOH have been added (Ka=1.76*10^-5)