Question

Calculate the pH during the titration of 40.00 mL of 0.1000M propanoic acid (HPr; Ka=1.3x10-5) after adding 16.33 mL of 0.1000M NaOH. ** All volumes should have a minimum of 2 decimal places.

Answer #1

M(HPr) = 0.1 M

V(HPr) = 40 mL

M(NaOH) = 0.1 M

V(NaOH) = 16.33 mL

mol(HPr) = M(HPr) * V(HPr)

mol(HPr) = 0.1 M * 40 mL = 4 mmol

mol(NaOH) = M(NaOH) * V(NaOH)

mol(NaOH) = 0.1 M * 16.33 mL = 1.633 mmol

We have:

mol(HPr) = 4 mmol

mol(NaOH) = 1.633 mmol

1.633 mmol of both will react

excess HPr remaining = 2.367 mmol

Volume of Solution = 40 + 16.33 = 56.33 mL

[HPr] = 2.367 mmol/56.33 mL = 0.042M

[Pr-] = 1.633/56.33 = 0.029M

They form acidic buffer

acid is HPr

conjugate base is Pr-

Ka = 1.3*10^-5

pKa = - log (Ka)

= - log(1.3*10^-5)

= 4.8861

use:

pH = pKa + log {[conjugate base]/[acid]}

= 4.8861+ log {0.029/0.042}

= 4.72

Answer: 4.72

Calculate the pH during the titration of 40.00 mL of 0.1000M
propanoic acid (HPr; Ka=1.3x10-5) after adding 26.5 mL of 0.1000M
NaOH. ** All volumes should have a minimum of 2 decimal places.

Calculate the pH during the titration of 40.00 mL of 0.1000M
propanoic acid (HPr; Ka=1.3x10-5) after
adding 10.41 mL of 0.1000M NaOH.
** All volumes should have a minimum of 2 decimal places.

Calculate the pH during the titration of 40.00 mL of 0.1000M
propanoic acid (HPr; Ka=1.3x10-5) after adding 20.98 mL of 0.1000M
NaOH.

Calculate the pH during the titration of 40.00 mL of a 0.1000 M
propanoic acid (Ka = 1.3 x 10^-5) after each of the following
volumes of 0.1000M NaOh has been added. Use ICE tables to show your
work.
a) 0.00 mL
b) 25.00 mL
c) 40.00 mL
d) 50.00 mL
The answers are:
a. 2.96
b. 5.12
c. 8.80
d. 12.05
Show work on how you arrive to each solution.

Calculate the pH during the titration of 50.00 mL of 0.1000M
phosphoric (H3PO4; Ka1=7.1x10-3, Ka2=6.3x10-8, Ka3=4.2x10-13) after
adding 33.71 mL of 0.1000M NaOH. ** All volumes should have a
minimum of 2 decimal places.

Calculate the pH during the titration of 50.00 mL of 0.1000M
phosphoric (H3PO4; Ka1=7.1x10-3, Ka2=6.3x10-8, Ka3=4.2x10-13) after
adding 33.71 mL of 0.1000M NaOH. ** All volumes should have a
minimum of 2 decimal places.

Calculate the pH during the titration of 50.00 mL of 0.1000M
phosphoric (H3PO4; Ka1=7.1x10-3, Ka2=6.3x10-8, Ka3=4.2x10-13) after
adding 28.79 mL of 0.1000M NaOH. ** All volumes should have a
minimum of 2 decimal places.

Calculate the pH during the titration of 50.00 mL of 0.1000M
phosphoric (H3PO4; Ka1=7.1x10-3, Ka2=6.3x10-8, Ka3=4.2x10-13) after
adding 24.16 mL of 0.1000M NaOH.

Be sure to answer all parts.
Calculate the pH during the titration of 40.00 mL of 0.1000
M HCl with 0.1000 M NaOH solution after the
following additions of base:
(a) 20.00 mL
pH =
(b) 39.50 mL
pH =
(c) 51.00 mL
pH =

Calculate the pH during the titration of 20.00 mL of 0.1000 M
C2H5COOH(aq) with 0.2000 M LiOH(aq) after 9.7 mL of the base have
been added. Ka of propanoic acid = 1.3 x 10-5.

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 20 minutes ago

asked 28 minutes ago

asked 29 minutes ago

asked 30 minutes ago

asked 32 minutes ago

asked 41 minutes ago

asked 52 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago