Question

(a) Calculate the quotient [H_{3}PO_{4}]/[H_{2}PO_{4}^{−} ]
in 0.0463 *M* KH_{2}PO_{4}. (Assume
*K*_{w} = 1.01 ✕ 10^{−14}, *K*_{a1} = 7.11 ✕ 10^{−3}, *K*_{a2} = 6.34 ✕ 10^{−8}, and *K*_{a3} = 4.22 ✕ 10^{−13}.)

Answer #1

Calculate the pH and the equilibrium concentrations of H2PO4-,
HPO42- and PO43- in a 0.0353 M aqueous phosphoric acid solution.
For H3PO4, Ka1 = 7.5×10-3, Ka2 = 6.2×10-8, and Ka3 = 3.6×10-13
pH = ?
[H2PO4-] = ?M
[HPO42-] = ?M
[PO43-] = ?M

Given the following Ka values:
H3PO4 <-->
H2PO4- + H+, Ka =
7.11*10-3
H2PO4- <-->
HPO42- + H+, Ka =
6.34*10-8
HPO42- <-->
PO43- + H+, Ka =
4.22*10-13,
a) please calculate the pH of the solution at the first
equivalence point for the above titration.
b) In the same titration as described above, what's the pH of
the solution after 15.00 mL of NaOH was added?

What is the [H2PO4-] of a
solution labeled "0.10 M Phosphoric Acid
(H3PO4)"?
[Ka1 = 7.1x10-3; Ka2 =
6.3x10-8; Ka3 = 4.2x10-13]
A. 4.2x10-13 M
B. 2.7x10-2 M
C. 7.1x10-3 M
D. 1.6x10-9 M
E. 1.6x10-16 M

What is the (H2PO4-) of a solution labeled "0.10 M Phosphoric
Acid"? [Ka1= 7.1 x 10 ^ -3 , Ka2= 6.3 x 10^ -8, Ka3 = 4.2 x 10
^-13]

Calculate the quotient [H3PO4]/[H2PO4] in 0.05 M K2HPO4. K1=
7.11x10^-3, K2= 6.32x10^-8, K3=4.17x10^-3

Calculate the pH during the titration of 50.00 mL of 0.1000 M
phosphoric [H3PO4; Ka1=7.1 x 10^(-3), Ka2=6.3 x 10^(-8), Ka3=4.2 x
10^(-13)] after adding 33.42 mL of 0.1000 M NaOH.

Calculate the pH of 0.103 M phosphoric acid
(H3PO4, a triprotic acid). Ka1 =
7.5 x 10-3, Ka2 = 6.2 x 10-8, and
Ka3 = 4.8 x 10-13.
Hint, if you are doing much work, you are making the problem harder
than it needs to be.

Phosphoric acid is a triprotic acid, and the Ka values are given
below. Calculate pH, pOH, [H3PO4], [H2PO4 2-], [HPO4 -], and [PO4
3-] at equilibrium for a 5.00 M phosphoric acid solution.
Ka1 = 7.5 x 10^-3
Ka2 = 6.2 x 10^-8
Ka3 = 4.2 x 10^-13

Which is the most prevalent species in a 0.25M aq solution of
phosphoric acid, H3PO4?
Ka1 = 7.5x10-3 , Ka2 = 6.2x10-8
, Ka3 = 4.2x10-13
a) H3PO4
b) H2PO4-
c) HPO42-
d) H3O+
The answer is A, can you explain why?

3. Show how phosphoric, H3PO4, dissociates
in water and calculate the pH of a 0.030 M solution of the acid.
Ka1 = 7.5 x 10-3; K a2 = 6.2 x
10-8; Ka3 = 4.8 x 10-13

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 23 minutes ago

asked 36 minutes ago

asked 43 minutes ago

asked 43 minutes ago

asked 54 minutes ago

asked 57 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago