Question

What is the [H_{2}PO_{4}^{-}] of a
solution labeled "0.10 M Phosphoric Acid
(H_{3}PO_{4})"?

[K_{a1} = 7.1x10^{-3}; K_{a2} =
6.3x10^{-8}; K_{a3} = 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

Answer #1

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 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.

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?

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.

2The acid-dissociation constants of phosphoric acid (H3PO4) are
Ka1 = 7.5 × 10-3, Ka2 = 6.2 × 10-8, and Ka3 = 4.2 × 10-13 at 25.0
°C. What is the molar concentration of phosphate
ion in a 2.5 M aqueous solution of phosphoric acid?
A) 0.13
B) 2.5 × 10-5
C) 8.2 × 10-9
D) 9.1 × 10-5
E) 2.0 × 10-19
Can you include the complete
steps where Ka2 and Ka3 is used.

phosphoric acid, H3PO4(aq), is a triprotic acid, meaning that
one molecule of acid has 3 acidic protons. estimate the pH and
concentration of all species in a .200 M phosphoric acid solution
Ka1=6.9x10^-3, Ka2=602x10^-8, Ka3=4.8x10^-13

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.

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

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