Question

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.

Answer #1

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 0.1000 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.

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

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 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 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.

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.

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.

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