Part A: Calculate the [H3O+] of the following polyprotic acid
solution: 0.370 M H3PO4. Express your answer using two significant
figures.
Part B: Calculate the pH of this solution.
Express your answer using one decimal place.
Part C: Calculate the [H3O+] and pH of the following polyprotic
acid solution: 0.360 M H2C2O4. Express your answer using two
significant figures.
Part D: Calculate the pH of this solution.
Express your answer using two decimal places.
Thank you so much!!
Calculate the [H3O+] of the following polyprotic acid solution:
0.380 M H3PO4. Express your answer using two significant figures.
[H3O+] =
Part B Calculate the pH of this solution. Express your answer
using one decimal place. pH =
Part C Calculate the [H3O+] and pH of the following polyprotic
acid solution: 0.330 M H2C2O4. Express your answer using two
significant figures. [H3O+] =
Part D Calculate the pH of this solution. pH
=
Calculate the [H3O+] of the following polyprotic acid solution:
0.135 M H3C6H5O7.
Express your answer using two significant figures.
Calculate the pH of this solution
Express your answer to two decimal places.
Calculate the [H3O+] and pH of each polyprotic acid
solution.
Dissociation Constants for Acids at 25 ∘C
Formula
Ka1
Ka2
Ka3
H2CO3
4.3×10−7
5.6×10−11
H3C6H5O7
7.4×10−4
1.7×10−5
4.0×10−7
PART A
0.130 M H3C6H5O7 H3O+
=
PART B
0.130 M H3C6H5O7 pH =
Phosphoric acid, H3PO4(aq), is a triprotic acid. Calculate the
pH and concentrations of H3O + (aq), H3PO4(aq), H2PO4 − (aq), HPO4
2− (aq), PO4 3− (aq), and OH− (aq) in a 0.100-M phosphoric acid
solution at 25°C.
Calculate the [H3O+] and pH of the polyprotic H3C6H5O7 with an
initial concentration 0.125 M. I got 0.011, but apparently it is
wrong even though I added the three dissociated concentrations.
Help would be very much appreciated! Here are the Ka values:
Ka1=7.4*10^-4, Ka2=1.7*10^-5 Ka3=4.0*10^-7
Calculate the pH at 25 C of a 0.75 M aqueous solution of
phosphoric acid (H3PO4). (Ka1, Ka2, and Ka3 for phosphoric acid are
7.5*10-3, 6.25*10-8, and
4.8*10-13, respectively.)
Calculate [H3O + ] for a 2.5 x 10-4 M solution of weak acid (Ka
= 5.3 x 10-4 )
A.
1.4 x 10-4 M
B.
2.1 x 10-4 M
C.
6.2 x 10-4 M
D.
7.3 x 10-4 M
E.
1.9 x 10-4 M
Calculate the pH at 25°C of a 0.65 M aqueous solution of
phosphoric acid (H3PO4). (Ka1, Ka2, and Ka3 for phosphoric acid are
7.5 × 10−3, 6.25 × 10−8, and 4.8 × 10−13, respectively.)
Please show how you do the quadratic equation. I am struggling
with this in particular. Thank you!