A.Neglecting activity coefficients, calculate the pH of an
aqueous solution of 5.0 x 10-7 M KOH.
B. What fraction of the total [H+ ] is derived from the
autoionization of water?
1. Calculate the pH of a 0.76 M KOH solution.
pH
2.
Be sure to answer all parts.
Calculate the pOH and pH of the following aqueous solutions at 25
°
C:
(a) 0.0715 M LiOH
pH =
pOH =
(b) 0.0521 M Ba(OH)2
pH =
pOH =
(c) 0.12 M NaOH
pH =
pOH =
A 20.00 mL solution of 0.0840M HOCl is titrated with 0.0560M KOH
solution. Calculate the pH after each of the following additions of
the KOH solution:
a. 15.00mL
b. 30.0mL
c. 32.0mL
A 25.0−mL solution of 0.100 M CH3COOH is titrated with a 0.200 M
KOH solution. Calculate the pH after the following additions of the
KOH solution
(a) 10.0 mL
(b) 12.5 mL
(c) 15.0 mL
A 26.0−mL solution of 0.120 M CH3COOH is titrated with a 0.220 M
KOH solution. Calculate the pH after the following additions of the
KOH solution:
(a) 0.00 mL
(b) 5.00 mL
calculate the mean ionic activity of a 0.0350 m Na3PO4 solution
for which the mean activity coeffiecient is 0.685.
Answer should be: 0.0547
Please show me how to get there. Thank you
Calculate the pH during the titration of 30.00 mL of 0.1000 M
KOH with 0.1000 M HBr solution after the following additions of
acid: (a) 5.00 mL (b) 29.50 mL (c) 36.00 mL
Calculate the pH during the titration of 30.00 mL of 0.1000
M KOH with 0.1000 M HBr solution after the
following additions of acid:
(a) 8.00 mL
pH =
(b) 29.80 mL
pH =
(c) 38.00 mL
pH =
calculate the pH for the titration 20 mL of 0.500 M HF
with 0.500 M KOH at the following volumes
ka, HF is 6.8E-4 using the Rice table
a.0 mL
b.10 mL
c.19 mL
d. 20 mL
e. 21 mL
f. 30 mL