Calculate [OH -] and pH for each of the following
solutions.
(a) 0.0034 M RbOH
[OH-] =_________ M
pH = _________
(b) 0.0872 g of KOH in 510.0 mL of solution
[OH -] =__________ M
pH = __________
(c) 79.8 mL of 0.00719 M Sr(OH)2 diluted to 900
mL
[OH -] = __________ M
pH = ____________
(d) A solution formed by mixing 64.0 mL of 0.000880 M
Sr(OH)2 with 36.0 mL of 2.6 x 10-3 M
RbOH
[OH -]...
Calculate [OH -] and pH for each of the following
solutions.
(a) 0.0043 M KOH
[OH-] = _____ M
pH = 11.63
(b) 0.0341 g of CsOH in 540.0 mL of solution
[OH -] = 4.21e-4 M
pH = 10.62
(c) 28.1 mL of 0.00187 M Ca(OH)2 diluted to 800
mL
[OH -] = _____ M
pH = 10.12
(d) A solution formed by mixing 71.0 mL of 0.000480 M
Ca(OH)2 with 24.0 mL of 1.3 x 10-3 M
KOH
[OH -] =...
1.Determine the pH and pOH for
each of the following solutions:
[OH−] = 1.6×10−7 M
[H3O+] = 4.5×10−4 M
[H3O+] = 2.0×10−4 M
[OH−] = 7.5×10−9 M
2.Acetic acid has a Ka of
1.8×10−5
What is the pH of a buffer solution containing 0.20 M HC2H3O2
(acetic acid) and 0.20 M C2H3O2−?
3. A volume of 40.0 mL of a 0.850 M HNO3 solution is
titrated with 0.780 M KOH. Calculate the volume of KOH
required to reach the equivalence...
Calculate [H3O+] and [OH−] for each of the following solutions at 25℃ given the pH.
Part A: pH= 8.60 Express your answer using two significant figures. Enter your answers numerically separated by a comma.
Part B: pH = 11.34
Part C: pH = 2.91
For each of the following strong base solutions, determine
[OH−],[H3O+], pH, and
pOH.
1. 6.77×10−3 M LiOH,
2. 0.0412 M Ba(OH)2
3. 5.9×10−4 M KOH
4. 3.0×10−4 M Ca(OH)2
Determine the pH of each of the following solutions
A)8.1×10−3 M phenol
B)9.5×10−2 M hydroxylamine.
Calculate the percent ionization of propionic acid (C2H5COOH) in
solutions of each of the following concentrations
(Ka is given in Appendix D in the textbook).
A)0.260 M .
B) 8.05×10−2 M .
c)1.99×10−2 M .
Calculate the pH, pOH, [H3O+], and [OH-] of the following
solutions:
(a) 0.001 M HNO3,
(b) 0.3 M Ca(OH)2;
(c) 3.0 M HNO3,
(d) 6.0 M NaOH,
(e) 0.05 M HBr
Find the pH of each of the following solutions
of mixtures of acids.
1) 7.0×10−2 M in HNO3 and 0.180 M in
HC7H5O2
2) 1.5×10−2 M in HBr and
2.0×10−2 M in HClO4