Find the pH of each of the following solutions of mixtures of
acids.
8.0×10−2 M in HNO3 and 0.185 M in HC7H5O2,
1.5×10−2 M in HBr and 2.0×10−2 M in HClO4,
9.5×10−2 M in HF and 0.230 M in HC6H5O,
0.100 M in formic acid and 5.5×10−2 M in hypochlorous acid
please show work
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 -]...
Determine the pH of each of the following solutions., 3.6×10−2 M
HI,9.23×10−2 M HClO4, a solution that is 4.0×10−2 M in HClO4 and
4.8×10−2 M in HCl, a solution that is 1.01% HCl by mass (Assume a
density of 1.01 g/mL for the solution.)
please show work
Determine the pH of each of the following solutions. 7.00×10−2 M
HNO3, 0.160 M HNO2, 2.10×10−2 M KOH, 0.245 M CH3NH3I, 0.318 M
KC6H5O.
I am not getting the correst answer to these.... please help and
show work. Thank you
Determine the pH of each of the following two-component
solutions.
1)4.5×10−2 M KOH and 2.5×10−2 M Ba(OH)2
2)0.265 M NH4NO3 and 0.102 M HCN
3)7.5×10−2 M RbOH and 0.120 M NaCl
4)9.2×10−2 M HClO4 and 2.2×10−2 M KOH
5)0.115 M NaClO and 5.50×10−2 M KI
Determine the pH of each of the following two-component
solutions.
1)4.5×10−2 M KOH and 2.5×10−2 M Ba(OH)2
2)0.265 M NH4NO3 and 0.102 M HCN
3)7.5×10−2 M RbOH and 0.120 M NaCl
4)9.2×10−2 M HClO4 and 2.2×10−2 M KOH
5)0.115 M NaClO and 5.50×10−2 M KI
Determine the chloride ion concentration in each of the
following solutions:
0.130 M
BaCl2:
M
0.666 M NaCl:
M
1.802 M
AlCl3:
M
(b) What is the concentration of a
Sr(NO3)2
solution that is 1.55 M in
nitrate ion?
M
Calculate the pH at the equivalence point in titrating 0.120 M solutions of each of the following with 8.0×10−2M NaOH....
sodium hydrogen chromate (NaHCrO4)