Calculate the pH and pOH of the following aqueous solutions at 25°C:
Calculate the pH and pOH of the following aqueous solutions at 25°C: (a) 0.629 M LiOH pH = pOH = (b) 0.199 M Ba(OH)2 pH = pOH = (c) 0.0620 M NaOH pH = pOH =
Complete this table of values for four aqueous solutions at 25
°C.
[H+] [OH-] pH pOH
solutionA : 8.7x10^-7 M
solutionB: 6.9x10^-9 M
solutionC: 9.75
solution D: 6.39
Calculate the pH of the following aqueous solutions at 25°C.
Kw at 25°C is 1.01e-14.
(a) 2.9 ✕ 10−11M KOH
(HINT: Does it make sense to get an acidic pH for this? A neutral
solution may have a higher concentration of OH- than this
solution.)
1
(b) 9.1 ✕ 10−7M
HNO3
2
Calculate the pH of each of the following solutions. (Assume
that all solutions are at 25°C.)
(a) 0.145 M acetic acid
(HC2H3O2, Ka =
1.8 ✕ 10−5)
(b) 0.145 M sodium acetate
(NaC2H3O2)
(d) 0.145 M
HC2H3O2 and 0.145 M
NaC2H3O2
hey so these are really stumping me, any heelp is
appreciated, but it'd really be great if you could take a photo
ofyour work done please so i can learn how it's done.. i keep
getting it wrong
Calculate the pH and
pOH of each of the following
solutions.
- Express your answer to two decimal places. Enter your answers
numerically separated by a comma.
-A) [H3O+]= 1.6×10−8 M
-B) [H3O+]= 1.0×10−7 M
-C) [H3O+]= 2.5×10−6 M
Calculate the pH and pOH for the following solutions:
a) 0.0450 M NaOH
b) 0.160 M Ca(OH)2
c) a 1:1 mixture of 0.0125 M HCl and 0.0125 M Ca(OH)2
d) a 2:3 mixture of 0.0125 M HNO3 and 0.0125 M KOH
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