36. What is the pH of a 0.0025 M Ba(OH)2 solution? a. 8.70 b. 11.40 c....
The pH of a solution of 0.02 M (2-10^2 M) CH_3 OH (methanol or methyl alcohol) in pure water is: a. 1.70 b. 2.00 c. 2.30 d. 5.30 e. 7.00 f 8.70 g. 11.70 h. 12.30 i. None of the above, the correct pH value is _______________.
Let's suppose that the pH of a solution of Ba(OH)2 is 11.40 by the following equation, Ba(OH)(aq) - Ba²+(aq) + OH (aq) What is expected for the molarity of OH (Hydroxide ion)? DA 1.3 x 10-5 M OB. 1.3 x 10-3M OC 6.0 x 10-4M 0 0.8 3x 10 4 M O E 2.5 x 10-5 M
What is the pH of an aqueous solution contains 0.0025 M of Hydroxide ion? 2.60 3.60 10.40 11.40 8.40
Question 10 3 pts What is the pH of an aqueous 0.0025 M NaOH solution? 10,20 8.95 11.40 2.60
what is the pH of an aqueous solution at 25 C in which [OH-] is 0.0025M? A.)+2.60 B.)-2.60 C.)+11.40 D.)-11.40 E.)-2.25
12) What is the pH of a 1.8 x10^-2 M Ba(OH)2 solution? (a) 12.56 (b) 2.85 (c) 4.44 (d) 6.38 13) What is the pOH of a 1.8 x10^-2 M Ba(OH)2 solution? (a) 1.44 (b) 2.85 (c) 6.37 (d) 9.56 14) Calculate the H3O+ ion concentration of a solution with a pH of 8.34. (a) 2.88 x 10^-9 M (b) 3.85 x 10^-5 M (c) 4.57 x 10^-9 M (d) 6.83 x 10^-5 M
What is the pH of a 2.89*10^-14 M Ba(OH)2 aqueous solution? A)3.24 B) 10.76 C) 9.22 D) 3.54 E) 10.46
What is the pH of a 0.01500 M solution of Ba(OH)2?
7. (a) Define pH (b) Calculate the pH of 0.030 M Ba(OH)2 solution (c) Calculate the pH of a solution containing 0.085 M nitrous acid alone and a solution containing 0.085 M nitrous acid and 0.10 M potassium nitrite (KNO2). K, for HNO2 = 4.5 x 10-
2. The pH of a 0.010 M aqueous solution of Ca(OH)2 is B) 12.00 D) 12.60 A) 11.70 C) 12.30 E) 1.70