Ba(OH)2 is a strong base. It dissociates completely as:
Ba(OH)2 = Ba2+ + 2 OH-
Thus, from the balanced reaction, 1 mole Ba(OH)2 gives 2 mole OH- .
So, 0.01500 M Ba(OH)2 will give 2 x 0.01500 M = 0.03000 M OH- .
Now,
pOH = -log[OH_] = -log[0.03000] = 1.5229
and pH = 14 – pOH = 14 – 1.5229 =12.4771
Answer = 12.48
Calculate the [OH^-], pOH and pH of a 0.232 M solution of Ba(OH)_2. Ba(OH)_2 (aq) rightarrow Ba^2+ (aq) + 2 OH^-(aq)
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 0.164 M solution of Ba(OH)2? Round answer to two decimal places. please show work
Question 34 What is the pH of a 1.8 x10^-2 M Ba(OH)2 solution? (1 point)* O 12.56 02.85 04.44 O 6.38 Question 35 What is the pOH of a 1.8 x10^-2 M Ba(OH)2 solution? (1 point)* O 1.44 2.85 6.37
36. What is the pH of a 0.0025 M Ba(OH)2 solution? a. 8.70 b. 11.40 c. 2.60 d. 11.70 e. 2.30
What is the pH of the resulting solution when 19.84 mL 0.128 M Ba(OH)2 is added to 52.05 mL 0.1267 M HCl? Enter your answer to three significant figures.
3. Calculate [OH-], [H], POH, and pH of a 0.0020 M Ba(OH)2 solution at 25°C.
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-
Part A What is the pH of a 0.0020 M Ba(OH)2 solution? 0 2.40 O 11.60 O 2.70 O 11.30 Submit Previous Answers Request Answer X Incorrect; Try Again Provide Feedback
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