We know that
pH + pOH = pKw
Given that
pOH = 6.50
Kw = 6.22 × 10–15
pKw = – logKw = – log(6.22 × 10–15) = 14.20621 = 14.21
pH = pKw – pOH = 14.21 – 6.50 = 7.71
pH of the solution = 7.71
A solution has a pOH of 3.80 at 50°C. What is the pH of the solution given that Kw = 6.70 x 10-14 at this temperature? • Round the answer to two decimal places. Provide your answer below: pH = 0
Use pOH in calculations Question A solution has a pOH of 3.80 at 50°C. What is the pH of the solution given that K - 6.70 x 104 at this temperature? . Round the answer to two decimal places. Provide your answer below:
A 10∘C solution has a pH of 8.0. At this temperature, Kw=2.93 × 10^−15. What is the pOH of the solution? Select the correct answer below: a. 1.0 b. 6.0 c. 6.5 d. 8.5 A 10 °C solution has a pH of 8.0. At this temperature, Kw = 2.93 x 10-15. What is the pOH of the solution? Select the correct answer below: O 1.0 O 6.0 O 6.5
Perform calculations that relate pH and POH Question = 5.48 x 10" at this temperature? A solution has a pH of 9.5 at 50 °C. What is the pOH of the solution given that K Select the correct answer below: O 2.5 O 3.8 4.5 Next Previous
An aqueous solution at 25°C has a pH of 9.2. Calculate the pOH. Round your answer to 1 decimal places. X 5 ?
Perform calculations that relate pH and POH Question What is the pH of a solution with [H, 0+1= 1.50 x 10-M? Report your answer to the hundredths place. Provide your answer below:
What is the relationship between pH, pOH, and Kw at that temperature? (Note: Select all that apply.) I don't understand the last question. Any explanation will help! Review Problem 16.060 At the temperature of the human body, 37 °C, the value of Kw is 2.5 x 10-14. Calculate (H+], [OH"), pH, and pOH of pure water at that temperature. [H+] = 1.6 x 10-7 M [OH-] = 1.6 x 103 m pH = 6.80 The number of significant digits is...
A solution has a hydrogen ion concentration of 10-5 M. What is the pH and pOH of the solution? (Assume temperature is 25C) Please with steps
At 50 oC, Kw = 5.48 × 10-14 What is pH + pOH at 50oC? A. 14.00 B. 3.54 C.14.26 D. 14.5 E. 13.26 Answer: E Why?
pH is a logarithmic scale used to indicate the hydrogen ion concentration, [H+], of a solution: pH = -log[H+]Due to the autoionization of water, in any aqueous solution, the hydrogen ion concentration and the hydroxide ion concentration, [OH-], are related to each other by the Kw of water: Kw = [H+][OH-] = 1.00 x 10-14where 1.00 x 10-14 is the value at approximately 297 K. Based on this relation, the pH and pOH are also related to each other as 14.00 = pH...