H2O (l) <................> H+ (aq) + OH- (aq)
Kw = [H+][OH-]
or
1.53 * 10^-13 = [H+][OH-]
at equilibrium, [H+] = [OH-]
thus
1.53 * 10^-13 = [OH-]^2
or
[OH-] = 3.91 * 10^-7 M
pOH = - log[OH-]
or
pOH = - log (3.91 * 10^-7 )
or
pOH = 6.408
thus
option B) 6.408 is the answer.
water at 70°C? (Kw at 70°C = 1.53 Ⓡ 10-13) What is the pOH of pure...
At 70°C, the ion-product constant of water, Kw, is 1.53 × 10–13 The pH of pure water at 70°C is: Select one: a. 5.828. b. 7.000. c. 6.508. d. 6.408.
What is the poH of pure water that has a Kw value of 4.38 x 10-14? O a. 7 O b. 13.36 O c. 6.80 O d.6.36 O e. 6.68
At 100 degrees Celsius, the ion product for pure water is Kw= 51.3*10^-14. What is the pOH of water at this temperature? A) 7.00 B) 7.27 C) 6.14 D) 6.63 E) 7.86
3) What is the concentration of hydroxide ions in pure water at 30.0°C, if Kw at this temperature is 1.47 10-14? 4) What is the pH of pure water at 40.0°C if the Kw at this temperature is 2.92 x 10-14?
At 10 °C, the ion product for pure water is Kw = 0.293 x 10-14 What is the pH of water at this temperature? 7.27 6.14 7.00 6.86 6.63
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?
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...
The ionization product of water, KW, is 3.5 × 10–13 at 80 °C. What is the pH of a neutral aqueous solution at this temperature?
for water (Kw) is 9.311 × 10-14 at 60 oC. Calculate the [H2O+], [OH-], pH, (8 pts.) The ionization constant and pOH for pure water at 60°C
The pOH of pure water at 40oC is 6.8. What is the hydronium concentration, [H3O+], in pure water at this temperature?