17. At 30 °C Kw = 1.471 x 10 -14. What is the [ H] and [OH-] at a neutral pH? ( 12 pt)
17. At 30 °C Kw = 1.471 x 10 -14. What is the [ H] and [OH-] at a neutral pH? ( 12 pt)
11. Calculate pH of the following solutions. At 25°C, Kw- [H30*] [OH'] = 1.00 x 10-14 pH=-log [H30 ] a) [H30 ] 2.30 x 10-12 M pOH=- log [OH] pH+ pOH = 14 b) [OH]=9.7x 102 M
SIMULATION Kw, Temperature, and Neutral pH 14.0 Temperature: Basic 50 °C Basic 1 → Calculate Clear 1 Neutral pH 7.01 Neutral => Neutral pH = 6.62 Kw=5.8 10-14 Acidic Acidic 0.0 0.0 50.0 Temperature (°C) 100.0 What is the [H3O+] for a neutral solution at this temperature, 50 °C? X mol/L Next (3 of 8) Recheck 5th attempt Since a neutral solution has equal concentrations of H30+ and OH-, we know that [H3O+] = [OH-] = x and Kw =...
What pH would be neutral if Kw = 6.40 x 10-14? Please show all work. Thanks!
The value of Kw at 25 °C is 1.0 × 10-14. At 30 °C, the value of Kw is 1.5×10-14. a.) Using LeChatelier's principle, predict whether the autoionization of water is exothermic or endothermic. 2 H2O(l) ⇄ H3O+(aq) + OH-(aq) b.) Calculate [H3O+] and [OH-] in a neutral solution at 30°C. What are the concentrations of [H3O+] and [OH-] in a neutral solution at 30 °C? [H3O+] = ???? M [OH-] = ???? M
The Kw for water at 0 °C is 0.12 x 10-14. Calculate the pH of a neutral aqueous solution at 0 °C. pH = Is a pH = 7.25 solution acidic, basic, or neutral at 0°C? O acidic basic neutral O
Given that Kw for water is 2.4 x 10-14 at 37 °C, calculate the pH of a neutral aqueous solution at 37 °C, which is the normal human body temperature. PH - Is a pH 7.00 solution acidic, basic, or neutral at 37 °C? O acidic O basic O neutral
(16-14) Given that Kw for water is 2.4 x 10^-14 at 37 degree C, compute the pH of a neutral aqueous solution at 37 degree C, which is the normal human body temperature. pH= Is a pH = 7.00 solution acidic, basic, or neutral at 37 degree C? Acidic basic neutral
7) At 50°C the value of Kw is 5.5 x 10-14. At what pH is waster neutral at 50°C. A) 6.63. B) 5.50. C) 7.00 D) 7.37. 8) A solution with a hydroxide ion concentration of 4.15 x 10-4 M is and has a hydrogen ion concentration of A) basic, 2.41 x 10-10 M B) acidic, 2.41 * 10-10 M C) basic, 2.41 x 10-11 M D) acidic, 2.41 x 10-11 M 9) Which one of the following salts, when...
Question 12 of 17 > Calculate the hydroxide ion concentration, [OH-], for a solution with a pH of 6.96. [OH-] = 3.98 x10-10 | М Incorrect Question 13 of 17 > Calculate the [OH-] and the pH of a solution with an (H+] = 6.6 x 10-12 M at 25°C. [OH-] = M pH = Calculate the (H+) and the pH of a solution with an [OH-] = 0.86 M at 25 °C. H+] = M pH = Calculate the...