15) Calculate the OH- ion concentration of a solution with a pH of 3.75.
(a) 1.78 x 10^-10 M (b) 2.17 x 10^-8 M (c) 2.75 x 10^-5 M (d) 5.62 x 10^-11 M
16) Calculate the H3O+ ion concentration of a solution with a pOH of 13.3.
(a) 0.08 M (b) 0.20 M (c) 0.29 M (d) 0.35 M
17) Calculate the Kb of Hypochlorous acid, Ka= 3.5 x10^-8.
(a) 1.3 x 10^-4 (b) 2.9 x 10^-7 (c) 3.1 x 10^-6 (d) 8.6 x 10^-4
18) Calculate the pKa of Hypochlorous acid, Ka= 3.5 x10^-8.
(a) 5.32 (b) 6.64 (c) 8.92 (d) None of the above
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15) Calculate the OH- ion concentration of a solution with a pH of 3.75. (a) 1.78...
16) Calculate the H3O+ ion concentration of a solution with a pOH of 13.3. (a) 0.08 M (b) 0.20 M (c) 0.29 M (d) 0.35 M 17) Calculate the Kb of Hypochlorous acid, Ka= 3.5 x10^-8. (a) 1.3 x 10^-4 (b) 2.9 x 10^-7 (c) 3.1 x 10^-6 (d) 8.6 x 10^-4 18) Calculate the pKa of Hypochlorous acid, Ka= 3.5 x10^-8. (a) 5.32 (b) 6.64 (c) 8.92 (d) None of the above
Question 39 Calculate the Kb of Hypochlorous acid, Ka=3.5 x10^-8. (1 point) 1.3 x 10^-4 2.9 x 10^-7 O 3.1 x 10^-6 O 8.6 x 10^-4 Question 40 Calculate the pka of Hypochlorous acid, Ka- 3.5 x10^-8. (1 point) 5.32 6.64 8.92 None of the above
E HW 9 х General Chemist (2) CHEM1306 Nove periodic QLSCHXbptcoEd-U3INKhrsvudurkW 3 VierPPORB9074HTOHSPQ/viewform Question 37 Calculate the OH-ion concentration of a solution with a pH of 3.75. (1 point)* 1.78 x 10^-10 M 2.17 x 10^-8 M 2.75 x 10^-5 M O 5.62 x 104-11 M Question 38 Calculate the H3O+ ion concentration of a solution with a pOH of 13.3. (1 point) * 0.08 M 0.20 M 0.29 M 0.35 M Question 39
Calculate the hydroxide ion concentration and the POH in an aqueous solution with a pH = 2.3 at 25°C. a. [OH 1 - 2.0 * 10-12M : POH - 2.30 b. [OH 7 -2.0 * 10-11M: POH = 11.70 C[OH 7 -5.0 x 10-3 M : POH = 11.70 d. [OH ) - 2.0 x 10-12 M : POH = 11.70 e.[OH ) - 2.0*10-12M : POH -8.50 Which of the following solutions is a good buffer system? a. A...
1) The pH of an aqueous solution at 25°C was found to be 13.00. The pOH of this solution is ___ The hydronium ion concentration is ____M. The hydroxide ion concentration is ____M. 2) The hydronium ion concentration in an aqueous solution at 25°C is 3.6×10-2M. The hydroxide ion concentration is M. The pH of this solution is ____. The pOH is _____ . 3) What is the pOH of an aqueous solution of 0.467 M hydrochloric acid? pOH = ___...
Calculate the pH of a solution with an analytical concentration of formate ion equal to 0.1500 M. The Ka for formic acid is 1.8 x 10-4
A. What is the pH of an aqueous solution with a hydrogen ion concentration of H] = 8.8 x 10-'M? pH = B. What is the hydroxide ion concentration, (OH), in an aqueous solution with a hydrogen ion concentration of [H+] = 8.8 x 10-'M? [OH-] = C. A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) =H(aq) + (aq) The equilibrium concentrations of the reactants and products are [HA] = 0.300 M, H+] = 4.00...
the pOH of a solution is 10.40. Calculate the hydrogen ion concentration in the solution. a) 4.0 x 10^-11 M b)3.6 M c)4.0 x 10^-10 d)2.5 x 10 ^-4 e)1.8 x 10^-4
Calculate the hydronium ion concentration and the pH of the solution that results when 22.6 mL of 0.060 M acetic acid,CH3CO2H (Ka= 1.8 x 10^-5), is mixed with 1.4 mL of 0.17 M NaOH . Hydronium ion concentration = pH =
a) What is the pH of an aqueous solution with a hydrogen ion concentration of [H']-7.5 x10-3 M? Number PH- b) What is the hydroxide ion concentration, [OH-], in an aqueous solution with a hydrogen ion concentration of[H+] = 7.5x10-3 M? Number OH-]= c) A monoprotic acid, HA, dissociates: H A H+A HA The equilibrium concentrations of the reactants and products are HA]-0.240 M [H+] = 4.00 x 10-4 M A] 4.00 x104M continued below... Calculate the Kg value for...