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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16) Calculate the H3O+ ion concentration of a solution with a pOH of 13.3. (a) 0.08...
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...
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
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...
2. Calculate the pH, pOH, [H3O+], and [OH-] of a 0.30 M solution of the weak acid, hypobromous acid, HOBr. The Ka value for HOBr is 2.8 x 10-9.
1. Calculate the hydronium ion concentration and the hydroxide ion concentration in lime juice with a pH of 2.0. Report answers in scientific notation and 2 significant figures Hydronium ion concentration = Hydroxide ion concentration = 2. What are the hydronium and hydroxide ion concentrations in a solution whose pH is 6.52? Report answers in scientific notation and 2 significant figures Hydronium ion concentration = Hydroxide ion concentration = 3. Which is the stronger acid, NH4+ or HBrO? Hint: Compare...
Determine pH, pOH, [H3O+] and [OH-] of a 0.265 M HClO solution. Ka of HClO is 2.9 x 10-8.
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 pH and pOH of the solutions with the following hydronium ion [H3O+] or hydroxide ion [OH–] concentrations. Determine which solutions are acidic, basic or neutral. (1.a) [OH–] = 8.2 × 10–11 M (1.b) [OH–] = 7.7 × 10–6 M (1.c) [H3O+] = 3.2 × 10–4 M (1.d) [H3O+] = 1.0 × 10–7 M
Part A A 0.150 M weak acid solution has a pH of 2.97. Find Ka for the acid. Part B Find the percent ionization of a 0.195 M HC2H3O2 solution. (The value of Ka for HC2H3O2 is 1.8×10−5.) Part C Find the pH of a 0.0191 M solution of hypochlorous acid. (The value of Ka for hypochlorous acid is 2.9×10−8.) Part D Find the pH of a 0.014 M solution of HF. (The value of Ka for HF is 3.5×10−4.) Part...
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