what is the hydronium ion concentration [H3O+] and the ph of a 0.5M acetic acid solution with Ka=1.8x10^-5? The equation for the dissociation of acetic acid is:
CH3CO2H(aq) + H2O(l) = H3O + (aq) + CH3CO2-(aq)
what is the hydronium ion concentration [H3O+] and the ph of a 0.5M acetic acid solution...
Calculate the hydronium ion concentration and the pH of the solution that results when 10.7 mL of 0.26 M acetic acid, CH3CO2H (Ka= 1.8x10-5), is mixed with 4.9 mL of 0.090 M NaOH . Hydronium ion concentration = M pH=
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 =
please help What is the hydronium ion concentration [H3O+] of a 0.010 M acetic acid solution in water? (K, for acetic acid = 1.76 x 10-5).
Form 1 29. Determine the pH of a 0.741 M LiOH solution at 25°C. A) 0.130 B) 13.87 C) 0.741 D) 13.26 E) 1.18 30. What is the hydronium ion concentration of a 0.500 M acetic acid solu Ka = 1.8 x 10-5? The equation for the dissociation of acetic acid is: centration of a 0.500 M acetic acid solution with CH3CO2H(aq) + H2O(1) = H30+(aq) + CH3CO2"(aq) A) 3.0 x 10-2 M B) 4.2 x 10-2 M C) 3.0...
What is the hydronium ion concentration of a 0.150 M hypochlorous acid solution with Ka-35x 1o-8? The equation for the dissociation of hypochlorous acid is: HOCI(aq) H2O) H30 a)+OCIag) 3.141 4.553 3.721 4.140
Find the hydronium ion concentration and pH for the following 1. 2. Calculate the hydronium ion concentration and the pH when 80.0 mL of 0.55 MNH, is mixed with 80.0 mL of 0.55 M HCl (K. = 5.6 x 10-10). Concentration M pH- Phenol (CH-OH), commonly called carbolic acid, is a weak organic acid. C, H, OH(aq) + H2O(0) = CH.0 (aq) +H3O+ (aq) K= 1.3 x 10-10 If you dissolve 0.593 g of the acid in enough water to...
What is the hydronium ion concentration of a 0.210 M hypochlorous acid solution with K = 2.9x10-87 The equation for the dissociation of hypochlorous acid is: HOCl(aq) + H2O(1) = H2O+(aq) + OCH(aq) 0.210 M O 7.8x10-5 M O 7.8*10-4 M O 6.1x10-9 M
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...
A) A buffer containing acetic acid and sodium acetate has a pH of 5.45. The Ka value for CH3CO2H is 1.80 × 10-5. What is the ratio of the concentration of CH3CO2H to CH3CO2-? [CH3CO2H]/[ CH3CO2-] = _________ B) What is the pH change when 29.6 mL of 0.117 M NaOH is added to 95.4 mL of a buffer solution consisting of 0.123 M NH3 and 0.179 M NH4Cl (Ka for ammonium ion is 5.6x10^-10.) pH change =_______
Calculate the hydronium ion concentration in a solution that contains 0.21 M acetic acid and 0.17 M sodium acetate. For acetic acid, ka = 1.8 x 10^-5