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![Ihave some acetic acid that dissociates in water.
[CH3COOH] = 0.405 M and [CH3COO]=0.505 M.
K3=1.8x10-5. Find the pH=? (3 sig fig)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3168e1bb-2109-44d1-a44a-81ed2e7f4d53%2F3eaaacd8-0d34-4bbf-b6c7-1b51b059559d%2Fuyiaoq.png&w=3840&q=75)
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- . Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.(a) Calculate the percent ionization of 0.00800 M butanoic acid (K₂ = 1.5e-05). % ionization = % (b) Calculate the percent ionization of 0.00800 M butanoic acid in a solution containing 0.0610 M sodium butanoate. % ionization = %Complete the balanced chemical equation for the following reaction between a weak acid and a strong base. CH:NH:CI(aq) + NaOH(aq) 4- 2+ | ]3+ 1 3 4 6 7 8 D4 15 Do ) (s) (1) (g) (aq) Na H C CI Reset • x H2O Delete 1L 2. +
- What is the pH of a 2.4 x 10-4 M NH3 solution? (?? = 1.8 x 10-5) What is the pH of a 0.075 M HBrO? (?a = 2.5 x 10-9)What is the ratio of NH4+ to NO2- in O2-saturated water when the pH is 8.20 and the pE is 4.42? (Ecell = 0.895)(a) Calculate the percent ionization of 0.00170 M butanoic acid (K₁ = 1.5e-05). % ionization = 8.96 % (b) Calculate the percent ionization of 0.00170 M butanoic acid in a solution containing 0.0610 M sodium butanoate. X% % ionization -
- 1) H3O+ 2)H₂CrO 4 3)[H*], NH,NHz, - H,O 4) KOH/H₂O, heatBe sure to answer all parts. Determine the pH of the following solutions at 25°C. (a) [H,0*] = 2.19 × 10-10 M pH (b) [H,0*]= 5.50 x 10-3 M pH ( Prev 18 of 2-What is the pH of the original 0.400 M propionic acid solution? K₂HA = 1.34 x 10-5 pH of 0.40 M HA = [?] Initial pH Enter
- Calculate the pH and fraction of dissociation (?) for each of the acetic acid (CH3COOH, p?a=4.756 ) solutions. A 0.00393 M solution of CH3COOH . pH= ?= A 1.93×10−12 M solution of CH3COOH . pH= ?= (Please type answer no write by hend)4. Determine the pOH of each solution. (a) [H3O*] = 1.2 × 10-8 M (b) [H3O*] = 5.5 × 10-2 M (c) [H3O*] = 3.9 × 10-9 M (d) [OH¯] = 1.88 × 10-13 M(Q9) The base ionization constant for (Kp) for acetate ion (CH3CO0') is equal to: O 4.75 9.25 O 1.8 x 10-5 O Is undefined (i.e., there is no such thing) 5.6 x 10-10