answer is D but I gotta show work
answer is D but I gotta show work A 0.19 m Silution a weak acid tund...
please give an explanation/ show work! thank you! For the diprotic weak acid H2A, Kal =2.0 x 10- and Ko e =8.6 x 10 What is the pH of a 0.0750 M solution of H,A? pH What are the equilibrium concentrations of H,A and A in this solution? H,A] = [A21=
What is the percent ionization of a 0.0741 M solution of a weak acid if the weak acid ionization constant, ka, is 2.0 x 10at 25 °C? Select one: a. 0.038% b. 0.30 % c. 1.4% d. 0.52% e. 5.2%
The pH of a 0.19 M solution of carbonic acid (H2CO3) is measured to be 3.53. Calculate the acid dissociation constant K, of carbonic acid. Round your answer to 2 significant digits. K = 1) x 6 ?
50.0 mL sample of the weak acid the concentration of the weak acid = 0.15 M 25 mL of the week acid into 100 mL beaker titrated this solution of 0.21 M NaOH moles of weak acid = 3.75*10^-3 moles of NaOH = moles of week acid c) How many milliliters of the NaOH are required to neutralize the sample of weak acid? d) How many moles of NaOH have been added at one half of the volume in part...
1 attempts left Check my work Be sure to answer all parts. In a 0.10 M solution, a weak acid is 1.0% dissociated. (a) Calculate the (H:0"],pH, OH), and pOH of the solution, lo 10 x 10 M [H30+] - M [OH)= pOH = pH = (b) Calculate K, of the acid.
2. DILUTION EFFECT ON THE PERCENT IONIZATION OF A WEAK ACID a. A weak acid, HX, is 1.3 % ionized in 0.20 M solution. What percent of HX is ionized in a 0.030 M solution? Show the complete setup. percent ionization b. From your result in (a) above answer the following questions: i) How did the percent of ionization change upon dilution? (increased, or decreased) ii) How did the [H,O') concentration of the above weak acid change upon dilution? (increased,...
please show all the work! 05124120 Benzoic acid or (B204) is a weak aud ike of 66.246x 10") often used in organic Chemistry - What is the pH of a 0.026 M solution of sodium benzoate Bz O Na?
2. (Acid Base Equilibria) lodic Acid (HI03) is a weak acid. If there are initially, 0.03 M of iodic acid present, calculate the equilibrium concentrations of the species present at equilibrium. EXPLAIN AND SHOW ALL WORK. HI03 H30103 Ka 17 x 10-1
A titration is carried out for 20.0mL of 0.10 M Oxalic Acid (weak acid) with 0.10 M of a strong base NaOH. Calculate the pH at these volumes of added base solution: (a) 0.0 mL (b) 5.0 mL (c) 10.0 mL (d) 15.0 mL (e) 20.0 mL (f) 25.0 mL (g) 30.0 mL Oxalic acid Ka1 = 5.9 x 10-2 Ka2 = 6.4 x 10-5
A) Find the pH of a 0.120 M solution of a weak monoprotic acid having Ka= 1.5×10−5. B) Find the percent dissociation of this solution. C) Find the pH of a 0.120 M solution of a weak monoprotic acid having Ka= 2.0×10−3. D) Find the percent dissociation of this solution. E) Find the pH of a 0.120 M solution of a weak monoprotic acid having Ka= 0.14. F ) Find the percent dissociation of this solution.