For the following reaction: HC2H3O2 ⇔ H+ + C2H3O2– , if [HC2H3O2] = 1.0 × 10^–8 M and the pH = 3.0, what is K?
A) 1.0 × 10^–2
B) 10.0
C) 1.00 × 10^–6
D) 100
For the following reaction: HC2H3O2 ⇔ H+ + C2H3O2– , if [HC2H3O2] = 1.0 × 10^–8...
In the following reaction: HC2H3O2 ⇔ H+ + C2H3O2–, if [HC2H3O2] = 0.28 M and the pH = 5.0, what is K?
Important Info: Ka reaction: HC2H3O2(aq) + H2O(l) <-->C2H3O2 (aq) +H3O+(aq) HC2H3O(aq) +OH-(aq) -> C2H3O2-(aq) + H2O (l) A 1.0 L buffer solution is 0.280 M in HC2H302 (acetic acid) and 0.320 M in NaC2H302 (sodium acetate). Calculate the pH of the budder and he Ka for HC2H3O2 IS 1.8 X 10-5 Calculate the pH of te solution above after the addition of 0.0400 moles of solid NaOH. Assume no volume change upon the addition of base.
What is the pH of NH4C2H3O2 given information below? HC2H3O2⇌H+ + C2H3O2- Ka=1.76*10^-5 pKa=4.75 NH3+H2O⇌NH4+ + OH- Kb=1.79*10^-5 pKb=4.75 Assume initial concentration of NH4C2H3O2 is 0.100 M Use quadratic formula if necessary
Calculate the [H+] and the pH of a buffer solution that is 0.20 M in HC2H3O2 and contains sufficient sodium acetate to make the [C2H3O2-] equal to 0.20 M (Ka for HC2H3O2 = 1.8 x 10-5). (For scientific notation, enter your answer as follows: 1.0e-2 for 0.010)
In the titration of 50.00 mL of 1.00 M HC2H3O2 with 1.00 M NaOH, a student was considering using bromcresol as an indicator. Ka HC2H3O2 = 1.8 x 10-5 Kb for C2H3O2-1 = 5.6 x 10-10 (1)How many milliliters of NaOH would it take to reach the endpoint with this titration? (2)What is the pH of the solution at the end point? (2)What indicator would be a better choice than bromcresol green for this titration?
Now, for a complete equilibrium problem Consider the following general reaction: HC2H3O2 (aq) + H2O (l) ⇌ H3O+ (aq) + C2H3O2–(aq) Kc = 1.8 x 10–5 (at 25 ºC) If a solution initially contains (7.9x10^-1) M of HC2H3O2, (and no H3O+ or C2H3O2– ), what is the equilibrium concentration of H3O+ (aq) in the mixture? In the appropriate blanks, provide the equilibrium [H3O+ (aq)], in the solution, in M, to two significant figures and to the appropriate power
CHEM 1151K Make-up HW 3 22. What is the pH of a buffer prepared with 1.0 M HC2H302 and 1.0 M C2H3O2? The Ka for acetic acid, HC2H3O2, is 1.8 × 10-5. HC2H3O2(aq) + H2O(/) CHAD-(aq) + H3O+(aq)
6. b) A student mixes 8.203 g of NaC2H3O2 with 100 mL of 1.0 M HC2H3O2, what is the pH of the buffer? (4 pts) b) If you add 5.0 mL of 0.5 M NaOH solution to 20.0 mL to the buffer above, what is the pH of the resulting solution? (4 pts)
Unit 10 8. What is the pH of a 1.0 L buffer that consists of 00750 MC,H,NH, and 0,0500 MC,HNH,Cl after the addition of 10.0 mL of 0.5 M HCl? a. Calculate moles of C,H,NH., C,H,NH,Cl, and HC b. Write a reaction of the HCl with the appropriate other species c. Set up a reaction table (will use moles and stoichiometry) using the reaction as a header. +Cl-(aq) Before Reacts After d. Looking at your "After" line, use that information...
Which of the following is most acidic? A. A solution with [H,0+] = 1.0 x 10-10 B. A solution with [H,0+] = 1.0 x 10-5 C. A solution with [OH-] = 1.0 x 10-10 D. A solution with [OH-] = 1.0 x 10-5 E. A solution with a pH of 5. Question 5 Which of the following is most basic? A. CA solution with [H,0+] = 1.0 x 10-10 B. A solution with [H0+] = 1.0 x 10-5 C. A...