please show work 20) Determine the pH of a 0.10 M NaCH3O2. For acetic acid, Ka...
20) Determine the pH of a 0.10 M NaC2H302. For acetic acid, Ka = 1.8 x 10-5. A) 4.18 B) 5.29 C) 7.33 D) 8.87
25 mL of 0.10 M acetic acid is titrated with 0.10 M NaOH. What is the pH after 30 ml of NaOH have been added? Ka for acetic acid = 1.8 x 10^-5.
The Ka for acetic acid, CH3COOH, is 1.8 × 10-5. A buffer, made from 0.10 M CH3COOH and 0.10 M CH3COO- has a pH of ________. a. 4.74 b. 14.00 c. 1.00 d. 9.26 e. 7.00
I need help with #4. "show by calculation why acetic acid (Ka = 1.8 X 10^-5), when combined with NaC2H3O3 as a buffer, will not produce a pH o 9.00" 1. What is the pH of a 1.0L buffer that is 0.10 M in Naz HPO4 and 0.15 M in NaH2PO4? Write the equilibrium reaction equation and corresponding Ka expression for the buffer. K for H2PO4 is 6.2 X 108 2. A 10.00 mL sample of 0.300 M NH3 is...
(Please show work) A 100.0 mLbuffer solution is 0.250 M in acetic acid (CH3COOH) and 0.250 M in sodium acetate (CH3COONa). [Acetic Acid (CH3COOH) Ka = 1.8 x 10-5] a)What is the pH of this buffer solution? b)What is the pH after addition of 0.0050 mol of HCl? c)What is the pH after addition of 0.0050 mol of NaOH?
4. Please calculate the resulting pH when 25 mL of 0.10 M acetic acid is titrated with 10 mL of 0.10 M NaOH (K. acetic acid = 1.8 x 10-5): CH,COOH (aq) + NaOH(aq) → CH3COONa (aq) + H20 (1)
Calculate the pH, the percent dissociation, and the concentration of OH- in 0.10 M of Acetic Acid solution (HC2H3O2) (Ka = 1.8 x 10^-5) (Kw = 1.0 x 10^-14)
Calculate the pH of a solution containing 0.10 mole of acetic acid, to which is added 0.03 mole of sodium hydroxide (Ka = 1.8 x 10-5).
Consider a titration of 250 mL 0.15 M acetic acid (Ka = 1.8 x10-5) with 0.10 M KOH. What is the pH of the acetic acid solution (ie: before the titration has begun?) What is the pH after adding 25 mL of 0.10 M KOH? What is the volume of base needed to reach the equivalence point? Is the pH at equivalence point acidic, basic, or exactly neutral? What is the pH after 500 mL of KOH has been added?
Determine the pH during the titration of 29.5 mL of 0.324 M acetic acid (Ka = 1.8×10-5) by 0.414 M NaOH at the following points. (a) Before the addition of any NaOH ________ (b) After the addition of 5.70 mL of NaOH _______ (c) At the half-equivalence point (the titration midpoint) _______ (d) At the equivalence point _______ (e) After the addition of 34.6 mL of NaOH ________