what is the ph of a buffer that contains 0.15 m ch3cooh and 0.10 m nach3coo (ka=1.8x10-5)? a. 4.74 b. 7.00 c. 4.57 d.4.92
what is the ph of a buffer that contains 0.15 m ch3cooh and 0.10 m nach3coo...
please solve and show work! A buffer contains 0.50 M CH3COOH (acetic acid) and 0.50 M CH3COONa (sodium acetate). The pH of the buffer is 4.74. What is the pH after 0.10 mol of HCI is added to 1.00 liter of this buffer? A.5.57 B.4.74 C.4.38 D. 4.92 E.4.57
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
consider 100.0 ml of a buffer solution that contains [NaCH3COO]=[CH3COOH]=0.250 M a) what is the pH of this buffer? b) what should the ph of the buffer be after 50.0ml of water is added? explain c) wtite balanced net ionic for the reaction that occurs whrn 1.0 M HCl ir added to this buffer. d) after adding 10.0 ml of 1.0 M HCl what will the ph of the solution be? e) as more 1.0 M HCl is slowly added...
What is the pH of a 0.402 M aqueous solution of NaCH3COO? Ka (CH3COOH) = 1.8x10-5
calculate the ph of a buffer solution that contains 1.5 M acetic acid (CH3COOH) and 0.3 M sodium acetate (CH3COONa) [Ka=1.8x10-5 for acetic acid]
To prepare 1.0 L of a buffer that is 0.10 M CH3COOH and 0.10 M CH3COo, you can i. Add 0.10 mol of NaCH3COO (8.20 g NaCH3COO) to 1 L of 0.10 M CH3COOH ii. Add 0.10 mol of NaOH (4.00 g NaOH) to 1 Lof 0.20 M CH3COOH ili. Add 0.20 mol NaCH3COO (28.7 g NaCH3COO) to 1 L of 0.10 M HOI A. Only i B. Only ii C. Only ii D. i, ii, and ii
i already know they answer please explain your solutions Ka for CH3COOH = 1.8x10^-5 pka i calculated 4.74 ID: A fer- a solut monione blir rw Name: was 11. If 0.40 g of solid NaOH is added to 1.0 liter of a buffer solution that is 0.10 Min CH,COOH and 0.10 Min NaCH,COO, how will the pH of the solution change? a. The pH increases from 4.74 to 4.83. b. The pH decreases from 7.00 to 4.83. c. The pH...
DA -. What is the pH of a buffer that contains 0.15 M CH,CUUH and 0.10 M NaCH.COO (K = 1.8 x 10°)?
1) What is the pH of a solution in which 25 mL of 0.10 M NaOH is added to 15 mL of 0.10 M HCl? 2) If you add 2.50 mL of 0.150 M HCl to 100 mL of a buffer consisting of 0.100 M CH3COOH and 0.200 M CH3COONa, what will be the change in pH? (Ka of CH3COOH is 1.8x10^-5)
what concentrations of CH3COO- and CH3COOH of those below would give a buffer with a pH of 4.11 (pKa= CH3COOH=4.84) Br What concentrations of [CH3COO 1 and [CH1COOH1 of those below would give a buffer with a pH of 4.11? (pKa CH3COOH = 4.84). 10 a) (CH3COO]-0.15 M, [CH3COOH] = 0.10 M b) [CH3COO]-0.10 M, [CH3COOH] = 0.53 M c) [CH3COO]-0.46 M, [CH3COOH]= 0.10 M d) [CH3COO]- 0.23 M, [CH3COOH] = 0.10 M 14