What must be the concentration of CH3COO- ion in 0.40 M CH3COOH to produce a buffer solution with pH = 4.80? (Ka CH3COOH = 1.8 × 10-5)
What must be the concentration of CH3COO- ion in 0.40 M CH3COOH to produce a buffer...
6. If the pH of a CH3COOH/CH3COO- buffer system is 4.5, what is the acetate concentration if the acetic acid concentration is 0.44 and the dissociation constant, Ka, of CH3COOH is 1.6 x 10-8 ?
If the hydroxide concentration of a CH3COOH/CH3COO- buffer system is 0.000045 M, what is the acetate concentration if the acetic acid concentration is 0.74 and the dissociation constant, Ka, of CH3COOH is 6 x 10-9 ? A hot piece of metal at 450K is placed in pure water that has a volume of 55.0 mL which has an initial temperature of 25.3°C. After five minutes, equilibrium is established and a final temperature of 44.4°C is reached . What is the...
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
5. Calculate the grams of NaCH3COO required for 100.0 mL of 0.20 M CH3COOH solution to achieve a pH of 4.40. (Assume no volume change.) K = 1.8 x 10-5 6. What is the pH of 100.0 mL of buffer consisting of 0.20 M CH3COOH/0.20 M NaCH3COO after 10.0 mL of 0.20 M HC1 was added into the solution ? Kg = 1.8 x 10-5 7. The pH of a sodium acetate-acetic acid buffer is 4.80. Calculate the ratio of...
6. If the pH of a CH3COOH/CH3COO buffer system is 4.5, what is the acetate concentration if the acetic acid concentration is 0.44 and the dissociation constant, Ka, of CH3COOH is 1.6 x 10-%? 7. A 23.3 g hot piece of metal at 350K is placed in pure water that has a volume of 55.0. The metal is placed in the water and after five minutes, equilibrium is established where the final temperature of the metal reaches 99.8°C. What is...
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
1. What is the pH of a buffer consisting of 0.30 M CH3COOH & 0.20 M NACH:COO? Ka= 1.8 x 10-5 2. What is the pH of the buffer with 0.10 M NH3 and 0.20 M NH4NO3? Kl = 1.8 x 10-5 3. What is the pH of a buffer formed from combining 10 mL of 0.250 M HCl with 90 mL of 0.150 M NH3? (K = 1.8 x 10-) 4. Calculate the pH of the solution that results...
Calculate the pH of a buffer solution containing 0.100 M CH3COOH and 0.100 M CH3COONa ; Ka of CH3COOH = 1.8 x 10-5
Which of the following pH values are within the buffer range for a buffer containing 0.5 M CH3COOH and 0.5 M CH3COONa? The Ka for CH3COO– is 1.8×10–5. Select any answers that apply. Multiple tries are permitted; however, 25% (1/4) point will be deducted for each incorrect response. Select one or more: 2.76 5.09 0.57 3.81 8.11
The following equilibrium is established in water solution: CH3COOH + H20 = CH3COO +H30+ K a = 1.8 x 10-5 Which of the following is false? a H20 is a weak base. b.H20 is the conjugate base of H30*. CH3COOH is a weak acid. O هنا Hydroxide concentration is negligible with respect to hydrogen ion concentration. e. CH3COO is the conjugate acid of CH3COOH.