What would the concentration of CH3COO- be at pH 5.3 if 0.1M CH3COOH was adjusted to that pH (pK = 4.76)?
What would the concentration of CH3COO- be at pH 5.3 if 0.1M CH3COOH was adjusted to...
What would be the correct buffered pH range of the following buffer system CH3COOH(aq) +CH3COO(aq) + Haq) ; pK, = 4.76 O 9.76 - 11.76 0 4.76-6.76 O 3.76-5.76 O 2.76 -4.76
Which of the following statements is TRUE? At pH = 9, [CH3COOH] would be a lot lower than [CH3COO-] At pH = 2, [CH3COO-] would be dominant, compared to [CH3COOH] The ratio of concentration of acetate to acetic acid in a solution would go up as pH goes down. At pH = 4.76, [CH3COO-] = 2 * [CH3COOH]
What is the pH, amount of CH3COO- and CH3COOH in mol of a buffer synthesized from 10mL of 0.1M CH3COONa and 2.0mL of 0.1M HCl?
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
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 ?
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)
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...
Calculate the MOLES of HA (CH3COOH) and MOLES of A- (CH3COO-) present in the solution. Remember, you started with 50.0 mL of 1.0 M solution for each • The pKa of CH3COOH is 4.76. Use this information with the moles of acid and moles of base to calculate the pH of this solution. Stockroom Information Name: 1M CH3COOH Volume: 50.000 mL Species (aq) Molarity 0.00417456 1M CH3COOH 50.000 mL @ 25.0°C H+ OH 2.41858e-12 0.995825 CH3COOH CH3COO 0.00417456 Temperature: 25.00°C...
A buffer at pH of 4.35 contains CH3COOH at a concentration of 0.60 M and CH3COONa at a concentration of 0.30 M. What will be the pH when 75.8 mL of 0.980 M NaOH is added to 450.4 mL of the buffer? The pKa of CH3COOH is 4.76 dlace of
What is the pH of a solution containing 0.342 mol L-1 CH3COOH and 0.428 CH3COO- mol L-1 ? Round your answer to 2 decimal places.