CHEM107 ACID_BASE BUFFERS AND PH UNIT-25 CTO-13: You have 500.0 mL of a buffer solution containing...
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N Le 2.30u is. You have 500.0 mL of a buffer solution containing 0.30 M acetic acid (CH2COOH) and 0.25 M sodium acetate (CH,COONa). What will the pH of this solution be after the addition of 20.0 mL of 1.00 M NaOH solution? [K,= 1.8 x 10-51 DKA - 109( 1.8x10-5) -4.74 a. 4.88 4.74 +log .30 = 4.8 b. 4.74 c. 4.67 d. 4.79 4.8 X e. 4.54 25
D. Buffers 1. A buffer solution was made by dissolving 10.0 grams of sodium acetate in 200.0 mL of 1.50 M acetic acid. Assuming the change in volume when the sodium acetate is added is not significant, estimate the pH of the acetic acid/sodium acetate buffer solution. The K, for acetic acid is 1.8 x 105. 2. Calculate the pH of a buffer solution that initially consists of 0.0400 moles of ammonia and 0.0250 moles of ammonium ion, after 20.0...
Determine the pH of a buffer formed by dissolving 20.0 g NaCH3COO into a 500.0 mL solution of 0.150 M of CH3COOH. Assume the volume of the solution does not change. The value for Ka for CH3COOH is 1.8 *10 ^-4 set up the ICE table in order to determine the unknown. (Set up the ICE table please).
7) Which one of the following is the weakest acid? A) HF (Ka = 6.8 × 10-4) B) HClO (Ka = 3.0 × 10-8) C) HNO2 (Ka = 4.5 × 10-4) D) HCN (Ka = 4.9 × 10-10) B) 5.7 x 10–2 M D) 2.9 x 10–3 M 22) Calculate the hydrogen ion concentration in a solution of iced tea with lemon having a pH of 2.87. A) 2.9x10–2M D) 2.9x10–3M B) 5.7 x 10–2 M E) 5.7 x 10–4...
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
A buffer formed from 20.0 mL of 0.120 M Acetic acid (CH3COOH) (pKa = 4.74) and 12.0 mL of 0.200 M sodium acetate (CH3COONa). What is the pH of this buffer after addition of 0.0001 mol of HCl?
Calculate the following: a. The pH of a 500.0 mL buffer solution containing 0.75 M HCN (Ka = 6.2 x 10^-10) and 0.55 M NaCN b. The pH of the above buffer after the addition of 100.0 mL of 1.0 M NaOH. c. The pH of the buffer if 100.0 mL of 1.0 M HCl was added to the solution in part a.
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...
You are to prepare a pH 3.50 buffer and you have 0.10M solution. HCOOH Ka= 1.8x10-4 CH3COOH Ka= 1.8x10-5 HCOONa CH3COONa How much of each solution would you need to prepare 500.0 mL of the buffer at the required pH?
A buffer solution is prepared by dissolving 1.000 g of sodium acetate (CH3COONa) into 100.00 mL of a 0.100 M solution of acetic acid. Then 2.00 mL of a 1.00 M solution of hydrochloric acid is added to the acetic acid/sodium acetate buffer solution. The Ka of acetic acid is 1.8 × 10−5. What is the pH of HCl?