Solid NaOH is added to a solution of 0.50 M acetic acid until the pH of...
Solid NaOH is added to a solution of 0.50 M acetic acid until the pH of the solution is 4.30. The resulting concentration (M) of sodium acetate in the solution is Ka (CH3COOH) = 1.8 x 10-5
- A.
0.020
- B.
0.13
- C.
0.30
- D.
5.0 x 10-5
-
E. 0.50
Homework Answers
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Solid NaOH is added to a solution of 0.50 M acetic acid until
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QUESTION 9 The pH of 0.50 M acetic acid is 2.52. Calculate the change in pH when 0.91 g of CH3COONa (FW - 82.03 g/mol) is added to 11.1 mL of 0.50 M acetic acid. CH3COOH. Ignore any changes in volume. The Ka value for CH3COOH is 1.8 x 10-5
(Please show work) A 100.0 mLbuffer solution is 0.250 M in acetic acid (CH3COOH) and 0.250...
(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?
Calculate the pH of a 0.50 M solution of sodium acetate (NaCH3COO) given that the Ka...
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Q: What is the pH of a solution containing 0.125 M KH2PO4 and 0.175 K2HPO4 Ka (H2PO4-) = 6.2 x 10-8 Ka (HPO42-) = 4.8 x 10-13 Q: A 0.15 M solution of a weak acid is 3.0 % dissociated. What is the Ka of this acid? Q: A solution of aspirin was prepared that is 0.16 M. The pH of this solution was measured to be 2.43. What is the Ka of aspirin? Q: A solution of formic acid...
40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 M NaOH. After...
40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 M NaOH. After 20.0 mL of the base solution has been added, the pH in the titration flask is 5.10. What was the concentration of the original acetic acid solution? [Ka(CH3COOH) = 1.8 × 10–5]
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a) A 50.0 mL solution of 0.200 M acetic acid (CH3COOH), 50.0 mL of 0.200 M is titrated with 0.200 M NaOH. Determine the pH.of acetic acid before any NaOH is added. The Ka of CH3COOH is 1.8 x 10-5. b) Determine the pH of the solution at the equivalent point.
A buffer solution is 0.78 M in acetic acid and 0.22 M in sodium acetate. Calculate...
A buffer solution is 0.78 M in acetic acid and 0.22 M in sodium acetate. Calculate the solution pH after adding 0.80 g of solid NaOH to 100.0 mL of the buffer solution. Ka of acetic acid is 1.8 10−5 . Assume negligible volume change.
hi there! please solve and show all work :) A buffered solution contains 0.50 M acetic...
hi there! please solve and show all work :)
A buffered solution contains 0.50 M acetic acid (HC2H302, K = 1.8 x10-5) and 0.50 M sodium acetate (NaC2H302)- "15pts) Calculate the pH of the solution: Calculate the pH after adding 0.020 mol NaOH into 1.00L of the buffer solution: m (base )
QUESTION 9 The pH of 0.50 M acetic acid is 2.52. Calculate the change in pH when 0.91 g of CH3COONa (FW - 82.03 g/mol) is added to 11.1 mL of 0.50 M acetic acid. CH3COOH. Ignore any changes in volume. The Ka value for CH3COOH is 1.8 x 10-5
Calculate the pH of a 0.50 M solution of sodium acetate (NaCH3COO) given that the Ka of acetic acid (CH3COOH) is 1.8 x 105, A 9.26 B.9.22 11.48 D.4.78 E. 2.52
hi there! please solve and show all work :)
A buffered solution contains 0.50 M acetic acid (HC2H302, K = 1.8 x10-5) and 0.50 M sodium acetate (NaC2H302)- "15pts) Calculate the pH of the solution: Calculate the pH after adding 0.020 mol NaOH into 1.00L of the buffer solution: m (base )
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