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explain every step please Question 2 The pH of 0.10 M of an unknown acid is...
2. (a) Determine the pH of 0.10 M lactic acid (HC3HSO3) (b) What is the pH of a buffer that is 0.12 M. lactic acid and 0.10 M sodium lactate (NaC3H5O3)? For lactic acid. Ka = 1.4 x 10-4. (10)
Find the pH of a solution prepared by adding 1.0 L of 0.10 M butyric acid to 0.50 L of 0.10 M NaOH. (Ka = 1.5 x 10-5) A. 12.69 B. 7.00 C. 2.41 D. 4.82 E. 13.35
Calculate the pH at the isoelectric point for a 0.10 M solution of the amino acid phenylanaline. Ka(-CO2H) = 6.30 x 10^-3 and Ka(-NH3) = 4.0 x 10^-10 for phenylalanine.
Calculate the pH, the percent dissociation, and the concentration of OH- in 0.10 M of Acetic Acid solution (HC2H3O2) (Ka = 1.8 x 10^-5) (Kw = 1.0 x 10^-14)
QUESTION 7 You are given an unknown acid solution with a pH of 2.24 and a concentration of 0.500 M. What is the Ka of this unknown acid? Note: "*" and "x" for this are negligible. No quadratic. 3.9 x 10-6 1.1 x 10-2 7.AX 10-6 6.6 x 10-5 9.1 x 103 7.1 x 10-9
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20) Determine the pH of a 0.10 M NaCH3O2. For acetic acid, Ka - 1.8 x 10-5 A) 4.18 NaczH30₂ + H₂O NaG2 H₂O₂ + H₂O B) 5.29 C) 7.33 1-8X105X7 0.10 D) 8.87 0.1-xc -X X=0.00134 € 0.1-8.
The pH of a 0.10 M solution of hydrazoic acid, HN3, is 2.86. Calculate the Ka value for hydrazoic acid. A. 1.4 x 10-4 B. 1.9 x 10-5 C. 1.9 x 10-3 D. 1.4 x 10-5 E. 2.6 x 10-3
Calculate the pH of the following solutions: 50.0 mL 0.10 M acetic acid + 1.0 mL 1.0 M HCl 50.0 mL 0.10 M acetic acid + 1.0 mL 1.0 M NaOH 50.0 mL 0.10 M sodium acetate + 1.0 mL 1.0 M HCl 50.0 mL 0.10 M sodium acetate + 1.0 mL 1.0 M NaOH 50.0 mL 0.10 M acetic acid/sodium acetate buffer 50.0 mL 0.10 M acetic acid/sodium acetate buffer + 1.0 mL 1.0 M HCl 50.0 mL 0.10...
2. What is the pH of a buffer solution that is 0.10 M Benzoic acid, HC.HO, and 0.15 M sodium benzoate. Ka = 6.6 x 10% Page 1
Calculate the pH of a solution of 0.10 M hydrogen cyanide HCN? (Ka = 4.9 x 10-10) The answer is 5.15 please explain.