A solution is prepared by mixing 20.0 mL of 0.050 M acetic acid and 10.0 mL of 0.100 M HCl. What is the pH of the solution? ( Ka acetic acid = 1.8 x 10-5)
A. 2.36
B. 0.22
C. 1.48
D. 1.00
E. 0.48
A solution is prepared by mixing 20.0 mL of 0.050 M acetic acid and 10.0 mL...
What is the pH of a solution prepared by mixing 25.0 mL of 0.100 M benzoic acid and 50.0 mL of 0.050 M KOH ? (Ka benzoic acid = 6.4 x 10-5) A. 8.36 B. 5.19 C. 8.81 D. 9.04 E. 5.64
1. Calculate the pH of a buffer solution prepared by mixing 0.250 L of 0.150 M acetic acid with 0.200 L of 0.250 M sodium acetate. Ka acetic acid = 1.8 x 10-5 Calculate the pH of this solution of after the addition of 0.003 L of 0.200 M HCL 2. Consider a buffer solution prepared by mixing 0.250 L of 0.150 M acetic acid with 0.200 L of 0.250 M sodium acetate. Ka acetic acid = 1.8 x 10-5...
A 20.0 mL sample of a 0.0875 M solution of acetic acid, CH3COOH, is titrated with a 0.115 M solution of KOH. What is the pH after 20.0 mL of KOH solution have been added? For CH3COOH, Ka=1.8 x 10–5.
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?
A student titrated a 100.0 mL sample of 0.100 M acetic acid with 0.050 M NaOH. (For acetic acid, Ka = 1.8 * 10^-5 at this temperature.) (a) Calculate the initial pH. (b) Calculate the pH after 50.0 mL of NaOH has been added. (c) Determine the volume of added base required to reach the equivalence point. (d) Determine the pH at the equivalence point?
What is the pH of a solution prepared by mixing: 0.30 moles of acetic acid (Ka = 1.8 X 10-5) 0.15 moles of sodium hydroxide in 1.0 L of solution A. 4.44 B. 13.18 C. none of the above D. 0.82 E. 4.74
What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH3COOH with 25.00 mL of 0.050 M CH3COONa? Assume that the volume of the solutions are additive and that Ka = 1.8 x 10-5 for CH3COOH.
23) What is the pH of a solution prepared by mixing: 0.20 moles of acetic acid 0.40 moles of sodium acetate 0.10 moles of sodium hydroxide in 1.0 L of solution a) 4.74 b) 4.14 5.34 d) 13.00 e) None of the above 24) Barbituric acid (Ka = 9.8 X 10-5) is titrated with 0.200 M NaOH. What is the initial pH of 20.0 mL of 0.100 barbituric acida) 2.50 b) 4.01 c) 8.35 d) 7.00 e) None of the above 25) What is the pH in...
A solution is prepared by dissolving 0.23 mol of formic acid and 0.27 mol of sodium formate in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of NaOH to this buffer solution causes the pH to increase slightly. The pH does not increase drastically because the NaOH reacts with the present in the buffer solution. The K, of formic acid is 1.8 x 10+ A formic acid B. sodium formate C water D. sodium E....
What is the pH of a solution obtained by mixing: 10.0 mL of 2.00 M hydrofluoric acid (HF) solution and 20.0 mL of 1.00 M hydrochloric acid (HCI) solution The Ka of hydrofluoric acid (HF) is 6.6 X 104 Show all of your work, give a final answer with the correct amount of significant figures. Correct answer is (0.176)