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 acid
a) 2.50 b) 4.01 c) 8.35 d) 7.00 e) None of the above
25) What is the pH in the titration above after 5.00 mL of 0.200 NaOH are added to the barbituric acid
a) 2.50 b) 4.01 c) 8.35 d) 7.00 e) None of the above
24. The pH of weak barbituric acid is given pH = 1/2(pKa+logC) = 1/2[-log(9.8*10^-5) -log(0.1)] = 2.50
25. Barbituric acid + NaOH ----------> sodium barbiturate + H2O
initial 2 mmoles 1 mmoles - -
after the reaction 1 mmlole o mmoles 1 mmole 1mmole
Now the mixture forms acidic buffer and its pH is given by pH = pKa + log(sodium barbiturate/Barbituric acid )
pKa= -log(Ka) =-log(9.8*10_5) = 4.008
pH = pKa + log(sodium barbiturate/Barbituric acid ) = 4.008+ log(1/1) = 4.008 4.01
23. (e) None of the above. Acetic acid is weak acid, sodium acetate is just a salt and
sodium hydroxide is a strong base.
24 (a) 2.50
25 (b) 4.01
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 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
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 buffer is prepared by mixing 200.0 mL of 0.1500 M NaOH with 200.0 mL of 0.200 M Benzoic Acid (a monoprotic carboxylic acid) in a 1-L volumetric flask and then diluted to volume with distilled deionized water. Calculate the pH of the buffer. Ka= 6.28 × 10−5and pKa= 4.01. A. 3.53 B. 4.01 C. 4.49 D. 7.00 E. 11.49
What is the pH of the solution obtained by mixing 30.00 mL of 0.250 M HCl and 30.00 mL of 0.125 M NaOH? We assume additive volumes. What is the pH of a solution that is 0.75 M in sodium acetate and 0.50 M in acetic acid? (ka for acetic acid is 1.3x10-5.) Calculate the pH of a solution prepared by mixing 15.00 ml of 0.10 M NaOH and 30.00 mL of 0.10 M benzoic acid solution. (Benzoic acid is monoprotic; its...
Please can I have step by step The pH of a solution prepared by mixing 50.0 mL of 0.125 M KOH and 50.0 mL of 0.125 M HCl is __________. Answer 7.00 A 25.0 mL sample of an acetic acid solution is titrated with a 0.175 M NaOH solution. The equivalence point is reached when 37.5 mL of the base is added. The concentration of acetic acid is __________ M. Answer 0.263
Calculate (to two decimal places) the final pH of the solution obtained by mixing 5.00 mL of 2.50 M NaOH with 650 mL of 300 mM acetate buffer that is initially at pH = 5.00. For acetic acid pKa = 4.76.
What is the pH of a buffer solution prepared by mixing 30.0 mL of 0.10 M of HOAC and 40.0 mL of a 0.1 M NaOAc Pka of the acid is 4.74
2. What is the "What is the pH of the solution obtained by mixing 30.00 mL of 0.250 M HCl and 30.00 mL of 0.125 M NaOH? We assume additive volumes. 3. What is the pH of a solution that is 0.75 M in sodium acetate and 0.50 M in acetic acid? (K, for acetic acid is 1.8x10-5.)
a solution is prepared by mixing 2.50 g of acetic acid (CH3CO2H, FW=60g/mol, Ka=1.75x10^(-5) with 4.70 g of sodium acetate (CH3CO2Na, FW=82g/mol) and adding water to a 500 mL volume. Note that sodium acetate yields Na+ and CH3COO-, the conjugate base of acetic acid. a.) what is the pH? b.) 15mL of 0.50 M HCl were added to the 500 mL solution, what is the pH after addituon of acid? write answer to 3 sig. figured.