The following information and reaction equation will be used for the folliowing problems. A 120 mL...
The following information and reaction equation will be used for the folliowing problems.
A 120 mL solution of 0.110M acetic acid is going to be titrated with a series of additions of 0.100 M NaOH. (Acetic actic has a Ka= 1.8x10-5)
HC2H3O2 (aq) + H2O (aq) <-----> H3O+ (aq) + C2H3O2- (aq)
HC2H3O2 (aq) + NaOH (aq) <-----> H2O (aq) + NaC2H3O2 (aq)
a) What is the pH of the above system after 66 mL of the 0.100 M NaOH has been added? (correct answer 4.75)
b)What is the pH of the above system after 132 mL of the 0.100 NaOH has been added? (correct answer 8.43)
c) What is the pH of the above system after 160 mL of the 0.100 NaOH has been added? (correct answer 12.00)
Homework Answers
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The following information and
reaction equation will be used for the folliowing
problems.
A 120 mL...
2) 19.63 mL of 0.100 M NaOH is required to neutralize 2.00 mL of a solution containing acetic acid according to th...
2) 19.63 mL of 0.100 M NaOH is required to neutralize 2.00 mL of a solution containing acetic acid according to the following reaction: HC2H302(aq) + NaOH(aq) → NaC2H3O2(aq) + H2O(1). How many grams of acetic acid are present in 2 mL solution? Report the correct number of significant figures, and report the units. 3) 19.63 mL of 0.100 M NaOH is required to neutralize 2.00 mL of a solution containing acetic acid according to the following reaction: HC2H3O2(aq) +...
Important Info: Ka reaction: HC2H3O2(aq) + H2O(l) <-->C2H3O2 (aq) +H3O+(aq) HC2H3O(aq) +OH-(aq) -> C2H3O2-(aq) + H2O...
Important Info: Ka reaction: HC2H3O2(aq) + H2O(l) <-->C2H3O2 (aq) +H3O+(aq) HC2H3O(aq) +OH-(aq) -> C2H3O2-(aq) + H2O (l) A 1.0 L buffer solution is 0.280 M in HC2H302 (acetic acid) and 0.320 M in NaC2H302 (sodium acetate). Calculate the pH of the budder and he Ka for HC2H3O2 IS 1.8 X 10-5 Calculate the pH of te solution above after the addition of 0.0400 moles of solid NaOH. Assume no volume change upon the addition of base.
Calculate the pH of the acetate buffer after 28.00 mL 0.100 HCl has been added. 10...
Calculate the pH of the acetate buffer after 28.00 mL 0.100 HCl has been added. 10 mL of acetate buffer (Ka = 1.8 x 10^-5): 0.160 M NaC2H3O2 / 0.200 M HC2H3O2
You are instructed to create 180. mL of a 0.06 M Acetate buffer with a pH of 4.0. You have Acetic acid and the sodium sa...
You are instructed to create 180. mL of a 0.06 M Acetate buffer with a pH of 4.0. You have Acetic acid and the sodium salt NaC2H3O2, available. (Enter all numerical answers to three significant figures.) HC2H3O2(s) + H2O(l) equilibrium reaction H3O+(aq) + C2H3O2−(aq) Ka1 = 1.7 ✕ 10−5 What is the molarity needed for the base component of the buffer? How many moles of base are needed for the buffer? How many grams of base are needed for the...
1) Calculate the pH of the 1L buffer composed of 500 mL of 0.60 M acetic...
1) Calculate the pH of the 1L buffer composed of 500 mL of 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of HCl is added (Ka HC2H3O2 = 1.75 x 10-5). Report your answer to the hundredths place. 2) Calculate the pH of the 1L buffer composed of 500 mL 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of NaOH is added (Ka HC2H3O2 = 1.75...
I've been having some trouble with answering this portion of an Ionization of Acids lab that...
I've been having some trouble with answering this portion of an Ionization of Acids lab that I finished up last week and would REALLY appreciate some guidance/help: In this section of the experiment we were told to weigh out approximately ~0.5g and ~1.5g samples of anhydrous sodium acetate, then measure 50.0mL of 0.100M acetic acid into a 100mL beaker. From here we measured the pH of the solution, then dissolved the ~0.5g and measured the pH again, and finally one...
in an experiment, 5.00 mL 0.100 M acetic acid (Ka = 1.75 x 10^-5 at 25...
in an experiment, 5.00 mL 0.100 M acetic acid (Ka = 1.75 x 10^-5 at 25 C) was titrated with 0.100 M NaOH solution. The system will attain this pH after 10.0 mL of the titrant has been added
1. The equivalence point of a weak, monoprotic acid with a volume of 22.00 mL was...
1. The equivalence point of a weak, monoprotic acid with a volume of 22.00 mL was reached after adding 22.10 mL of 0.1025 M NaOH(aq) and the pH at this volume was 8.91. The pH was 3.37 when the volume of NaOH(aq) added was 11.05 mL. What is the value of Ka for this unknown acid? 0.1025 0.1030 3.37 8.91 1.23 x 10-9 4.27 x 10-4 2. A solution of acetic acid, HC2H3O2, a weak monoprotic acid, was standardized by...
A student titrated a 100.0 mL sample of 0.100 M acetic acid with 0.050 M NaOH....
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?
A 50.0 ml sample of 0.50 M acetic acid, ch3cooh is titrated with a 0.150 M...
A 50.0 ml sample of 0.50 M acetic acid, ch3cooh is titrated with a 0.150 M NaOH solution. calculate the ph after 25.0 ml of the base have been added (ka=1.8x10^-5)
2) 19.63 mL of 0.100 M NaOH is required to neutralize 2.00 mL of a solution containing acetic acid according to the following reaction: HC2H302(aq) + NaOH(aq) → NaC2H3O2(aq) + H2O(1). How many grams of acetic acid are present in 2 mL solution? Report the correct number of significant figures, and report the units. 3) 19.63 mL of 0.100 M NaOH is required to neutralize 2.00 mL of a solution containing acetic acid according to the following reaction: HC2H3O2(aq) +...
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