# A 35.0 mL sample of 0.150 M acetic acid is titrated with 0.150 M NaOH solution. Calculate the pH after the following volumes of base have been added: a) 0mL, b) 17.5 mL, c) 34.5 mL, d) 35 mL I've

43,451 results
1. ## water chemistry

35.0 mL sample of 0.150 M acetic acid (HC2H3O2) (Ka = 1.8 x 10-5) is titrated with 0.150 M NaOH solution. Calculate the pH after 17.5 mL volumes of base have been added
2. ## Chemistry

A 35.0 mL sample of 0.150 M acetic acid is titrated with 0.150 M NaOH solution. Calculate the pH after the following volumes of base have been added: a) 0mL, b) 17.5 mL, c) 34.5 mL, d) 35 mL I've figured out a,b, and c. But at 35 mL the moles become equal
3. ## Chemistry

A 20.0-mL sample of 0.300 M HBr is titrated with 0.150 M NaOH. What is the pH of the solution after 40.3 mL of NaOH have been added to the acid?
4. ## Chemistry

A sample of 25.00 mL of vinegar is titrated with a standard 1.02 M NaOH solution. It was found that a volume of 19.60 mL of the standard NaOH solution is used to completely neutralize the acetic acid in the solution. Calculate the concentration of the
5. ## Chemistry

In this experiment NaOH is standardized to find out the percent by mass of the acetic acid in a sample of vinegar. A student had not allowed the NaOH pellets to dissolve completely before standardizing it with KHP, but when the student refilled the buret
6. ## Chemistry

A 0.150 M solution of nitrous acid (HNO2) is made. Ka = 4.5 x 10-4 1. Show the equilibrium which occurs when this acid is dissolved in water. 2. What is the pH of the solution? Show all work clearly. 3. 100.0 mL of the solution is titrated against 0.150 M
7. ## Chemistry

A 0.150 M solution of nitrous acid (HNO2) is made. Ka = 4.5 x 10-4 1. Show the equilibrium which occurs when this acid is dissolved in water. 2. What is the pH of the solution? Show all work clearly. 3. 100.0 mL of the solution is titrated against 0.150 M
8. ## Chem

Please tell me if these are right! 1.How many milliliters of 0.215 M NaOH solution are needed to completely neutralize 2.50 ml of 0.825 M H2SO4 solution? I got 19.2 ml 2. A 10.0-ml sample of vinegar which is an aqueous solution of acetic acid HC2G3O2
9. ## chem help w/ Lab

Weight of the mustard package Sample: 3.02 (g) Weight of the mustard package Solution: 33.3 (g) Trial #1 Trial #2 Trial #3 Weight of Mustard Package Solution Delivered (g) : 1.09 .948 .909 Weight of NaOH Solution Delivered (g) : .354 .304 .269
10. ## chemistry

19 mL of 0.50 mool/L NaOH which is standardized becomes titrated alongside 24 mL of 0.44 mol/L acetic acid. Determine the pH of the solution Please judge my work: Becasue NaOH and acetic acid react in a 1:1 ratio, initital moles of acetic acid =0.0019 L x
11. ## Chemistry

Commercial vinegar was titrated with NaOH solution to determine the content of acetic acid, HC2H3O2. For 20.0 milliliters of the vinegar 26.7 milliliters of 0.600-molar NaOH solution was required. What was the concentration of acetic acid in the vinegar if
12. ## Chemistry

A 25 mL sample of wine is found to have a concentration of acetic acid of 0.23 M. If this was titrated with a 0.16 M NaOH solution how many mL's of NaOH would be required?
13. ## Balthazar

A 30 ml sample of of 0.150 m hydrazoic acid (ka = 4.50x10^-4 ) is titrated with a 0.100 m NaOH what is the ph after the ff additions of NaOH 30ml 45ml 60ml
14. ## College Chemistry

1) A 25mL sample of the .265M HCI solution from the previous question is titrated with a solution of NaOH. 28.25mL of the NaOH solution is required to titrate the HCl. Calculate the molarity of the NaOH solution. 2) A 1.12g sample of an unknown monoprotic
15. ## Chemistry

Question: A 0.400 g sample of propionic acid was dissolved in water to give 50.00 mL of solution. This solution was titrated with 0.150 M NaOH. what was the pH of the solution when the equivalence point was reached? I'm not really sure how i would go about
16. ## General Chemistry

"How would you prepare 150. mL of 0.1M sodium hydroxide given a stock solution of 3.0M NaOH?" I made calculations and figured the process would be to dilute 5 mL of the 3.0M NaOH to 150. mL. Is this correct? For the ideal 150. mL of 0.1M NaOH, I calculated
17. ## chemistry

25.0g of 5.0% (by mass) acetic acid solution are titrated with 0.300 M NaOH. What volume of NaOH will be needed to neutralize this sample?
18. ## Chemistry

You are asked to prepare 500. mL of a 0.150 M acetate buffer at pH 5.00 using only pure acetic acid, 3.00 M NaOH, and water. Calculate the quantities needed for each of the following steps in the buffer preparation. 1. Add acetic acid to ~400 mL of water
19. ## chemistry

You were given 25.00 ml of an acetic acid solution of unknown concentration. You find that it requires 29.60 ml of a 0.1050 M NaOH solution to exaclty neutralize this sample. A) What is the molarity of the acetic acid solution? B) what is the percentage of
20. ## Chemistry

Pure acetic acid, known as glacial acetic acid, is a liquid with a density of 1.049 g/mL at 25°C. Calculate the molarity of a solution of acetic acid made by dissolving 10.00 mL of glacial acetic acid at 25°C in enough water to make 150.0 mL of solution.
21. ## chem-acid-base titrations

Acetic acid (HC2H3O2) is an important component of vinegar. A 10.00mL sample of vinegar is titrated with .5052 M NaOH, and 16.88 mL are required to neutralize the acetic acid that is present. a.write a balanced equation for this neutralization reaction
22. ## chemistry

a sample of 20.0 mL of 0.100 M HCN (Ka=6.2*10^-10) is titrated with 0.150 M NaOH. a) what volume of NaOH is used in this titration to reach the equivalence point? b) What is the molar concentration of CN- at the equivalence point? c) What is the pH of the
23. ## Chemistry

Consider a weak acid-strong base titration in which 25.0 mL of 0.100 M acetic acid is titrated with 0.100 M NaOH. a) Calculate the pH after the addition of 3.00mL of NaOH. b) What is the pH of the solution before the addition of NaOH (pKa of acetic
24. ## Chemistry

a 30 mL sample of vinegar is titrated with .1098 M NaOH. it takes 43.28 mL naOH solution to reach the endpoint. Determine the acetic acid concentration in the vinegar solution?
25. ## chemistry

A 0.1 M solution of acetic acid is titrated with 0.05M solution of NaOH. What is the pH when 60% of the acid has been neutralized? The equilibrium constant (Ka) for acetic acid is 1.8x10^-5
26. ## organic chemistry

A solution of acetic acid (CH3COOH; Ka = 1.74 x 10-5) was titrated to a final pH of 4.76 by using NaOH solution. What % of acetic acid is converted to sodium acetate (CH3COO-Na+)? Show your method
27. ## CHEM 136

A sample of 25.00 mL of 0.100 M HNO2(in a flask) is titrated with 0.150 M of NaOH solution at 25 degrees. 1) calculate the volume(Ve) of the NaOH solution needed to completely neutralize the acid in the flask. 2)calculate the pH for (a)the initial acid
28. ## Chemistry

A 25.0mL sample of a 0.100M solution of acetic acid is titrated with a 0.125M solution of NaOH. Calculate the pH of the titration mixture after 10.0, 20.0, and 30.0 mL of base have been added.
29. ## chem.

A 10.0 mL of vinegar, an aqueous solution of acetic acid (HC2H3O2), is titrated with .5062M NaOH, and 16.58mL is required to reach the equivalence point. A. What is the molarity of the acetic acid? B. If the density of the vinegar is 1.006 g/cm^3, what is
30. ## chem equilibrium

Determine the pH of a buffer that is prepared by mixing 100 mL of 0.2 M NaOH and 150 mL of 0.4 M acetic acid assuming the volume is additive. Calculate the pH of the solution when 0.5 mL of 1 M of HCl was added hence calculate the buffer
31. ## chemistry

Lab: Determining Ka of Acetic Acid Purpose: The purpose of this experiment is to determine the molar concentration of a sample of acetic acid and to calculate its Ka. Materials: phenolphthalein 125 mL Erlenmeyer flask 25 mL pipet and bulb pH metre acetic
32. ## Chemistry

In this experiment NaOH is standardized to titrate it with vinegar so thtat the percent by mass of the acetic acid can be determined. How does dissolved CO2 in distilled water affect the accuracy of the determination of a NaOH solution's concentration? How
33. ## Analytical Chemistry

Suggest a range of sample masses for the indicated primary standard if it is desired to use between 35 and 45mL of titrant: (a) 0.175 M HClO4 titrated against Na2CO3(CO2 product) (b) 0.085 M HCl titrated against Na2C2O4 Na2C2O4-->Na2CO3+CO
34. ## chemistry

Acetic acid, CH3CO2H, is the active ingredient in vinegar. It's often abbreviated "HOAc". Vinegar is acidic because acetic acid makes H3O+ when it partially ionizes in water: HOAc(aq) + H2O H3O+(aq) + OAc–(aq) Suppose that you have a solution of
35. ## chemistry

A 12.6 mL sample of vinegar, containing acetic acid, was titrated using 0.542 M NaOH solution. The titration required 24.1 mL of the base. what is the molar concentration of acid in the vinegar?'
36. ## CHEM HELP ASAP

I figured all the parts of the problem except for the last one. Can you tell me what to do? In the preparation of a mustard solution, an individual package of mustard was emptied into a beaker and the mass was determined to be 3.809 grams. The mustard was
37. ## CHEM PROB MR BOB

I figured all the parts of the problem except for the last one. Can you tell me what to do? In the preparation of a mustard solution, an individual package of mustard was emptied into a beaker and the mass was determined to be 3.809 grams. The mustard was
38. ## CHEM HELP ASAP

I figured all the parts of the problem except for the last one. Can you tell me what to do? In the preparation of a mustard solution, an individual package of mustard was emptied into a beaker and the mass was determined to be 3.809 grams. The mustard was
39. ## Chemistry

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
40. ## Chemistry

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
41. ## Chemistry

I got pH = 5.3 A 1.00 L buffer solution is 0.250 M in HC2H3O2 and 0.250 M in NaC2H3O2. Calculate the pH of the solution after the addition of 0.150 mol of solid NaOH. Assume no volume change upon the Additon o f NaOH. The Ka value for HC2H3O2 at 25 C is
42. ## Chem Problem

I originally asked you the first question and I got the answer 7.7 but theres other parts to the problem but Im not sure what to do In the preparation of a mustard solution, an individual package of mustard was emptied into a beaker and the mass was
43. ## Chem Problem

I originally asked you the first question and I got the answer 7.7 but theres other parts to the problem but Im not sure what to do In the preparation of a mustard solution, an individual package of mustard was emptied into a beaker and the mass was
44. ## Chemistry- Dr.Bob222

What is the pH of a solution that is 0.150 M in acetic solution and 0.300 M in sodium acetate? The Ka of acetic acid is 1.8 x 10^-5. My work: pH= pKa + log (base/acid) pH= -log (1.8 x 10^-5) + log (0.300/0.150) pH=5
45. ## chemistry

10 ml sample of vinegar an aqueous solution 0f acetic acid( HC2H3O2) is titrated with 0.5062 M and 16.58 ml is required to reach equivalence point what is the molarity of the acetic acid b. if the density of vinegar is 1.006 g/cm3 what is the mass percent
46. ## chemistry

What is the molarity of the acetic acid if 0.5ml of a vinegar solution has been titrated with the 0.101M solution of NaOH and the volume of the NaOH solution at the equivalence point is 5.0mL?
47. ## Chem

What is the pH of the resulting solution if 30.00 mL of 0.100M acetic acid is added to 10.00mL of 0.100 M NaOH? For acetic acid, Ka=0.000018. I know that NaOH is a strong base and acetic acid is a weak acid. What is the equation: C6H5COOH+NaOH C6H5COOH
48. ## Chemistry

A 30 mL sample of 0.150 M KOH is titrated with 0.125 M HClO4 solution. Calculate the pH after the following volumes of acid have been added: 30 mL, 35 mL, 36 mL, 37 mL, and 40 mL.
49. ## Chemistry

A 30 mL sample of 0.150 M KOH is titrated with 0.125 M HClO4 solution. Calculate the pH after the following volumes of acid have been added: 30 mL, 35 mL, 36 mL, 37 mL, and 40 mL.
50. ## chemistry

My question is found in the analysis section. Thanks to all who can help Lab: Determining Ka of Acetic Acid Purpose: The purpose of this experiment is to determine the molar concentration of a sample of acetic acid and to calculate its Ka. Materials:
51. ## chemistry

If 3.30 mL of vinegar needs 42.5 mL of 0.150 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.50 qt sample of this vinegar?
52. ## chemistry

3.30 mL of vinegar needs 43.0 mL of 0.150 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.70 qt sample of this vinegar?
53. ## science

25 ml sample of 0.150 m solution of aqueous trimethylamine is titrated with 0.100 M soultion of hcl. calculate the pH of the solution after 10.0ml,20 ml and 30.0 ml of acid have been added; pkb of (CH3)3 N =4.19?
54. ## chemistry

A 10.0-mL sample of vinegar, which is an aqueous solution of acetic acid, CH3COOH, requires 16.5 XML of a 0.500M NaOH solution to reach the endpoint in a titration (where the moles of acid are equal to the moles of base). What is the molarity of the acetic
55. ## Chemistry

A 10.0 ml sample of vinegar which is an aqueous solution of acetic acid, requires 16.5ml of a 0.500M NaOH solution to reach the endpoint in a titration (where the moles of acid are equal to the moles of base). What is the molarity of the acetic acid
56. ## Physical chemistry 2

50 ml of 0.02M acetic acid is titrated with 0.1M NaOH.Calculate the pH of the solution when 10ml of NaOH is added
57. ## chemistry II

What is the molarity of a solution of acetic acid if 35.00mL is titrated to the end point with 68.20ml of 0.750M KOH? What is the percentage by mass of acetic acid solution? The density of acetic acid is 1.06 g/ml
58. ## Chem

what volume of acetic acid must be added to 150.0 mL of water to generate a 15.0% acetic acid solution? I just need help on how to solve it please!:)
59. ## chemistry

Methanoic acid HCO2H(aq) also known as formic acid, is partly responsible for the characterisitic itchy rash produced by the leaves of the stinging nettle plant. Calculate the pH of 0.150 mol/L methanoic acid. The Ka for methanoic acid is 1.8 x 10^-4. My
60. ## chem

a 50ml aliquot sample of vinegar is titrated with a 0.078 M NaOH sol'n. The phenolpthalein end point was reached after the addition of 35.6 ml. Equation: HC2H3O2 + NaOH _____> NaC2H3O2 + H20 Calculate the % by mass/vol. of acetic acid in the sample.
61. ## College Chemistry

I need help with this question!! a sample of pure KHP weighing .8097g dissolved in water and titrated with 40.25 mL of NaOH solution. The same NaOH solution was used to titrate a solution of a weak diprotic acid H2X. A sample of 0.18694g of the weak acid
62. ## Chemistry

A buffer is made by mixing 100 mL of 0.25 M acetic acid (CH3COOH) and 150 mL of 0.10 M sodium acetate (CH3COONa). Calculate the pH of the solution after 0.5g of solid NaOH is added to the solution (Given Ka (CH3COOH) =1.8 x 10-5)
63. ## chemistry

Lab: Determining Ka of Acetic Acid Purpose: The purpose of this experiment is to determine the molar concentration of a sample of acetic acid and to calculate its Ka. Materials: 25 mL pipet and bulb burette 2x150 mL beaker 125 mL Erlenmeyer flask acetic
64. ## college

What is the concentration of a solution of HCL in which a 10.0 mL sample of acid required 50.0 mL of 0.150 M NaOH for neutralization?
65. ## chemistry help asap

Please check these thanks. 1. In a titration, 33.21 mL 0.3020M rubidium hydroxide solution is required to exactly neutralize 20.00 mL hydrofluroic acid solution. What is the molarity of the hydrofluroic acid solution? Answer: 0.502HF 2. A 35.00 mL-sample
66. ## chemistry

Lab: Determining Ka of Acetic Acid Purpose: The purpose of this experiment is to determine the molar concentration of a sample of acetic acid and to calculate its Ka. Materials: 25 mL pipet and bulb burette 2x150 mL beaker 125 mL Erlenmeyer flask acetic
67. ## Chemistry

If a 11.0 mL sample of vinegar (aqueous acetic acid ) requires 19.0 mL of 0.500 M NaOH to reach the endpoint, what is the original molarity of the acetic acid solution?
68. ## Chemistry

If you have 200 ml of a 0.1M solution of acetic acid (pka=4.75), 1. How many ml of a solution of 1.O M NaOH would you need to adjust the pH to 5.2? 2. How many ml of water would you then add to make the solution of 0.05M in total acetic acid (ie., acetic
69. ## chemistry

Concentrated acetic acid, HC2H3O2 is 17.4 M. How many mL of concentrated acetic acid do you need to prepare 125 mL of a 0.150 M solution of acetic acid?
70. ## CHEMISTRY

1.Chemistry Question: A 0.1 M solution of acetic acid is titrated with 0.05M solution of NaOH. What is the pH when 60% of the acid has been neutralized? The equilibrium constant (Ka) for acetic acid is 1.8x10^-5 2. Chemistry question: On average, how far
71. ## Inorganic chemistry

A 50ml sample of vinegar is titrated with 0.774M NaOH(aq). If the titration requires 41.6ml of NaOH(aq), what is the concentration of acetic acid in the vinegar?
72. ## bio chem

What is the ph when 100 mL of 0.1 M NaOH is added to 150 mL of 0.2 M Hac if pka for acetic acid =4.76?
73. ## Chem

A sample contains an unknown amount of tartaric acid, H2C4H4O6. If 0.3888 g of the sample requires 37.74 mL of 0.1000 M NaOH to neutralize the H2C4H4O6 completely, what is the percentage of H2C4H4O6 in the sample? The molar mass of H2C4H4O6 is 150.09
74. ## chem

1.Pippete 20ml of 0.1M acetic acid and 20ml of 0.1M NaOH into a 100ml beaker (Remember that the final volume of this solution is the sum of the volumes of the acetic acid and NaOH solutions that have been mixed) 2. Pippete 20ml of 0.1 acetic acid into
75. ## Chemistry

Calculate the molar concentration of acetic acid (CH3COOH) in a 5.00-mL sample of vinegar (density is 1.00 g/mL) if it is titrated with 25.00 mL of NaOH.
76. ## chemistry

Prepare 500mL of a 0.200 M acetate buffer at pH 4.90 using only pure acetic acid, 3M NaOH, and water. 1) Add acetic acid to ~400mL of water in a 500 mL beaker. How many grams of acetic acid are needed? 2)Add 3 M NaOH solution until pH is 4.90. What volume
77. ## chemistry

A volume of 100mL of 1.00 M HCl solution is titrated with 1.00 M NaOH solution. You added the following quantities of 1.00 M NaOH to the reaction flask. Classify the following conditions based on whether they are before the equivalence point, at the
78. ## Chemistry

Assuming that the lab procedure was conducted in an identical manner in all other respects, if a large quantity of vinegar had been taken initially for analysis, for example, a 50.0 ml instead of 25.0mL discuss briefly how each of the following would
79. ## Chemistry

A beaker with 150 mL of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 7.90 mL of a 0.480 M HCl solution to the beaker. How much will the pH change?
80. ## Chemistry

A beaker with 150 mL of an acetic acid buffer with a pH of 5.00 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 5.60 mL of a 0.280 M HCl solution to the beaker. How much will the pH change?
81. ## Chemistry lab

A 1.340gram sample of an unknown acid, H3A, was placed in a 250.0 mL volumetric flask and diluted to volume with water. A 45.35 mL sample of this acid solution was titrated with 37.77 mL of a 0.1006M NaOH solution. A) Using one set - up dimensional
82. ## Chemistry

Assuming that the lab procedure was conducted in an identical manner in all other respects, if a large quantity of vinegar had been taken initially for analysis, for example, a 50.0mL instead of 25.0 mL discuss briefly how each of the following would
83. ## chemistry

2. When preparing a NaOH solution, a student did not allow the NaOH pellets to completely dissolve before standardizing the solution with KHP. However, by the time the student reﬁlled the buret with NaOH to titrate the acetic acid, the remaining NaOH
84. ## Chemistry

Please help me... I don't understand this at all. I need to calculate the molarity of the acetic acid in this problem: A 4,00 mL sample of vinegar (acetic acid) was tirated with 0.1250M NAOH according to the following equation: HC2H3)s + NAOH --- NAC2H3O2
85. ## Chemistry

1.) Watch the animation, and observe the titration process using a standard 0.100 M sodium hydroxide solution to titrate 50.0 mL of a 0.100 M hydrochloric acid solution. Identify which of the following statements regarding acid-base titrations are correct
86. ## AP CHEM

Please help me with these AP Chemistry homework problems and show me the steps how to find the solutions: Liquid-Liquid Tirations: What is the concentration of the unkown solution for each of the following titrations? #5) 25.36 mL of 0.178 M NaOH is
87. ## chemistry

Titration was used to determine the molarity of acetic acid in vinegar. A primary standard solution of KHP was used to standardize the NaOH. 1. When performing this experiment, impure KHP was used to standardize the NaOH solution. If the impurity is
88. ## chemistry help

a 3.54 grams solid sample of an unknown monoprotic acid was dissolved in distilled water to produce a 47.0 mL solution at 25 degrees. This solution was then titrated with 0.2 M NaOH. The equivalence point was reached when 35.72 mL of 0.2 M NaOH was
89. ## chemistry

a 3.54 grams solid sample of an unknown monoprotic acid was dissolved in distilled water to produce a 47.0 mL solution at 25 degrees. This solution was then titrated with 0.2 M NaOH. The equivalence point was reached when 35.72 mL of 0.2 M NaOH was
90. ## chemistry

A 15.00 mL sample of an unknown monoprotic weak acid solution is titrated with 0.35 M NaOH. The initial buret reading is 0.23 mL. The phenolphthalein indicator turns the solution light pink when the buret reads 29.58 mL. A. what volume of 0.35 M NaOH was
91. ## gen chem

a 10 ml vinegar sample was completely neutralized by 22.5 0.2M NaOH solution . calculate the molarity and percent acetic acid in vinegar I keep getting 2.7% acetic acid is this correct? my friend got 27% and if I am wrong where do you think I messed up?
92. ## Chemistry

15.00mL sample of a solution of H2SO4 of unknown concentration was titrated with 0.3200 N NaOH. The titration required 21.30mL of the base. What was the normality of the acid solution? what was the molarity of the acid solution?
93. ## Chemistry

Hi, could someone help me with these calculations for my lab; Given: Volume of vinegar analyzed:5 mL Con'c of NaOH: 0.09890M Avg. V of NaOH from titration:43.75 mL Moles of NaOH required to reach the equivalence point: ? Would this be
94. ## Chemistry

1. You have been given a sample of unknown molarity. Calculate the molarity of a solution which has been prepared by dissolving 8.75 moles of sodium chloride in enough water to produce a solution of 6.22l. 2. You have a sample which consists of 428g sodium
95. ## CHEMISTRY

You have been given a sample of unknown molarity. Calculate the molarity of a solution which has been prepared by dissolving 8.75 moles of sodium chloride in enough water to produce a solution of 6.22l. 2. You have a sample which consists of 428g sodium
96. ## CHEMISTRY URGENT

1. You have been given a sample of unknown molarity. Calculate the molarity of a solution which has been prepared by dissolving 8.75 moles of sodium chloride in enough water to produce a solution of 6.22l. 2. You have a sample which consists of 428g sodium
97. ## chemistry 2

Titration of 50.0 mL of acetic acid reaches equivalence after delivery of 22.5mL of standardized NaOH 0.21 M. What is the initial concentration of acetic acid and what is the pH of the solution? What is the pH at equivalence? What is the pH adition of 20.0
98. ## Chemistry

You are carrying out the titration of 100.0 mL of 1.000M acetic acid with 1.000 M sodium hydroxide. Ka = 1.76x10^-5 of acetic acid. (a) Calculate the initial pH of your acetic acid sample. (b) Calculate the pH of the solution after the addition of 25.0mL
99. ## Chemistry

Titration of 50.0 ml of acetic acid reaches equivalence after delivery of 22.5 ml of standardized NaOH 0.21 M. What is the initial concentration of acetic acid and what is the pH of the solution? What is the pH at equivalence? What is the pH after addition
100. ## Chemistry

Calculate the percentage of acetic acid used in 2.1g of acetic acid that was titrated against 0.1M NaOH