Calculating the Concentration of Acetic Acid in Vinegar Lab

A titration involves reacting two solutions - one with a known concentration and the other with an unknown concentration. The goal of the lab is to calculate the concentration of acetic acid in vinegar, so that is the solution with the unknown concentration. Therefore, there must be a way to find the concentration of the base solution so that it can be known. A separate procedure can be used to do this. The process is called standardization and is formally defined as the process by which the concentration of a standard solution is determined by titration against a primary standard. The primary standard used in standardizing sodium hydroxide is potassium hydrogen phthalate, otherwise known as KHP.
1. KHP is a solid. What tool in the lab can you use to be sure within 4 significant figures of the number of moles of acid in your reaction?
2. You will need to make a more dilute solution of sodium hydroxide than the 6 M sodium hydroxide that you'll find in the hood to react with KHP. It is recommended that you make a 0.2 M solution. How many significant figures are represented by a 6 M solution of sodium hydroxide?
3. How will you make a 0.2 M solution of sodium hydroxide from a 6 M solution of sodium hydroxide? Provide detail.
4. Do you have more significant figures to describe the number of moles of KHP? Or the number of moles of sodium hydroxide?

1. Is aceticacid a strong acid or a weak acid? Write a net ionic equation of aceticacid in water.
2. If a strong base is added to aceticacid, at what pH(acidic, basic, or neutral) will you expect to find the point at which moles of acid are equal to moles of base?
3. Write a net ionic equation of aceticacid with str

A titration was conducted to determine the percent of acetic acid within vinegar. The reaction of this titration is HC(2)H(3)O(2) --->NaC(2)H(3)O(2) +H(2)O (water)
Given Concentration of NaOH 0.2959 M.
Final Buret Reading:26.72 mL
Initial buret reading :0.02 mL
Volume of NaOH added: 2

Here is the problem:
0.25 ml of 0.10M aceticacid solution. The pH meter reads 2.88. Use the measured pH and known concentration of theaceticacid solution to determine the pKa of aceticacid.
1. Using the equation pKa= -log Ka, calculate the Ka from the pH value and the starting aceticacidconcentration.
2. Calculate the

Acid content of vinegar
Flask 1 Flask 2
Inital volume of NaOH in burette 0 17.5
Final volume of NaOH in burette 17.5 35.3
Volume of NaOH used for titration

Provide a method for determining the Ka of aceticacid by titration with NaOH based on the data below.
Show details of the calculations.
Titration #1
4 drops of methyl red indicator (to show endpoint).
Burette fill with 50ml of 0.1 M NaOH.
Titrate by adding 1ml increments of NaOH.
Continue titration past the endpoint t

Given theconcentration of a weak acid, calculate the pH of the solution. The Ka for aceticacid, CH3COOH, is 1.8x10^-5. Calculate the [H+] of a 0.20 M solution of aceticacid in water.

Write a balanced equation for the neutralization of aceticacid with NaOH.
I have actually gotten better at balancing equations---but I have no idea where to even start with this one.
Any help you can provide would be greatly appreciated.
Thank You,

1) Calculate the pH of the following solutions:
(a) 0.010 M acetic acid (Ka= 1.76E-5)
CH3COOH + H2O --> H3O+ + CH3COO-
initial 0.010 -- ? ?
Equilibrium 0.010-x -- ? ?
Show how did you solve this equation to get 1.76E-5:
Ka = [H3O][CH3COO]/[CH3COOH] = 1.76E-5
(b)

See the attached file.
1. Suppose X ~ U[-2, 2]. For what a,b is a+bX~U[0,1]?
2. A city bus is supposed to arrive at a fixed stop at 12:00 noon, but its arrival time is uniformly distributed between 11:57 AM and 12:04 PM. If it has not yet arrived at 12:01 PM, what is the probability that it will arrive by 12:02 PM?
3. The con