One problem in studying Tomato Juice is that it has an opaque red color which would interfere with the observation of the color of a pH indicator.
to determine the concentration of the unknown solution and to determine the molar concentration of acetic acid in a sample of vinegar by titrating it with a standard solution of NaOH.
You can determine the amount or concentration of NaOH by titrating with a standard solution of acid.
Determination of the concentration of sodium hydroxide in solution with the help of a neutralization reaction.
I presume you are titrating a standardized solution of (eg) HCl with NaOH to determine the molarity of the alkali. You would normally use an indicator which will change colour at the end point (eg colourless to pink for phenolphthalein). If the solution is very coloured to begin with it can mask the colour change and so make the end point hard to see and lead to a miscalculation of molarity.
Unless the compound you are titrating is air sensitive, which is uncommon, the main effect of air on a titration is on the strong base solution. If you are titrating a weak acid with a strong base, then the strong base solution must be very carefully standardized so that you know the exact number of moles of base. However, carbon dioxide (CO2) in the air can combine with water to form carbonic acid (H2CO3). When CO2 mixes with the water of the strong base solution forming H2CO3, it will tend to slightly neutralize it, reducing the actual concentration base in the solution.
to determine the concentration of the unknown solution and to determine the molar concentration of acetic acid in a sample of vinegar by titrating it with a standard solution of NaOH.
You can determine the amount or concentration of NaOH by titrating with a standard solution of acid.
In titrations, the end point is when you have brought the tested sample to absolute neutral. At this point, if you add one more drop of titrating solution to the sample, you would change the pH sufficient to change the color of the indicator in the sample. This is the point at which you can determine the pH of the original solution, by calculating back the amount of titrating solution you had to add to the sample to neutralize it.
Determination of the concentration of sodium hydroxide in solution with the help of a neutralization reaction.
The easiest way is to add back some of the solution you were titrating. If phenolphthalein remains, it will react with the solution and change back to purple. Incidentally, phenolphthalein will always remain in the solution of the titration reaction - it changes color depending upon the pH of the solution, but the indicator itself is not affected by the titration reaction.
what is procedural laguage
To determine the concentration of a solution, you would need to separate the solution. You then determine how much of the solution is diluted, and how much is whole.
I presume you are titrating a standardized solution of (eg) HCl with NaOH to determine the molarity of the alkali. You would normally use an indicator which will change colour at the end point (eg colourless to pink for phenolphthalein). If the solution is very coloured to begin with it can mask the colour change and so make the end point hard to see and lead to a miscalculation of molarity.
Unless the compound you are titrating is air sensitive, which is uncommon, the main effect of air on a titration is on the strong base solution. If you are titrating a weak acid with a strong base, then the strong base solution must be very carefully standardized so that you know the exact number of moles of base. However, carbon dioxide (CO2) in the air can combine with water to form carbonic acid (H2CO3). When CO2 mixes with the water of the strong base solution forming H2CO3, it will tend to slightly neutralize it, reducing the actual concentration base in the solution.
You need to determine the percent of hydrogen (pH) molecules in the solution.
In a solution particles are not identifiable.
standardization of solution is the process used to determine the concentration of solution