Calculate the accurate molarity of the sodium hydroxide solution using date from each titration to determine two values for the molarity. Calculate the average molarity of the sodium hydroxide solution from the individual values, and use the average in subsequent calculations.Given: Molarity of sulfuric acid:0.205 M(Sodium hydroxide with sulfuric acid)Approx Titration-initial buret reading : 0mLfinal buret reading : 31.8mLtitration 1-initial buret reading : 0mLfinal buret reading : 31.5 mLtitration 2-initial buret reading: 0mLfinal buret reading : 31.7mLAnalysis of vinegarApprox titration -initial buret reading : 0mLfinal buret reading : 20.1 mLtitration 1- volume of vinegar solution:5mLinitial buret reading : 0mLfinal buret reading : 20.9mLtitration 2-Volume of vinegar solution :5mLinitial buret reading : 0mLfinal buret reading : 20.0mL Experimental Procedure:Part A. Preparation of the NAOH solutionWeigh approximately 2 g of sodium hydroxide pellets on a watch glass and transferthe solid to your large beaker.1.Add about 400 mL of deionized water and stir to dissolve the solid. This solution hasa concentration of approximately 0.1 M NAOH. Its molarity must be determinedexactly by titrating it with sulfuric acid according to equation (1) above.2.Part B. Titration of NaOH with sulfuric acid1. Rinse a clean buret with about 10 mL of the NaOH solution. Add the solution, brieflydrain a small volume to remove bubbles from the buret tip, then fill the buret with thesolution to about the 0 mL line. Record the actual volume.2.Collect about 40 mL of standard sulfuric acid solution in a small beaker. Record themolarity of the acid.3.Rinse a 10.00 mL pipet with a little of the sulfuric acid (2-3 mL) and discard the acid.4.Using the pipet, transfer 10.00 mL of sulfuric acid solution to a clean flask (the flaskdoes not have to be dry and can be wet with water, but do not rinse the flask withacid).5.Add 20 mL deionized water and 3 drops ofphenolphthalein indicator. Place the flaskon a sheet of white paper so the color change will be more clearly visible.6.Now add the sodium hydroxide solution from the buret until a faint pink colorpersists for at least 30 seconds. During the addition swirl the flask gently. During thistitration, the sodium hydroxide can be added fairly rapidly to give an approximateidea of how much solution is needed to neutralize the acid in the flask.7.Record the volume of sodium hydroxide used, but do not use it in your calculations.8.Refill the buret with sodium hydroxide.9.Rinse out the flask with water and again pipet 10.00 mL of the sulfuric acid solutioninto the flask, followed by about 20 mL of water and 3 drops.of indicator.0.Repeat the titration more carefully using the volume of sodium hydroxide solutionfrom step 7 to estimate the approximate volume required for the final titration. Ade20 - 2 Purpose of the Experiment:ofsolution). You will therefore be doing two acid-base titrations in this exercise.Equation (1) illustrates the reaction between sulfuric acid and sodium hydroxide:H,SO, (aq) +2 NaOH (aq) - Na,sO, (aq) +2 H,O (1) (1)Equation (2) shows the reaction between acetic acid and sodium hydroxide:HC,H,O, (aq) + NaOH (aq) - NaCH,O, (aq) + H,O (1) (2)gaiar

A numerical problem based on quantitative analysis, which is to be accomplished.

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Chemistry: Principles and Practice

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ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.60QE: Consider all acid-base indicators discussed in this chapter. Which of these indicators would be...

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Calculate the accurate molarity of the sodium hydroxide solution using date from each titration to determine two values for the molarity. Calculate the average molarity of the sodium hydroxide solution from the individual values, and use the average in subsequent calculations.

Given: Molarity of sulfuric acid:0.205 M

(Sodium hydroxide with sulfuric acid)Approx Titration-

initial buret reading : 0mL

final buret reading : 31.8mL

titration 1-

initial buret reading : 0mL

final buret reading : 31.5 mL

titration 2-

initial buret reading: 0mL

final buret reading : 31.7mL

Analysis of vinegar

Approx titration -

initial buret reading : 0mL

final buret reading : 20.1 mL

titration 1-

volume of vinegar solution:5mL

initial buret reading : 0mL

final buret reading : 20.9mL

titration 2-

Volume of vinegar solution :5mL
initial buret reading : 0mL

final buret reading : 20.0mL

Experimental Procedure:
Part A. Preparation of the NAOH solution
Weigh approximately 2 g of sodium hydroxide pellets on a watch glass and transfer
the solid to your large beaker.
1.
Add about 400 mL of deionized water and stir to dissolve the solid. This solution has
a concentration of approximately 0.1 M NAOH. Its molarity must be determined
exactly by titrating it with sulfuric acid according to equation (1) above.
2.
Part B. Titration of NaOH with sulfuric acid
1. Rinse a clean buret with about 10 mL of the NaOH solution. Add the solution, briefly
drain a small volume to remove bubbles from the buret tip, then fill the buret with the
solution to about the 0 mL line. Record the actual volume.
2.
Collect about 40 mL of standard sulfuric acid solution in a small beaker. Record the
molarity of the acid.
3.
Rinse a 10.00 mL pipet with a little of the sulfuric acid (2-3 mL) and discard the acid.
4.
Using the pipet, transfer 10.00 mL of sulfuric acid solution to a clean flask (the flask
does not have to be dry and can be wet with water, but do not rinse the flask with
acid).
5.
Add 20 mL deionized water and 3 drops ofphenolphthalein indicator. Place the flask
on a sheet of white paper so the color change will be more clearly visible.
6.
Now add the sodium hydroxide solution from the buret until a faint pink color
persists for at least 30 seconds. During the addition swirl the flask gently. During this
titration, the sodium hydroxide can be added fairly rapidly to give an approximate
idea of how much solution is needed to neutralize the acid in the flask.
7.
Record the volume of sodium hydroxide used, but do not use it in your calculations.
8.
Refill the buret with sodium hydroxide.
9.
Rinse out the flask with water and again pipet 10.00 mL of the sulfuric acid solution
into the flask, followed by about 20 mL of water and 3 drops.of indicator.
0.
Repeat the titration more carefully using the volume of sodium hydroxide solution
from step 7 to estimate the approximate volume required for the final titration. Ade
20 - 2

Purpose of the Experiment:
of
solution). You will therefore be doing two acid-base titrations in this exercise.
Equation (1) illustrates the reaction between sulfuric acid and sodium hydroxide:
H,SO, (aq) +2 NaOH (aq) - Na,sO, (aq) +2 H,O (1) (1)
Equation (2) shows the reaction between acetic acid and sodium hydroxide:
HC,H,O, (aq) + NaOH (aq) - NaCH,O, (aq) + H,O (1) (2)
gaiar

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