CHEM 112 Lecture Notes - Lecture 26: Sodium Hydroxide, Sodium Fluoride, Potassium Nitrite

47 views4 pages

cerisebuffalo390

12 Apr 2016

School

Department

Course

Professor

For unlimited access to Class Notes, a Class+ subscription is required.

Document Summary

Titration definitions: midpoint also known as the equivalence half-point; the middle of the first endpoint and the equivalence point, by volume, equivalance point the point were moles of solution are equal to moles of titrant. Titrating a weak acid with a strong base: 100 ml of 0. 100m acetic acid is titrated with 0. 100 m naoh. Calculate the ph when 35 ml of the base is added: write the reaction. Oh- + ch3cooh ch3coo- + h2o. If they were not the same, then you would have to use the m1v1 = m2v2 equation: see the table below. 0. 01: now do a second table with the concentrations. Titrating a weak base with a strong acid: there is still a buffer region in which the ph changes slowly! Question: a titration needs to be done to determine the exact acid concentration in an unknown solution. It is estimated that the hydronium concentration in the solution is around 2. 75 x 10-6.

Related Questions

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

Drag items A-F to: Before equivalence point, At equivalence point, After equivalence point

A.) The pH of the solution is close to 2

B.) The pH of the solution is close to 12

C.) The pH of the solution is 7

D.) The color of the solution is pink

E.) The color of the solution is blue

F.) The pH changes most rapidly

2.) Consider the balanced equation for the titration of an acid, HCl, with a base, NaOH:

HCl(aq)+NaOH(aq)âNaCl(aq)+H2O(aq)

According to the balanced equation, to neutralize one mole of the acid (HCl) you will have to add one mole of the base (NaOH). Based on the number of moles of HCl and NaOH at a particular stage of titration, the progress of the reaction with respect to the equivalence point can be decided, as shown in the following table:

You can use the following equation to determine the number of moles in a given solution or volume of titrant: number of moles=molarity (mol/L)Ãvolume (in liters)

A volume of 100 mL 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 equivalence point, or after the equivalence point.

Drag items A-F to Before equivalence point, At equivalence point, After equivalence point

A.) 50.0 mL of 1.00 M NaOH

B.) 150 mL of 1.00 M NaOH

C.) 200 mL of 1.00 M NaOH

D.) 10.0 mL of 1.00 M NaOH

E.) 5.00 mL of 1.00 M NaOH

F.) 100 mL of 1.00 M NaOH

Textbook is showing HCl + NaOH titrating problem. After adding 5 mL of NaOH, why is the equation OH + H3O _--> 2h2o? Where is the h3o coming from