Titration Lab Report

STANDARDIZATION OF A SODIUM HYDROXIDE SOLUTION PRE-LABORATORY EXPERIMENT 10 QUESTIONS NAME DATE 1. What is the purpose of this experiment? 2. A sample of KHP has a mass of 2.345 g is used for a titration, how many moles of KHP is this sample? 3. How many moles of NaOH would be needed to reach the endpoint of this titration with sample of KHP from the previous question? 4. If the initial volume of the NaOH in the burette was 0,50 mL and the final volume is shown to the right, what is the volume of NaOH used in this titration? 18 19 5. What is the concentration of the NaOH solution used in this titration? EXPERIMENT 10 155

QUESTION 9 Acid-Base Titration In this experiment, an indicator called phenolphthalein is used to signal the endpoint of the titration (when the acid has been fully neutralized by the base). The indicator is colorless in acidic solution and pink in basic solution. During the titration, the pink color will appear and then disappear quickly with each addition of base (titrant). If a student is having trouble seeing the pink color in the sample flask, what can be done to help them see the color more clearly? Experiment - Acid-Base Titration.pdf O Remove safety goggles to get them out of the way. O Add several more drops of indicator - the more the better! O Place a piece of white paper or a white paper towel beneath the sample flask. O Place something dark beneath the sample flask.

EXPERIMENT 10 PRE-LABORATORY QUESTIONS STANDARDIZATION OF A SODIUM HYDROXIDE SOLUTION NAME DATE 1. What is the purpose of this experiment? 2. A sample of KHP has a mass of 2.345 g is used for a titration, how many moles of KHP is this sample? 3. How many moles of NaOH would be needed to reach the endpoint of this titration with sample of KHP from the previous question? 4. If the initial volume of the NaOH in the burette was 0.50 mL and the final volume is shown to the right, what is the volume of NaOH used in this titration? 19 5. What is the concentration of the NaOH solution used in this titration? EXPERIMENT 10 155

A Question 13 (1 point) Retake question *A buffer solution is prepared by adding 6.02 mL of 1.11 M HI to 192.0 mL of 0.11 M methylammine solution. The buffer is allowed time to establish. Then, 0.005 mol of a strong acid is added. What is the pH? Round your answer to 2 decimal places. Your Answer: Answer

II only O both I & II ОШ only QUESTION 13 Consider an acid-base titration in which the base is dispensed from a burette into a flask containing an acid. If any drops of the base adhere to the inner walls of the flask, but do not actually mix with the solution, the calculated acid concentration would be O the same as the actual value. O lower than the actual value. O higher than the actual value. Need more information Click Save and Submit to save and submit, Click Save All Answers to save all answers. Save Al

C. Titration of acid by a base Standardization of NaOH Volume of NaOH Mass of KHP Initial buret Final buret Trial used Molarity of NaOH (g) reading (mL) reading (mL) (mL) (1) (2) (3) (4) (5) 1.2075 0.7 25 24.3 0.243 (6) (7) (8) (9) (10) 1.2062 16.4 40.9 24.49 0.2412

7) What is the molarity of a 12.46 mL sulfuric acid solution if 18.22 mL of 0.100 M potassium hydroxide is required to reach the endpoint as indicated by a titration .

based on the data tables provided, what is % CH3COOH in vinegar

In titration, what solution is placed inside the burette? Group of answer choices stock solution analyte diluted solution titrant

O II only QUESTION 5 In the experiment "Preparation and Standardization of a Sodium Hydroxide Solution", why was the burette rinsed with NaOH before filling it to "zero" for the titration? To remove any residual liquids from the burette O To check that the burette works properly To remove any air bubbles and fill the tip of the burette All of the above QUESTION 6 Save A Click Save and Submit to save and submit. Click Save All Answers to save all ansuers.

I need help with question 3?

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1 2 3 4 Questions 1-4 refer to the same strong acid/strong base (SA/SB) titration. A 25.00 mL solution of 0.200 M hydroiodic acid (HI) is being titrated with 0.200 M sodium hydroxide (NaOH). What is the initial solution pH (when 0.00 mL of titrant have been added) (Two decimal places) Type your answer... Questions 1-4 refer to the same strong acid/strong base (SA/SB) titration. A 25.00 mL solution of 0.200 M hydroiodic acid (HI) is being titrated with 0.200 M sodium hydroxide (NaOH). What is the solution pH (when 15.00 mL of titrant have been added? (Two decimal places) Type your answer... Questions 1-4 refer to the same strong acid/strong base (SA/SB) titration. A 25.00 mL solution of 0.200 M hydroiodic acid (HI) is being titrated with 0.200 M sodium hydroxide (NaOH). What is the solution pH at the equivalence point? (Two decimal places) Type your answer... Questions 1-4 refer to the same strong acid/strong base (SA/SB) titration. A 25.00 mL solution of 0.200 M hydroiodic acid (HI) is…

YOU DON'T NEED TO ANSWER ALL THE QUESTIONS ALL I NEED HELP WITH IS QUESTIONS 4 and 5. I got d, e, e for the 1st 3 questions if that helps you, but you don't need to worry about questions 1-3 I just included them in case it helps you.      1.What reagent is used as the indicator for the neutralization? a)citric acid b)sodium hydroxide c)sodium citrate d)phenolphthalein   2. What is the mole ratio of NaOH to citric acid for this neutralization reaction? a)2 mole NaOH/1 mole citric acid b)1 mole NaOH/1 mole citric acid c)1 mole NaOH/2 mole citric acid d)1 mole NaOH/3 mole citric acid e)3 mole NaOH/1 mole citric acid   3.If 35.00 mL of 0.1104 M NaOH were used to reach the neutralization point, how many moles of NaOH were dispensed? a)3.154 x 10-3 mol NaOH b)1.104 x 10-4 mol NaOH c)258.8 mol NaOH d)3.864 x 10-3 mol NaOH  4. Using the above mole ratio, convert the moles of NaOH in the previous question to moles of citric acid. a)1.288…

How many mL of 16 N HCl is needed to make a 0.3 N solution from a 500 mL solution of 0.15 N HCl to be used as titrant?   This is titration

QUESTION 8 A 0.9600 M NAOH solution was diluted with a factor of 4. Then the diluted solution of NaOH was titrated against an unknown acld. The volumes of NaOH(aq) titrated are shown in the table below. Volumes of NaOH(aq): Rough titration First titration Third titration Second Third titration titration Final burette reading: (mL) Initial burette reading: (mL) 19.00 34.05 20.86 36.01 23.57 19.00 19.07 5.76 21.02 8.54 The molarity of the unknown acid is 0.08108 M and the volume of the unknown acid used in each titration is 14.80 mL. Was the unknown acid monoprotic, diprotic or triprotic? Show your calculations and reasoning. (i)

Question: Comment on the solubility of the two dyes in water. In your answer consider intermolecular bonds and their relative strengths. Solubility of dye C: Solubility of dye D:

Graph the data by plotting the pH (y-axis) versus the amount of citricacid solution added (x-axis). Make sure that you label the axes of thegraph   Titration Data                         Titration of NaOH Volume Citric Acid  Solution Added (mL) pH 0.0 mL (initial) 7.8 0.5 mL 7.8 1.0mL 7.2 1.5 mL 7.1 2.0 mL 6.9 2.5 mL 6.8 3.0 mL 6.7 3.5 mL 6.6 4.0 mL 6.5 4.5 mL 6.4 5.0 mL 6.2 5.5 mL 6.1 6.0 mL 5.9 6.5 mL 5.9 7.0 mL 5.8

Suppose a student wants to determine the color change interval of an unknown indicator. Her results are given in the table. Tube # pH Unknown indicator 4 6.39 red 7.11 red 6. 7.87 purple 7 8.81 purple 8. 9.07 blue 9 10.10 blue What is the interval of the unknown indicator? The color change interval is between pH 7.11 and pH 7.87. The color change interval is between pH 7.11 and pH 9.07. The color change interval is between pH 9.07 and pH 10.10. The color change interval is between pH 6.39 and pH 10.10. O O

1. At what point (how many milliters of added acid) was the solution in beaker “B” neutralized?     Neutralization of Acids and Bases Test Data:   Table 2:  Initial pH Test Results Container Substance in Container pH using the pH meter A distilled water  6.8  B 0.5 g sodium bicarbonate with distilled water 7.5  C vinegar  2.3 Table 3: Neutralization Amount of Acid Added (mL) pH using the pH Meter 1 mL 7.5 2 mL 7.3 3 mL 7.2 4 mL 7.2 5 mL 7.2

Please answer the 3 boxes for ph

Questions: 1. Why does the tip of your buret need to be free of air bubbles? 2. Explain why the volume of water did not need to be exactly measured or recorded. 3. Define the endpoint of a titration. 4. What is a standard solution? Why is a standard solution necessary for titration? 5. A student starts a titration without phenolphthalein in the Erlenmeyer flask. The student realizes the mistake and adds the phenolphthalein during the titration. Once the phenolphthalein is added, the solution in the Erlenmeyer flask remains colorless. Can the results of this titration be used? Concisely explain. 6. Write a balanced equation for the neutralization of hydrobromic acid with potassium hydroxide. 7. What is the molarity of a 12.46 mL sulfuric acid solution if 18.22 mL of 0.100 M potassium hydroxide is required to reach the endpoint as indicated by a titration. 43

3. Sprite does not contain phosphoric acid. Only sodas that are dark in color contain this acid. sodas such as Sprite contain citric acid, sugar, and carbonaled water Design a simple experiment to determine the concentration of citric acid in SpriteProvide a de tailed procedure

When performing a titration in the lab, which equipment is not used? 1. burette 2. pipette 3. funnel 4. watch glass 5. Erlenmeyer flask

Questions 11-14 refer to the same strong base/strong acid (SB/SA) titration. A 15.00 mL solution of 0.100 M sodium hydroxide (NaOH) is being titrated with 0.250 M hydrobromic acid (HBr). What is the solution pH before the titration begins? (Two decimal places) Type your answer...