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

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

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

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.

Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. solution initial components initial type (check all that apply) change effect of change on pH (check one) acidic A H₂O basic add NaNO3 neutral acidic O pH higher pH lower pH the same O pH higher B H₂O, HCI basic add K Cl O pH lower neutral acidic C H₂O, HCI basic add KOH neutral acidic D H₂O basic add HNO3 Oneutral O pH the same O pH higher O pH lower O pH the same O pH higher O pH lower O pH the same 5

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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…

Question 1

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…

Just answer please label answer to questions so I know do all please  1. Stomach acid is approximately 0.10 M HCl. How many mL of stomach acid can be neutralized by one regular antacid tablet that contains 500 mg of solid CaCO3 (100.09 g/mol)? a. 1000b.50 c. 500 d. 100 e. 200 3. What is the formula of the precipitate that forms when aqueous NaCl and aqueous Hg2(NO3)2 are mixed?a. Hg2Cl2b. NaNO3 c.HgCl2 d. HgCl e. Hg2Cl

need answer

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

Question 2

Please answer the 3 boxes for ph

Calculate the Molarity

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

Help me answer this one question:

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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...

Please help me answer this question:

uestion Completion Status: 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 the same as the actual value. lower than the actual value. O higher than the actual value. O Need more information QUESTION 14 What is the BEST numerical value for the quantity of liquid in the graduated cylinder? Save All A Click Save and Submit to save and submit. Click Save All Answers to save all answers.

How to calculate the molarity of the acetic acid. And how to calculate the grams of acetic acid in 1 liter of the vinegar.

Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. solution initial components initial type (check all that apply) change effect of change on pH (check one) O acidic A H₂O, KOH basic ○ pH higher add KI O pH lower neutral acidic B H₂O basic add H CIO4 O neutral ☐ acidic C H₂O ☐ basic add Na CIO O neutral acidic O pH the same O pH higher O pH lower O pH the same O pH higher O pH lower O pH the same O pH higher D H₂O, KOH basic add HI O pH lower Oneutral O pH the same

Each row of the table below describes an aqueous solution at 25 °C. The second column of the table shows the initial components of the solution. • Use the checkboxes in the third column to explain the type of the initial solution. The fourth column describes a change in the solution. • Use the fifth column to predict how the change in the solution will change its pH. solution initial components initial type (check all that apply) change effect of change on pH (check one) acidic pH higher A H₂O basic add Nal pH lower neutral pH the same acidic pH higher B H₂O, KOH basic add H Br pH lower neutral pH the same acidic pH higher C H₂O basic add NaOH pH lower neutral pH the same acidic pH higher H2O, КОН basic add K Br pH lower neutral pH the same