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Part 1- Calculations: To calculate the exact concentration of your ~0.1 M NAOH(aq) solution, the following logic stream can be used. The stockroom will provide you with a stock solution of KHP(aq), whose concentration is known and labeled on the bottle. Be sure to record this concentration, with proper units, in the data section of your notebook! use 25.00 mL of KHP solution concentration of KHP mass of KHP (grams) moles of KHP grams KHP(s) liters of solution 1:1 mole ratio of KHP:NaOH from balanced chemical equation molarity of NaOH(aq) volume of NaOH(aq) (mL) moles NaOH moles of NaOH liters of solution added to neutralize KHP

Part 1- Calculations: To calculate the exact concentration of your ~0.1 M NAOH(aq) solution, the following logic stream can be used. The stockroom will provide you with a stock solution of KHP(aq), whose concentration is known and labeled on the bottle. Be sure to record this concentration, with proper units, in the data section of your notebook! use 25.00 mL of KHP solution concentration of KHP mass of KHP (grams) moles of KHP grams KHP(s) liters of solution 1:1 mole ratio of KHP:NaOH from balanced chemical equation molarity of NaOH(aq) volume of NaOH(aq) (mL) moles NaOH moles of NaOH liters of solution added to neutralize KHP

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Hi I am having trouble finishing and finding the rest of the data for my Titration lab. I've already imputed the given data and just need to find the rest of the excel boxes using those data, thank you.

1 2 KHP STandardization g/L KHP Moles/L KHP 3 20.03 4 5 Moles per Trial 6 7 NaOH Standardization Trial 1 Trial 2 Trial 3 Reading Start Reading End 8 1.01 1.5 1.3 9 24.48 25.12 24.55 10 Total 11 NaOH mol/L 12 Average (3 Trials) 13 STD 14 15 Titration 16 Trial 1 Trial 2 Trial 3 Reading Start Reading End 17 1 1.01 1.5 18 35.05 34.99 35.25 19 Total 20 Moles of NaOH 21 Moles of H2SO4 22 H2SO4 mol/L Average 3 Trials STD Three Trials % STD 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 Sheet1 +
Transcribed Image Text:1 2 KHP STandardization g/L KHP Moles/L KHP 3 20.03 4 5 Moles per Trial 6 7 NaOH Standardization Trial 1 Trial 2 Trial 3 Reading Start Reading End 8 1.01 1.5 1.3 9 24.48 25.12 24.55 10 Total 11 NaOH mol/L 12 Average (3 Trials) 13 STD 14 15 Titration 16 Trial 1 Trial 2 Trial 3 Reading Start Reading End 17 1 1.01 1.5 18 35.05 34.99 35.25 19 Total 20 Moles of NaOH 21 Moles of H2SO4 22 H2SO4 mol/L Average 3 Trials STD Three Trials % STD 23 24 25 26 27 28 29 30 31 32 33 34 35 36 37 38 39 40 41 42 43 44 Sheet1 +
Acid-Base Titrations – Background Part 1– Standardization of ~0.1 M NaOH(aq): In Part 1 of today's experiment, you will prepare an approximately 0.1 M solution of NaOH(aq) by diluting a 6 M solution of NaOH(aq). You will then accurately determine the exact concentration of your ~0.1 M NAOH(aq) solution by a process known as standardization. To "standardize" means to accurately determine the concentration of a solution, so that solution may be used for another measurement. You can think of it as calibrating a solution. Crystalline potassium hydrogen phthalate (abbreviated KHP) will be used as the primary standard acid. By titrating a NaOH solution against a measured mass of KHP, you can accurately determine the concentration of the NaOH solution. Then, it is possible to titrate solutions of acids having unknown concentrations with the NaOH solution (whose concentration has now been determined) to find the respective unknown acid molarities. Potassium hydrogen phthalate (KHP) is a weak, monoprotic (one acidic H, denoted by H*) organic acid that reacts with aqueous sodium hydroxide according to the reaction: H :0: H :0: H H* Н. Na + NaOH(aq) *H' `H H :0: potassium hydrogen phthalate(aq) KHP (C3H;KO4) In order to detect the equivalence point (the endpoint when the reactants are exactly neutralized), an indicator dye, such as phenolphthalein, is added to the reaction mixture. The endpoints of your titrations will be signaled by the phenolphthalein color change. The indicator, in this case, is sensitive to the relative amount of hydroxide ion in solution which increases quickly once the KHP reactant is used up. Part 1- Calculations: To calculate the exact concentration of your ~0.1 M NAOH(aq) solution, the following logic stream can be used. The stockroom will provide you with a stock solution of KHP(aq), whose concentration is known and labeled on the bottle. Be sure to record this concentration, with proper units, in the data section of your notebook! use 25.00 mL of KHP solution concentration of KHP mass of KHP grams KHP(s) liters of solution/ moles of KHP (grams) 1:1 mole ratio of KHP:NaOH from balanced chemical equation molarity of NaOH(aq) volume of NaOH(aq) (mL) moles NaOH moles of NaOH liters of solution/ added to neutralize KHP Acid-Base Titrations – Background В-1 Part 2 – Determination of the Unknown Concentration of Sulfuric Acid: By now, you'll know the exact concentration of your ~0.1 M NaOH(aq). In Part 2 of today's experiment, you'll titrate your ~0.1 M NaOH(aq) solution against a solution of sulfuric acid (H2SO4) whose concentration is unknown. 2NAOH(aq) + H;S0:(aq) Na2SO4(aq) + 2H;O(1) Once again, phenolphthalein will be used to indicate the equivalence point of the titration; the point where enough NaOH(aq) has been added to completely consume the H2SO4(aq) and any further addition of NaOH(aq) quickly raises the pH of the solution. Part 2 – Calculations: Although the balanced chemical equation is different from Part 1, the logic to determine the unknown H,SO4(aq) concentration is nearly the same, albeit in reverse. molarity of NaOH(aq) volume of NaOH(aq) (mL) moles NaOH moles of NaOH liters of solution/ added to neutralize H,SO4 2:1 mole ratio of NaOH:H2SO4 from balanced chemical equation molarity of H,SO4(aq) moles H2SO4 liters of solution/ use 25.00 mL of H,SO, solution moles of H2SO4
Transcribed Image Text:Acid-Base Titrations – Background Part 1– Standardization of ~0.1 M NaOH(aq): In Part 1 of today's experiment, you will prepare an approximately 0.1 M solution of NaOH(aq) by diluting a 6 M solution of NaOH(aq). You will then accurately determine the exact concentration of your ~0.1 M NAOH(aq) solution by a process known as standardization. To "standardize" means to accurately determine the concentration of a solution, so that solution may be used for another measurement. You can think of it as calibrating a solution. Crystalline potassium hydrogen phthalate (abbreviated KHP) will be used as the primary standard acid. By titrating a NaOH solution against a measured mass of KHP, you can accurately determine the concentration of the NaOH solution. Then, it is possible to titrate solutions of acids having unknown concentrations with the NaOH solution (whose concentration has now been determined) to find the respective unknown acid molarities. Potassium hydrogen phthalate (KHP) is a weak, monoprotic (one acidic H, denoted by H*) organic acid that reacts with aqueous sodium hydroxide according to the reaction: H :0: H :0: H H* Н. Na + NaOH(aq) *H' `H H :0: potassium hydrogen phthalate(aq) KHP (C3H;KO4) In order to detect the equivalence point (the endpoint when the reactants are exactly neutralized), an indicator dye, such as phenolphthalein, is added to the reaction mixture. The endpoints of your titrations will be signaled by the phenolphthalein color change. The indicator, in this case, is sensitive to the relative amount of hydroxide ion in solution which increases quickly once the KHP reactant is used up. Part 1- Calculations: To calculate the exact concentration of your ~0.1 M NAOH(aq) solution, the following logic stream can be used. The stockroom will provide you with a stock solution of KHP(aq), whose concentration is known and labeled on the bottle. Be sure to record this concentration, with proper units, in the data section of your notebook! use 25.00 mL of KHP solution concentration of KHP mass of KHP grams KHP(s) liters of solution/ moles of KHP (grams) 1:1 mole ratio of KHP:NaOH from balanced chemical equation molarity of NaOH(aq) volume of NaOH(aq) (mL) moles NaOH moles of NaOH liters of solution/ added to neutralize KHP Acid-Base Titrations – Background В-1 Part 2 – Determination of the Unknown Concentration of Sulfuric Acid: By now, you'll know the exact concentration of your ~0.1 M NaOH(aq). In Part 2 of today's experiment, you'll titrate your ~0.1 M NaOH(aq) solution against a solution of sulfuric acid (H2SO4) whose concentration is unknown. 2NAOH(aq) + H;S0:(aq) Na2SO4(aq) + 2H;O(1) Once again, phenolphthalein will be used to indicate the equivalence point of the titration; the point where enough NaOH(aq) has been added to completely consume the H2SO4(aq) and any further addition of NaOH(aq) quickly raises the pH of the solution. Part 2 – Calculations: Although the balanced chemical equation is different from Part 1, the logic to determine the unknown H,SO4(aq) concentration is nearly the same, albeit in reverse. molarity of NaOH(aq) volume of NaOH(aq) (mL) moles NaOH moles of NaOH liters of solution/ added to neutralize H,SO4 2:1 mole ratio of NaOH:H2SO4 from balanced chemical equation molarity of H,SO4(aq) moles H2SO4 liters of solution/ use 25.00 mL of H,SO, solution moles of H2SO4
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