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. 12KHP STandardizationg/L KHPMoles/L KHP320.0345Moles per Trial67NaOH Standardization Trial 1Trial 2Trial 3Reading StartReading End81.011.51.3924.4825.1224.5510Total11NaOH mol/L12Average (3 Trials)13STD1415Titration16Trial 1Trial 2Trial 3Reading StartReading End1711.011.51835.0534.9935.2519Total20Moles of NaOH21Moles of H2SO422H2SO4 mol/LAverage 3 TrialsSTD Three Trials% STD23242526272829303132333435363738394041424344Sheet1+ Acid-Base Titrations – BackgroundPart 1– Standardization of ~0.1 M NaOH(aq):In Part 1 of today's experiment, you will prepare an approximately 0.1 M solution ofNaOH(aq) by diluting a 6 M solution of NaOH(aq). You will then accurately determine theexact 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 solutionmay be used for another measurement. You can think of it as calibrating a solution. Crystallinepotassium hydrogen phthalate (abbreviated KHP) will be used as the primary standard acid. Bytitrating a NaOH solution against a measured mass of KHP, you can accurately determine theconcentration of the NaOH solution. Then, it is possible to titrate solutions of acids havingunknown concentrations with the NaOH solution (whose concentration has now beendetermined) to find the respective unknown acid molarities.Potassium hydrogen phthalate (KHP) is a weak, monoprotic (one acidic H, denoted byH*) organic acid that reacts with aqueous sodium hydroxide according to the reaction:H:0:H:0:HH*Н.Na+ NaOH(aq)*H'`HH: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 ofyour 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 theKHP reactant is used up.Part 1- Calculations:To calculate the exact concentration of your ~0.1 M NAOH(aq) solution, the followinglogic 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 ofKHP solutionconcentration of KHPmass of KHPgrams KHP(s)liters of solution/moles ofKHP(grams)1:1 mole ratio of KHP:NaOHfrom balanced chemical equationmolarity of NaOH(aq)volume of NaOH(aq)(mL)moles NaOHmoles of NaOHliters of solution/added toneutralize KHPAcid-Base Titrations – BackgroundВ-1Part 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 oftoday's experiment, you'll titrate your ~0.1 M NaOH(aq) solution against a solution of sulfuricacid (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; thepoint where enough NaOH(aq) has been added to completely consume the H2SO4(aq) and anyfurther 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 determinethe unknown H,SO4(aq) concentration is nearly the same, albeit in reverse.molarity of NaOH(aq)volume of NaOH(aq)(mL)moles NaOHmoles of NaOHliters of solution/added toneutralize H,SO42:1 mole ratio of NaOH:H2SO4from balanced chemical equationmolarity of H,SO4(aq)moles H2SO4liters of solution/use 25.00 mL ofH,SO, solutionmoles of H2SO4

Question

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. 12KHP STandardizationg/L KHPMoles/L KHP320.0345Moles per Trial67NaOH Standardization Trial 1Trial 2Trial 3Reading StartReading End81.011.51.3924.4825.1224.5510Total11NaOH mol/L12Average (3 Trials)13STD1415Titration16Trial 1Trial 2Trial 3Reading StartReading End1711.011.51835.0534.9935.2519Total20Moles of NaOH21Moles of H2SO422H2SO4 mol/LAverage 3 TrialsSTD Three Trials% STD23242526272829303132333435363738394041424344Sheet1+ Acid-Base Titrations – BackgroundPart 1– Standardization of ~0.1 M NaOH(aq):In Part 1 of today's experiment, you will prepare an approximately 0.1 M solution ofNaOH(aq) by diluting a 6 M solution of NaOH(aq). You will then accurately determine theexact concentration of your ~0.1 M NAOH(aq) solution by a process known as standardization.To &#34;standardize&#34; means to accurately determine the concentration of a solution, so that solutionmay be used for another measurement. You can think of it as calibrating a solution. Crystallinepotassium hydrogen phthalate (abbreviated KHP) will be used as the primary standard acid. Bytitrating a NaOH solution against a measured mass of KHP, you can accurately determine theconcentration of the NaOH solution. Then, it is possible to titrate solutions of acids havingunknown concentrations with the NaOH solution (whose concentration has now beendetermined) to find the respective unknown acid molarities.Potassium hydrogen phthalate (KHP) is a weak, monoprotic (one acidic H, denoted byH*) organic acid that reacts with aqueous sodium hydroxide according to the reaction:H:0:H:0:HH*Н.Na+ NaOH(aq)*H'`HH: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 ofyour 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 theKHP reactant is used up.Part 1- Calculations:To calculate the exact concentration of your ~0.1 M NAOH(aq) solution, the followinglogic 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 ofKHP solutionconcentration of KHPmass of KHPgrams KHP(s)liters of solution/moles ofKHP(grams)1:1 mole ratio of KHP:NaOHfrom balanced chemical equationmolarity of NaOH(aq)volume of NaOH(aq)(mL)moles NaOHmoles of NaOHliters of solution/added toneutralize KHPAcid-Base Titrations – BackgroundВ-1Part 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 oftoday's experiment, you'll titrate your ~0.1 M NaOH(aq) solution against a solution of sulfuricacid (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; thepoint where enough NaOH(aq) has been added to completely consume the H2SO4(aq) and anyfurther 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 determinethe unknown H,SO4(aq) concentration is nearly the same, albeit in reverse.molarity of NaOH(aq)volume of NaOH(aq)(mL)moles NaOHmoles of NaOHliters of solution/added toneutralize H,SO42:1 mole ratio of NaOH:H2SO4from balanced chemical equationmolarity of H,SO4(aq)moles H2SO4liters of solution/use 25.00 mL ofH,SO, solutionmoles of H2SO4

Accepted Answer

Interpretation-
To complete the data in table for KHP standardization, NaOH standardization and part…