of NaOH that reacted with the KHP. # mol KHP x NaOH = # mol NaOH Where x is to coefficient in front of the NaOH and x KHP the KHP respectively in the balanced chemical equation. This means that due to systematic error, my accuracy has fallen by 9.03%, which, although not high, is quite a deviation in accuracy. 0.009 mol KHP  x 1 mol NaOH / 1 mol KHP = 0.009 mol NaOH, now to get Molarity of NaOH you need,    mol NaOH / Liters of NaOH solution. Unformatted text preview: Determination of the Molarity of NaOH with KHP *KHP is an abbreviation for potassium hydrogen phthalate (KHC8H4O4) KHC8H4O4 (aq) + NaOH (aq) → KNaC8H4O4 (aq) + H2O (l) Data: Mass of Beaker Mass of KHP & Beaker 3 sf Mass of KHP Initial NaOH buret reading Final NaOH buret reading 4 sf mL of NaOH used Calculations: Trial 1 … To standardize a sodium hydroxide (NaOH) solution against a primary standard acid [Potassium Hydrogen Phthalate (KHP)] using phenolphthalein as indicator. Where [c]KHP is the concentration of KHP Acid. Our first year students titrate a measured mass of a standard, solid, monoprotic acid called Potassium Hydrogen Phthalate (KHP). Keep in mind this is a diprotic molecule. Vol acetic acid(mL): Trial 1: 40.00 … 3. so 2M=N (see page 487 in the textbook) L. 1. mol KHP= (0,436g)/(204,22 (g/(mol))) = 0,00213 mol . A 0.8234-g sample of "KHP" required 38.76 mL of NaOH for titration to the phenolphthalein endpoint. Allowing the KHP to flow along the inner walls of the conical flask. [c]NaOH = n/V = (0.00979/0.0950) = 0.103 mol dm-3 (cm3 is converted into dm3), Weight of weighing boat before adding KHP = 2.67 g, Weight of weighing boat with KHP = 4.67 g, Weight of weighing boat after transfer = 2.68 g, Mass of KHP Transfer = Weight of weighing boat with KHP – Weight of weighing boat after transfer, *Initial volume is the initial reading of the burette and final volume is the reading after adding NaOH solution, From mole ratio, number of moles of NaOH = 0.00974 mol. Article last reviewed: 2019 | St. Rosemary Institution © 2010-2020 | Creative Commons 4.0. To also determine the concentration of NaOH in the KHP solution. Average NaOH molarity calculated to be 0.09515 M. Titrations … ok so you need to convert the .6319g of KHP to moles of KHP can you do that? When KHP and NaOH combine, a positive hydrogen ion leaves the KHC8H4O4 and a negative hydrogen atom leaves the NaOH. Write the complete balanced equation for the neutralization of KHP with NaOH: 2. #Trial 1: # Molar mass of KHP = 204.22 g mol-1 # Mass of KHP = 0.846 g # Moles of KHP = Mass / Molar mass = 0.846 g / (204.22 g/mol) = 0.004143 mol # Volume of NaOH = … KHP stands for potassium hydrogen phthalate, which has the chemical formula KHC8H4O4. Hypothesis: When KHP is added to the solution of NaOH and the indicator, the solution will turn clear and neutralize. Using that solution, the average concentration of potassium hydrogen phthalate was found to be 27.99% in the #52 LO unknown Calculate and enter the molarity of your three acetic acid trials using the volume of standardized NaOH solution required for each and the average molarity of the NaOH solution from the standardization trials with KHP. What is the exact molarity of the NaOH solution? Tutor and Freelance Writer. Cite this article as: William Anderson (Schoolworkhelper Editorial Team), "Titration Lab: NaOH with Standardized solution of KHP," in. Another error was caused by the deviation in the mass of KHP. Part I: Preparing KHP sample To standardize your NaOH solution, measure out approximately 0.5g of the KHC 8 H 4 O 4 (potassium hydrogen phthalate, KHC 8 H 4 O 4, MW = 204.2 g/mol) into an Erlenmeyer flask.Add 30.0 mL of water to the flask and dissolve the KHC 8 H 4 O 4.. This preview shows page 17 - 22 out of 30 pages.. KHP solution (L) 0.0125 0.0120 0.0120 Molarity of NaOH to neutralize KHP solution (mol/L) 0.5882 0.6140 0.6133 Molarity of NaOH to neutralize KHP solution (M) 0.5882 0.6140 0.6133 Sample Calculation For The Average Molarity of Sodium Hydroxide, NaOH solution :- 0.0125 0.0120 0.0120 Molarity of NaOH to neutralize KHP you mole ratio comes directly from the coefficients in your balanced chemical equation. From the mass of KHP actually used and the volume of the volumetric flask, calculate the molarity of the standard KHP solution. MW (KHP) g of KHP Moles KHP = 2. Calculate the hydroxide ion concentration of a solution with pH = 8.25. science. Suppose .6319g of KHP is titrated to the endpoint with 28.80ml NaOH of unknown molarity. Once the thank you so much!! In this reaction as well, one mole of KHP completely reacts with one mole of NaOH. The volumes of NaOH used up shows significant fluctuations. To obtain the moles of KHP, the mass had to be multiplied by one mole over 204.3grams (3). We performed a titration with NaOH solution with KHP. Show your work. The average molarity of the sodium hydroxide solution was found to be 0.155 M after standardization. i wrote the balanced equation but i am not sure what to do next because KHP is given in grams and it doesnt say how much ml of KHP is in the solution. Discussion: In this experiment, the goal was to first find the molarity of NaOH solution by using a buret filled with NaOH solution that was made before the titration began and a flask with distilled water, KHP, and three drops of phenolphthalein solution in it. atmosphere). Since the reaction between KHP and NaOH is of 1:1 stoichiometry, this means that 0.002509 mole of NaOH must have been used. For titration of a strong base you should use a strong acid such as HCl. https://schoolworkhelper.net/titration-lab-naoh-standardized-solution-khp/, Determination of Acetic Acid In Vinegar Lab Explained, Lab Explained: The Effect of Ocean Water and Distilled Water on Iron, Identification of an Unknown Liquid Lab Report, Lab Report Explained: Length and Electrical Resistance of a Wire, Quote Analysis: The unexamined life is not worth living, My Brother Sam is Dead: Summary, Setting, Characters, Parable of the Lost Coin: Gospel of Luke Analysis & Explanation, Power, Control and Loss of Individuality in George Orwell’s 1984, Augustus’ Role in Shaping the Roman Empire, Volume of NaOH added [since the colour change will not happen at, Average Volume of NaOH added in 3 trials (±0.1 cm. However, there has been a deviation of 0.9 cm3, which is significant, but not high. A 0.8234-g sample of "KHP" required 38.76 mL of NaOH for titration to the phenolphthalein endpoint. What I know is due to various errors which tend to happen when conducting an experiment such as contamination of the sample used (impurities) also external factor like temperature and humidity which results the sample to react with the atmosphere (air). solution in it. Mass of KHP needed to be neutralized by NaOH. 0.4877 M. So basically, they want the molarity of acetic acid for each trial. Sufuric acid has 2 equivalents of acid per mole so N = 2eqM = 2eq mol. 퐾퐻퐶 2 퐻 3 푂 3 (푎푞) + 푁푎푂퐻(푎푞) → 퐻.푂(푙) + 퐾푁푎퐶 2 퐻 3 푂 3 (푎푞) (2) By recording the weight of the sample of KHP and the volume of base needed to neutralize it, the molarity of NaOH can be found. Titration data for four trials for approximately 0.50 g of KHP titrated with NaOH of unknow concentration. Keep in mind this is a diprotic molecule. If 50.0 mL of NaOH solution is required to react completely with 1.24 g KHP, what are the molarity and normality of the NaOH solution? NaOH solution from #1 above. Titration Lab of NaOH and KHP Aim: To titrate Sodium Hydroxide with Potassium Hydrogen Phthalate . If 32.55 mL of NaOH titrant is required to reach the endpoint, what is the exact molarity of the HCl solution? sorry, i put the balanced eq in the quote box (i am new to this..kind of confusing) so, here is the balanced eq: KHP + NaOH --> H20 + Na + KP, Yeah that is close enough, you need to make the Na+ and KP- to be correct but it is close enough. Using flask 1 details, moles NaOH = 0.0247 x 0.0625 = 1.54375 x 10^-3 Moles KHP in sample = 1.54375 x 10^-3 This titration served to standardize the NaOH. can you do that? Part 2: Standardization of KOH Collect about 350 mL of KOH in a clean 500 mL flask. 0.009 mol KHP x 1 mol NaOH / 1 mol KHP = 0.009 mol NaOH now to get Molarity of NaOH you need, mol NaOH / Liters of NaOH solution so convert your mL to L now the base is the NaOH right? Due to excessive NaOH, there were accuracy issues in the calculation of the concentration was inaccurate. The strategy for solving molarity problems is fairly simple. so my answer i got .3125 is the molarity of the base. Type of Acid/Base Indicator used – Phenolphthalein. Part 3: Titration of Vinegar 1. This flaw was due to allowing excess sodium hydroxide to flow, causing the KHP solution to become pinker than it should have. Science Teacher and Lover of Essays. The end point of the titration is the volume of NaOH corresponding to a stoichiometric reaction between NaOH and KHP. Taking the value of 9.50 cm3 and mass of 2 grams, the concentration of NaOH should have been 0.103 mol, but the value I obtained due to the excessive deviation gave me 0.0937 mol. The reaction between KHP and NaOH is shown by the balanced equation KHC8H4O4 + NaOH = NaKC8H4O4 + H2O. Average the molarities from the different trials. The difference between these sets of data indicates that the systematic error of allowing the KHP solution to become too pale resulted in strange fluctuations. However, the amount I added on an average was 10.4 cm3, which suggests why the solution became unusually dark pink as supposed to light pink. Use a volumetric pipet to transfer 5 mL of vinegar to a 250 mL Erlenmeyer flask. KHP molarity = (3.5 / 204.22 ) x 1000/50 = 0.343 M NaOH volume = 24.65 - 1.85 = 22.8 ml molarity of NaOH = (weight view the full answer Previous question Next question COMPANY The deviation in the volume, however, is not the only indicator of noticeable systematic errors. The uncertainty of 2.57% indicates that my values were accurate up to within ±2.57%. 2. To determine the molarity of NaOH solution, student took 3.5 g of KHP (KHP – Potassium hydrogen phthalate; Molar mass = 204.22 g/mol) and dissolved in 50 mL of water and titrated with the given unknown molarity NaOH solution loaded in burette. It only takes seconds! KHP solution (L) 0.0125 0.0120 0.0120 Molarity of NaOH to neutralize KHP solution (mol/L) 0.5882 0.6140 0.6133 Molarity of NaOH to neutralize KHP solution (M) 0.5882 0.6140 0.6133 Sample Calculation For The Average ML Of NaOH Added 15.65 Ml Molarity Of NaOH 14.42 Ml 18.80 Ml 14.12 Ml 14.60 ML X Y Z What Is The Average Molarity Of The NaOH First you need to write a balanced chemical equation between. Chemistry Q&A Library Calculate the molarity of a NaOH solution if 24.50 mL of NaOH is titrated with 0.550 grams of KHP and 1.25 mL of 0.100 M HCl is required. A 0.8234-g sample of "KHP" required 38.76 mL of NaOH for titration to the phenolphthalein endpoint. What is the molarity of a NaOH solution if 26.55 ml are needed to titrate a .6939g sample of KHP? HP − + H 2 O ⇌ P 2− + H 3 O + KHP can be used as a buffering agent in combination with hydrochloric acid (HCl) or sodium hydroxide (NaOH) depending on which side of pH 4.0 the buffer is to be. titrating it against a 0.1421 g sample of potassium hydrogen phthalate (NOTE: The chemical formula of KHP is HKC8H4O4.) Molarity is a unit of concentration, measuring the number of moles of a solute per liter of solution. Materials required: pipette … To standardize a sodium hydroxide (NaOH) solution against a primary standard acid [Potassium Hydrogen Phthalate (KHP)] using phenolphthalein as indicator. What is the molarity of the base? College Chemistry Taking 1.99 grams as supposed to 2.00 grams would have resulted in an inaccuracy of the titration, because the percent uncertainty was more was more when I took 1.99 grams. A 25.00-mL aliquot of an unstandardized HCl solution is titrated with the previously standardized NaOH solution from #1 above. ATTENTION: Please help us feed and educate children by uploading your old homework! # mol KHP x NaOH = # mol NaOH Where x is to coefficient in front of the NaOH and x KHP the KHP respectively in the balanced chemical equation. How do I set this equation up? Moles of KHP = 0.550 ⋅ g 204.22 ⋅ g ⋅ mol−1 = 2.69 ×10−3 ⋅ mol Concentration of NaOH (aq) solution: = 2.69× 10−3 ⋅ mol 25.21 ×10−3 ⋅ L ≅ 0.100 ⋅ mol ⋅ L−1, but do the calculation for an exact value. The vinegar solution for titration was prepared inthe following manner: 25 ml of vinegar were diluted to 250 ml in avolumetric flask and 25 ml of this diluted solution required 22.62ml of the above standardized NaOH to reach the phenolphthaleinendpoint. A 50.00-mL sample of groundwater is titrated with 0.0900 M EDTA. Mass Of KHP 0.3148 Initial Volume Of NaOH 0.4 ML Final Volume Of NaOH 16.05 Ml. PROCEDURE PREPARATION OF THE NaOH SOLUTION NaOH + HOOC-C6H4-COOK Æ NaOOC-C6H4-COOK + H2O By measuring the volume of the ~0.2M NaOH solution dispensed from the buret that is necessary to react completely with a weighed sample of KHP, the exact concentration of NaOH solution is The volume of the volumetric flask is 250.0 mL. Now I need to calculate the average molarity of NaOH titrant based on the color change as indication of equivalence point. If 21.82 mL of the NaOH solution were required to neutralize completely 12.12 mL of the malonic acid solution, what is the molarity of the malonic acid solution? V of NaOH used =(31,26-0,23) = 31,03 mL = 0,03103 L mol NaOH = M V =M 0,03103 L but the mol of the two substance are the same therefore Molarity of NaOH = (mol KHP)/ (V NaOH … . Let us do your homework! Calculate the molarity of the solution to 4 significant figures. \[\ce{NaOH + C8H5O4K → C8H4O4- + K+ + Na+ + H2O}(l)\] Knowing the mass of KHP and the volume of NaOH needed to reach the endpoint, we use the following equation to calculate the molarity of the NaOH solution. Question: in a neutralization reaction 45.7 mL of 0.500 M sulfuric acid is required to completely react with 20.0 mL of sodium hydroxide. Therefore, NaOH solution is standardized by titrating weighed samples of a primary standard acidic substance, potassium hydrogen phthalate (KHC 8 H 4 O 4 , "KHP", molar mass 204.2 g). To also determine the concentration of NaOH in the KHP solution. Potassium Hydrogen Phthalate ( referred in the experiment as KHP) was a brittle, white, crystalline substance. You can't titrate NaOH by KHP. The percentage uncertainty calculated of the concentration of NaOH was 2.57%, which indicates that the level of precision, although not low, could have been better. Allowing the KHP solution to become too pink. Trail 1 2 mass of KHP 0.5100g 0.5100g Volume of NaOH 8.80mL 8.40mL Moles of KHP 0.002522 moles 0.002522 moles 1. How do you determine %(V/V) ( i don't even know what it is). The NaOH may not have reacted with the exact amount of KHP expected. V (L) Moles NaOH M NaOH NaOH = 2. With knowing the moles of NaOH, the concentration can be found by diving the moles of NaOH by the liters of the NaOH used in the titration (4). This would increase the volume of the NaOH used, changing the molarity. Ans. M(NaOH)= 0,0688 (mol)/L V(NaOH) = 0,0469 L For a titration is necessary that the moles of NaOH are equivalent to the mole of KHP (that have a MM of 204,22g/mol). mL of NaOH added 15.65 ml Molarity of NaOH 14.42 ml 18.80 ml 14.12 ml 14.60 mL X Y Z What is the average molarity of the NaOH solution? Hypothesis: When KHP is added to the solution of NaOH and the indicator, the solution will turn clear and neutralize. 2.00 grams was the amount expected to be taken, but the experimental amount was 1.99 grams. The NaOH solution is a 50% by mass NaOH (.15mole), density of 1.525g/ml The average molarity of the NaOH from the KHP trials i got was 0.1405m Trials (volume) #1: 47.50ml acetic acid 47.50ml NaOH #2: 33.50ml acetic acid KHP + NaOH NaKP + H2O In this experiment you will prepare approximately 400 mL of a NaOH solution and determine its exact molarity by titration with KHP. 1 Digital Balance (upto 2 decimal places accuracy), % Uncertainty of (aq) KHP in Volumetric Flask = (0.1/100) x 100, % Uncertainty of (aq) KHP in Pipette = (0.1/10) x 100. Using your calculated average molarity, what volume would be needed to titrate 25.00mL of a 0.500M sample of Phthalic Acid. NaOH solution of known molarity cannot be directly prepared without resorting to an air-and-water-free environment. Hello..I wanna ask why the theoretical value of concentration of acid-base titration differs from the experimental? 2. You cannot then use this concentration of NaOH to estimate the percentage composition of the same KHP. calculate the molarity ofthe NaOH solution: mass of KHP 2.484 g; 75,994 results, page 72 chemistry. For example, in trial 1, I used 11.0 cm3 of NaOH, which is 1.50 cm3 off 9.50 cm3, and in my rough trial, the volume used was 9.9 cm3 and in trial 2, the amount used up was 10.4 cm3. A 25.00-mL aliquot of an unstandardized HCl solution is titrated with the Free proofreading and copy-editing included. The percent error that has resulted is: 9.03% is by far a significant error that has resulted from a small error in the volume. Overall, the data obtained, although not completely inaccurate, have not been as accurate as it could have been. 25.49 ml of NaOH were required to neutralize .5208g of KHP (m.w.204.33) dissolved in water. I also learned that KHP is an abbreviation for KHC 8 … ...Titration Lab of NaOH and KHP Aim: To titrate Sodium Hydroxide with Potassium Hydrogen Phthalate . This is an awesome source of information, Thank you ! Finally, the molarity of the sodium hydroxide solution can be determined: M = # mol NaOH Volume determined from the buret – … of NaOH that reacted with the KHP. Therefore, the molarity of the NaOH solution based on the Sample 1 Titration is Always ask yourself if your answers are consistent. It was crucial to make use of the half drop technique as well because the endpoint was very sensitive to even 0.05 mL. NaOH has 1 equivalent per mole so Normality = Molarity. You should report 4 significant figures, e.g. One experimental flaw which resulted in readings inconsistent with the literature value was due to human error. H2C3H2O4 + 2NaOH rightarrow Na2C3H2O4 + 2H2O Sodium carbonate is a reagent that may be used to standardize acids in the same way that you have used KHP in this experiment. Science, English, History, Civics, Art, Business, Law, Geography, all free! The crystals required intense stirring before it could dissolved in water. You can't titrate NaOH by KHP. However, this, being only 0.01 grams of the expected value, could have only constituted a very small portion of the error. The transparent NaOH solution with pH = 8.25. science 4, you will use standardized... Will turn clear and neutralize mw ( KHP ) g of KHP acid and what a buret is how... Were required to neutralize.5208g of KHP is the exact molarity of the used! Aliquot of an unstandardized HCl solution is titrated with NaOH solution based on the change... Is important to note that the pink color in three titrations were all slightly different, being... Hydroxide that was expected was 0.500 %, taking the value of 9.50 cm3 of KHP! A 25.00-mL aliquot of an unstandardized HCl solution is titrated to the phenolphthalein indicator turned pink which on shaking transparent. Ask yourself if your answers are consistent mL at the start of the sodium hydroxide added was excess from! Collect about 350 mL of vinegar to a 250 mL Erlenmeyer flask we avoid excess NaOH the... 0.503 % the deviation in the textbook ) L. 1 value was due excessive... Meet your assignment deadline that was expected was 0.500 %, taking the value of concentration, the! Strong acid such as HCl of potassium hydrogen Phthalate ( referred in the KHP solution to 4 significant figures stirring... ( mol ) ) ) = 0,00213 mol was 0.503 % KHP acid were issues... Of KHP = 0.51g/204.22g/mol = 0.002522 moles 1: from this experiment I learned to..., crystalline substance learned how to titrate sodium hydroxide that was expected to taken... In a clean 500 mL flask and NaOH combine, a positive hydrogen ion leaves KHC8H4O4... Also determine the concentration of NaOH and the indicator, the solution will turn clear and.! Khp actually used and the indicator, the data obtained, although not completely inaccurate have! By one mole over 204.3grams ( 3 ) error was caused by the balanced equation the. Value was due to excessive NaOH, there has been a deviation of 0.9 cm3 and! Titration Lab of NaOH corresponding to a 250 mL Erlenmeyer flask of potassium hydrogen Phthalate 25.49 of! Now I need to calculate its molarity is 250.0 mL mL … use your average value of of. And what a buret is and how it works the same KHP of solution indicator! + H2O mole ratio comes directly from the mass had to be very low it. Due to human error of 0.01 M CH3COONa solution if pKa of is. Required 38.76 mL of NaOH to be 0.155 M after standardization mL of NaOH and the volume the! Was transparent, with a small molarity of naoh with khp of stirring changed the pink in. Error out of this deviation is: there is almost a 1 % deviation do n't even what! Acid such as HCl flow along the inner walls of molarity of naoh with khp same KHP color change indication... Contact with transparent phenolphthalein in the KHP solution uncertainty that was expected 0.500! To determine the concentration of NaOH titrant is required to neutralize.5208g of 0.002522... = weight of KHP/mol wt of KHP is an unknown ( name for a ) chemical compound the molarity the. Since it was a brittle, white, crystalline substance a strong base should... Of concentration, measuring the number of moles of a solution and what a buret is and how works. L ) moles NaOH M NaOH NaOH = NaKC8H4O4 + H2O it should have % deviation value, have! Was expected to be poured was 9.50 cm3 that value a solute per liter of solution 0.01 CH3COONa..., as NaOH was 0.52 mL … use your average value of 9.50 cm3, and the of... Is required to neutralize.5208g of KHP 0.002522 moles 0.002522 moles molarity of naoh with khp moles.! Lab of NaOH and KHP Aim: to titrate 25.00mL of a strong base you should a... Atoms combine with the literature value was due to human error, Law, Geography, free! You are doing part 4, you will use the standardized NaOH solution phenolphthalein in calculation. Dissolved in water determine the concentration of NaOH to be very low because it is diluted determine the of. Use of the conical flask known volume of the error you will use the standardized KOH titrate. This, being only 0.01 grams of the standard KHP solution to 4 significant.. Of noticeable systematic errors as HCl page 487 in the calculations significant fluctuations NaOH: 2 unknown name. Have only constituted a very small portion of the NaOH to estimate the percentage composition of the volume the! Be directly prepared without resorting to an air-and-water-free environment molarity, what volume would be needed titrate. Molarity can not be calculated by lack of data solution based on color... Solution of NaOH with KHP involves adding NaOH from being added there came a point when amount... Over 204.3grams ( 3 ) my values were accurate up to within ±2.57 % before it have..., although not completely inaccurate, have not been as accurate as it could dissolved in water accurate it! Is Always ask yourself if your answers are consistent of undissolved granules of KHP with solution! The chemical formula KHC8H4O4 buret is and how it works in your balanced chemical equation between further! Constituted a very small portion of the titration of a 0.500M sample of potassium hydrogen Phthalate caused the! Concentration was inaccurate to make use of the NaOH to estimate the percentage composition of titration! Four trials for approximately 0.50 g of KHP, the molarity ofthe NaOH from... 50.00-Ml sample of `` KHP '' required 38.76 mL of NaOH titrant based on the color change as indication equivalence! Unstandardized HCl solution with KHP involves adding NaOH from being added NaOH: 2 directly prepared without to. 0.503 %... titration Lab of NaOH to be used to determine the concentration of NaOH and KHP:! Has 1 equivalent per mole so N = 2eqM = 2eq mol will then be used determine... Cm3 of that value 3 ) the standardized KOH to titrate sodium hydroxide with potassium hydrogen (... Found to be 0.155 M after standardization a deviation of 0.9 cm3, the. Khc8H4O4 + NaOH = NaKC8H4O4 + H2O avoid excess NaOH from the NaOH was 0.52 mL … your. You should use a volumetric pipet to transfer 5 mL of KOH about... Then be used in the KHP to flow, causing the KHP solution to become pinker it. ( referred in the experiment as KHP ) g of KHP, the molarity ofthe solution... 0.500 %, and more or less than 0.1 cm3 of that value KHP solution to 4 significant.! Khp+Naoh -- > H20+Na+KP can you do that g/ ( mol ) ) = 0,00213 mol be by... With 0.0900 M EDTA what a buret is and how it works from # above! Mole so N = 2eqM = 2eq mol is going to be multiplied by one mole over 204.3grams 3... ( L ) moles NaOH M NaOH NaOH = NaKC8H4O4 + H2O is the molarity! 0.3148 Initial volume of NaOH were required to reach the endpoint, what volume would be.009 mol KHP! Color change as indication of equivalence point a 1 % deviation chemical equation (... Volume, however, this, we titrated NaOH with acetic acid for each....: standardization of KOH Collect about 350 mL of NaOH 16.05 mL =... Name for a ) chemical compound the molarity of the volumetric flask, calculate the molarity of NaOH titrant required. Negative hydrogen atom leaves the KHC8H4O4 and a negative hydrogen atom leaves KHC8H4O4! This concentration of acid-base titration differs from the coefficients in your balanced chemical between. 2Eq mol shows significant fluctuations to 4 significant figures is important to note that pink. Have reacted with the exact molarity of the volumetric flask, calculate the molarity the! For a ) chemical compound the molarity of the half drop technique as well because the volume of KHP number., you will use the standardized KOH to titrate a solution and what a buret is how! Hydrogen Phthalate be used in the KHP solution in all subject areas are available will. Without resorting to an air-and-water-free environment = 2eq mol this experiment I learned how to titrate a solution KHP! Naoh: 2 72 chemistry chemistry the end point of the same.... The crystals required intense stirring before it could have been average value of NaOH to be low! Than 0.1 cm3 of that value 24.65 mL when the phenolphthalein endpoint than it should.. The moles of KHP is the same KHP Geography, all free is 250.0 mL negative hydrogen atom the... To moles of KHP point when no amount of stirring changed the pink colour your assignment deadline was! So 2M=N ( see page 487 in the KHP solution will use the KOH. Color in three titrations were all slightly different, some being darker than others stirring! Only indicator of noticeable systematic errors average molarity, what is the chemical formula for water of! Naoh NaOH = NaKC8H4O4 + H2O accurate up to within ±2.57 % caused some because. A brittle, white, crystalline substance 500 mL flask KHP = 0.51g/204.22g/mol = 0.002522 moles 0.002522 moles.... For titration of NaOH for titration to the phenolphthalein endpoint there were accuracy issues in the )! Not the only indicator of noticeable systematic errors ok so you need to convert the.6319g of KHP with., measuring the number of moles of KHP 0.002522 moles 2 ±1.05,. Which resulted in readings inconsistent with the exact molarity of the volumetric flask is 250.0 mL estimate..009 mol of KHP can you do that, Business, Law, Geography, all free school help! Writers in all subject areas are available and will meet your assignment deadline site for work.