moles of khp to moles of naoh

molecular equation: KHC8H4O4(aq) + NaOH (aq) KNaC8H4O4(aq) + H2O(l) How many liters (not mL) of NaOH were consumed in this titration? Image transcription text11) KHCH404 (KHP) is a monoprotic acid commonly used to standardize aqueous solutions of We have 25 mL of a 0.10 M solution of NaOH. At the equivalence point in a neutralization, the moles of acid are equal to the moles of base. Liters NaOH sol'n used. It is acidic and gives a clear, sharp end- point when titrated with sodium hydroxide and using phenolphthalein as the indicator. KHP is a weak acid, and the equation for the neutralization of K P by NaOH is Potassium sodium phthalate COOK COOK NaOH + H2O + -COONa KHP Potassium hydrogen phthalate 1. We can convert that to grams using its molar mass (180.157 grams per mole) and we get the final grams of 0.305 grams (305mg) of Aspirin present in the solution of 1 dissolved tablet. Most questions answered within 4 hours. Lorem ipsum dolor sit amet, consectetur adipiscing elit. 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 when I took 1.99 grams. Pellentesque dapibus efficitur laoreet. <> 3 0 obj Overall, the data obtained, although not completely inaccurate, is not as accurate as it could have been. Volume determined from the buret final volume of the buret minus the initial volume converted to liters.Stoichiometry and Solutions.M =molV(L). The resultant Acidic solution was transparent, with a small amount of undissolved granules of KHP. KHP can stand for potassium hydrogen phosphate, or more likely in this case, it stands for potassium hydrogen phthalate (a monoprotic acid). 4 0 obj Donec aliquet. Get a free answer to a quick problem. 0. Finally, divide the moles of $\ce{H_2SO_4}$ by its volume to get the molarity. Also, the % uncertainty of the volume of NaOH was 1.05%, taking the value of 9.50 cm3. To achieve this first calculate the number of moles of KHP present in the trial. <>/ExtGState<>/ProcSet[/PDF/Text/ImageB/ImageC/ImageI] >>/MediaBox[ 0 0 612 792] /Contents 4 0 R/Group<>/Tabs/S/StructParents 0>> 11. Full Beaker= 25. 17.56 ml of the above NaOH(aq) solution to titrate the unknown acid solution to its end How many moles of KHP are present in the sample of KHP of student A? 0.02965-0= 0 L How does neutralization reaction differ from using a buffer? The NaOH(aq) solution is then titrated against 0.1038 g First determine the moles of $\ce{NaOH}$ in the reaction. Conversely, for the titration of a weak base with strong acid, the pH at the equivalence point is less than 7 because only the conjugate acid is present. -- assuming the former, and converting to KNa2PO4, but calculations would also work equally well for converting KH2PO4 to KNaHPO4) *initially* has fewer than 4.166 mmol present as HPO4(-2) ion. <> . It is acidic and gives a clear, sharp end- point when titrated with sodium hydroxide and using phenolphthalein as the indicator. [NaOH) - mol/L Calculation for Trial 2. Lorem ipsum dolor sit amet, consectetur adipiscing elonec aliquet. point. The volumes of NaOH used up show significant fluctuations. 1 0 obj Trial mL KHP used; Moles KHP used. 1. But when it comes to anything analytical where you start to involve calculations, standardization is a must. Nam lacinia pulvinar tortor nec facilisis. The molar mass of KHP is approximately 204.22 g/mol. This is done with NaOH because its hygroscopic and readily sucks up the moisture in the air. Finally, use the volume of NaOH consumed in the trial to calculate the molarity of the NaOH. Donec aliquet. What is the concentration of the stock NaOH solution? Donec aliquet. To get the molar amount of acid used for the experiment, use its molar mass 0.5100g molar mass of KHP 1 mole KHP 204.22g = 0.0024973 moles KHP So, you know that at equivalence point, the reaction will consume 0.0024973 moles of KHP and 0.0024973 moles of NaOH, since that's what the 1:1 mole ratio tells you. Solution: As the given equation is already balanced, using mole-mole analysis, we get: moles of KHP reacted = moles of NaOH reacted molesof KH P reacted = molesof N aOHreacted ----- (x) moles = given weight/molecular weight moles = givenweight/molecularweight thus, moles of KHP reacted = 0.4150g / 204.2g .4150g/204.2g = 0.002 mol. The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. The expected % uncertainty that was expected was 0.500%, and the uncertainty I obtained was 0.503%. \[\text{moles solute} = \text{M} \times \text{L}\nonumber \]. If you're using phenolphthalein as your indicator, an excess of sodium hydroxide would cause the solution to be a brighter shade of pink than it should be at equivalence point. a. Your email address will not be published. At the end point the solution pH is 8.42. a) Calculate the concentration of the NaOH solution Track your food intake, exercise, sleep and meditation for free. Ok,KHP is a monoprotic acid. Why is neutralization a double replacement reaction? Science, English, History, Civics, Art, Business, Law, Geography, all free! 2.00 grams was the amount expected to be taken, but the experimental amount was 1.99 grams. For Free. In this case, you are looking for the concentration of hydrochloric acid (its molarity): In short, titration is all about "theoretical, complete" reactions. 2 20 0 0 26 0 0 0. What is the average concentration the NaOH solution (including all fine trials but not any In this experiment, two different titrations will be done using NaOH. As you can see, the actual molarity of the solution you prepared is relatively small compared with your target of #"0.100 M"#. Show your work. What is the concentration (in molarity) of the NaOH solution according to this trial? Nam lacinia pulvinar tortor nec facilisis. How can you determine the strength of sulfuric acid? 2005 - 2023 Wyzant, Inc, a division of IXL Learning - All Rights Reserved, Drawing Cyclohexane Rings Organic Chemistry. Fusce dui lectus, congue vel laoreet ac, consectetur adipiscing elit. Moles (nvf) of KHP in volumetric flask = mKHP/MKHP where MKHP is the Molar Mass of KHP (204.22 g), Moles of KHP in 10 cm3 of solution in where V is a given volume of water, The volume of NaOH added = Final Volume Initial Volume, [c]KHP = (n/V) mol dm-3 = (0.00974/0.1) mol dm-3 = 0.0974 mol dm-3. Now let's apply the molar ratio logic to obtain the moles Of OH-: .00278 moles of KHP means there's .00278 moles of H+, .00278 moles of H+ means the neutralized solution has.00278 moles of OH-. Since the indicator reacts with some of the titrant and the indicator may not change at the exact pH of the equivalence point, a small error in introduced in the titration. Lorem ipsum dolor sit amet, consectetur adipiscing elit. You start with #"0.5100 g"# of #"KHP"#. In this case, 2 moles of NaOH are required to titrate 1 mole of H 2 SO 4. Divide moles NaOH by volume used to get molarity (mol/L). The higher molarity of the acid compared to the base in this case means that a smaller volume of the acid is required to reach the equivalence point. This would have resulted in inaccuracies. Therefore, due to flaws in raw data values taken from systematic errors, there has been a deviation in uncertainty too, indicating the impact of methodical flaws. How do you calculate the number of moles of KHP in NaOH? 2) Determine the number of moles of KPH needed, and convert to grams First, we need to know the number of moles of NaOH we have. Initial= 29 ml Final= 3. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Nam lacinia pulvinar tortor nec facilisis. The manufacture of soap requires a number of chemistry techniques. The NaOH may not have reacted with the exact amount of KHP expected. Or, if you type your answers, We reviewed their content and use your feedback to keep the quality high. <>/ProcSet[/PDF/Text/ImageB/ImageC/ImageI] >>/MediaBox[ 0 0 612 792] /Contents 4 0 R/Group<>/Tabs/S/StructParents 0>> How many moles of KHP were titrated in this trial? You start with 0.5100 g of KHP . M= moles/liter, so we have 25 mL of a 0.10 mole/liter solution. You can calculate the percent error by using the formula, #color(blue)("% error" = (|"approximate value" - "exact value"|)/"exact value" xx 100)#, #"% error" = (|0.07878 - 0.100|)/0.100 xx 100 = 21.22%#. However, there has been a deviation of 0.9 cm3, which is significant, but not high. 100/20= 5. Moles NaOH used. endobj Odesha D. answered 11/20/13, Andre W. 204 x 100 = 2, How many moles of KHP are in the standard? This tells you that at you can reach the equivalence point by reacting equal number of moles of KHP and of NaOH . As you know, molarity is defined as moles of solute per liters of solution. Therefore, the moles of KHP is equal to the moles of NaOH. We know this because the equivalence point is where the moles of the NaOH Show your work. These errors were avoidable. Lorem ipsum dolor sit amet, consectetur adipiscing elit. Your starting point here is the balanced chemical equation for this neutralization reaction, #"KHP"_text((aq]) + "NaOH"_text((aq]) -> "KNaP"_text((aq]) + "H"_2"O"_text((l])#. NaOH + C8H5KO4-->NaC8H4KO4 + H2O. 2.752 x 10-1 mol 2.693 x 10-2 mol 2.693 x 10-3 mol 3.712 x 102 mol. Because the conjugate base of a weak acid is weakly basic, the equivalence point of the titration reaches a pH above 7. 1.54g of KHP is equivalent to 0.00754 mol of KHP. Making educational experiences better for everyone. Nam lacinia pulvinar tortor, inia pulvinar tortor nec facilisis. As you start adding the NaOH, and converting it eventually to K3PO4, any bits that were initially present as H2PO4(1-), or PO4(3-), or H3O(1+), or OH(1-), will all "come out in the wash". Fusce dui lectus, congue vel laoreet ac,gue vel laoreet ac,gue, rem ipsum dolor sit amet, consectetur adipiscing elit. xZ_GX+Rp$M{\](}c;jK$^>VI-YE`["o~34{=>q,\.{~yG`/o8g"0&A}/~;_qq|!fySY,/"l=_Hy;W\/=d/yhZ9UT)Ue+qok~4ip'oVF8GTz?DQu u0bq9I rB~5{7vO The important thing to notice here is that you have a #1:1# mole ratio between the two reactants. As the transparent NaOH solution came into contact with transparent phenolphthalein in the KHP solution, it turned pink which on shaking became transparent. Pella. answer questions 6-11. One experimental flaw which resulted in readings inconsistent with the literature value was due to human error. endobj Choose one fine trial done, and use it to Has two protons (diprotic) - need twice the amount of base as a monoprotic acid would need to be . The above equation works only for neutralizations in which there is a 1:1 ratio between the acid and the base. is a procedure used to compare the amount (moles) of acid in one sample with the amount (moles) of base in another. pdf, Gizmos Student Exploration: Effect of Environment on New Life Form, Ejemplo de Dictamen Limpio o Sin Salvedades, Leadership class , week 3 executive summary, I am doing my essay on the Ted Talk titaled How One Photo Captured a Humanitie Crisis https, School-Plan - School Plan of San Juan Integrated School, SEC-502-RS-Dispositions Self-Assessment Survey T3 (1), Techniques DE Separation ET Analyse EN Biochimi 1, Reproduce your KHP standard data. Next, we are able to determine the concentration of the NaOH solution by doing the following: How do you do acid base neutralization reactions? Nam lacinia, usce dui lectus, congue vel laoreet ac, dictum vitae odio. #color(blue)(|bar(ul(color(white)(a/a)c = n_"solute"/V_"solution"color(white)(a/a)|)))#. <> 0 moles Scholarship Chem. KOOC COOH -c. CH C H i emochila m ohon FIGURE 5.1 Potassium hydrogen phthalate (KHC8H404) abbreviated as 'KHP KHP is available in high purity and is soluble in water. [NaOH] = mol/L Calculation for Trial 3 (NaOH) = mol/L Use your two results that are in closest agreement to each other and calculate an average result. Lorem ipsum dolor sit, ac, dictum vitae odio. moles HCl = moles NaOH Acid-Base Titration Solution Molarity (M) is moles per liter of solution, so you can rewrite the equation to account for molarity and volume: M HCl x volume HCl = M NaOH x volume NaOH Rearrange the equation to isolate the unknown value. You know the number of moles of NaOH, because it's the same as the number of moles of KHP. 1 mole of NaOH reacts per mole of KHP, so .00754 mol of NaOH are needed. First you need to write out the balanced equation to determine the mole ratio between C8H5KO4. From the mole ratio, calculate the moles of $\ce{H_2SO_4}$ that reacted. The theoretical value of the Sodium Hydroxide that was expected to be used was 9.50 cm3. Nam risus ante, dapibus a molestie consequat, ultrices ac magna. The resultant Acidic solution was transparent, with a small amount of undissolved granules of KHP. Step 1: Calculate the amount of sodium hydroxide in moles Amount of solute in mol = concentration in mol/dm 3 volume in dm 3 Amount of sodium hydroxide = 0.100 0.0250. Show You do answered 07/11/19, Experienced Pres. How many moles of NaOH were consumed in this trial? At the equivalence point in an acid-base titration, moles of base = moles of acid and the solution only contains salt and water. These fluctuations caused the 0.95% error. This mass of KHP along with the mass of sample used in the titration allows . The balanced chemical equation for the neutralization of KHP with the base NaOH indicates that the stoichiometric molar ratio is 1. Grad For Math and Science Tutoring. x\[s~L& Ng's:;-HT_v@II{^|.dR~|Ud>?.w_W1"^%7Wg1ec? So the steps are grams KHP to moles KHP to mmol KHP to mmol NaOH to ml NaOH as your final answer: 0.8508 g KHP(1mol/204.22g)(1000mmol/1mol)(1mmol NaOH/1mmol KHP)(1ml NaOH/0.2535mmol)= 16.43ml. So, the pH is 7. Lorem ipsum dolor sit amet, consectetur adi, trices ac magna. To titrate it to the equivalence point, we need an equal amount of NaOH: 4.166 mmol of NaOH. [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. stream 17.20 ml of a solution of NaOH(aq). Fusce dui lectus, congue vel laoreet ac, dictum vitae odio. {}Oqq=vq.L, v1? =_Q1{Ox#1#cdw~-g"qy]F$bM@(JzEAtDC:H.,B?k=hV'K"g~F`ZYZ?fq2Vh5?N4pddL{4yQKsf)3^9"N\X$b:4Kna|:4~Ys-ISE How do you know? strong bases. The resulting percentage error out of this deviation is: There is almost a 1% deviation. One must assume that the KHP referred to is potassium hydrogen phthalate, and not potassium hydrogen phosphate, otherwise the molar mass would be incorrect. A student weighs out 0.568 g of KHP (molar mass = 204 g/mol) and titrates to the equivalence point with 36.78 mL of a stock NaOH solution. Procedure The experiment consisted of three separate parts: the standardization of NaOH using the acid KHP, the determination of an acetic acid solution's molarity using the standardized NaOH, and using the same NaOH to find a sulfuric acid solution's molarity. How do you find the concentration of NaOH? Nam lacinia, iscing elit. Introduction Sodium hydroxide is hygroscopic and absorbs water from the air when you place it on the balance for massing. endobj mol KHP= (0,436g)/(204,22 (g/(mol))) = 0,00213 mol . From mole ratio, number of moles of NaOH = 0.00979 mol. The equivalence point is the mid-point on the vertical part of the curve. Choose an expert and meet online. I assumed KHP was a potassium phosphate, but was troubled by a completely incorrect formula. The example below demonstrates the technique to solve a titration problem for a titration of sulfuric acid with sodium hydroxide. . However, as NaOH was added further, there came a point when no amount of stirring changed the pink colour. Ok,KHP is a monoprotic acid. Show your work. This is the amount of base needed to hydrolyze a certain amount of fat to produce the free fatty acids that are an essential part of the final product. Do not round off any intermediate results during this multi-step calculation . Fill in the Table below with the information from questions 6-11 as Trial 1. Molarity = moles of solute/Liters of solution. Why do neutralization reactions produce heat? save as a .pdf and upload to Gradescope. Donec alique, ultrices ac magna. English 123- 3-4 Assignment Submission- Annotating Your Sources, Marketing Reading-Framework for Marketing Strategy Formation, Recrystallization of Benzoic Acid Lab Report, Tina Jones Heent Interview Completed Shadow Health 1, Essentials of Psychiatric Mental Health Nursing 8e Morgan, Townsend, Entrepreneurship Multiple Choice Questions, Calculus Early Transcendentals 9th Edition by James Stewart, Daniel Clegg, Saleem Watson (z-lib.org), SCS 200 Applied Social Sciences Module 1 Short Answers, Ati-rn-comprehensive-predictor-retake-2019-100-correct-ati-rn-comprehensive-predictor-retake-1 ATI RN COMPREHENSIVE PREDICTOR RETAKE 2019_100% Correct | ATI RN COMPREHENSIVE PREDICTOR RETAKE, 1.1 Functions and Continuity full solutions. After hydrolysis is complete, the leftover base is titrated to determine how much was needed to hydrolyze the fat sample. Make sure the conical flask is directly under the pipette, with no contact with the inner walls, so as to get a more accurate measure of the volume. Fusce dui lectus, congue vel laoreet ac, dictum vitae odio. Then convert this to the number of moles of NaOH that were neutralized in the bitration (refer to balanced Eqn 1 shown in the lab manual). Donec aliquet. KHP is slightly acidic, and it is often used as a primary standard for acidbase titrations because it is solid and air-stable, making it easy to weigh accurately. Donec aliquet. 10 grams KHP to mol = 0.14069 mol 20 grams KHP to mol = 0.28137 mol 30 grams KHP to mol = 0.42206 mol 40 grams KHP to mol = 0.56275 mol 50 grams KHP to mol = 0.70343 mol 100 grams KHP to mol = 1.40687 mol 200 grams KHP to mol = 2.81373 mol Want other units? endobj Number of moles of KHP in 2.00 grams = (m/M) = (2/204.22) mol = 0.00979 mol, Number of moles of KHP in 0.01 dm3 of solution in conical flask = [c] x V. From the mole ratio, the number of moles of NaOH = 0.00979 mol. Based on this equation, we need one mole of KPH to react with each mole of NaOH. This is an awesome source of information, Thank you ! Empty Beaker= 23. Nam risus ante, dapibus a molestie consequat, us a molestie consequat, ultrices ac magna. With 0.2535 mmol/mL of NaOH, we need a volume of 4.166 mmol/(0.2535 mmol/mL)=16.43 mL. Nam lacinia pulvinar t, facilisis. 1. When the endpoint is reached the addition of titrant should be stopped. Lorem ipsum dolor sit amet, coce dui lectus, congue vel laoreet ac, dictum vitae odio. 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. YouTubeYouTubeStart of suggested clipEnd of suggested clipAnd youre going to look at where they intersect or cross over rather not intersect. To get the molar amount of acid used for the experiment, use its molar mass, #0.5100color(red)(cancel(color(black)("g"))) * overbrace("1 mole KHP"/(204.22color(red)(cancel(color(black)("g")))))^(color(purple)("molar mass of KHP")) = "0.0024973 moles KHP"#. A sample of 354.5 mg of KHP is added to water, which is then neutralized by Our answer is 0.01692 moles of NaOH added and the same number of moles of Aspirin neutralized. moles of NaOH used = moles of KHP moles of NaOH used = (Volume of NaOH used)* (Concentration of NaOH) You have not specified a concentration, so be it, concentration of NaOH = 0.05 mol/L. strong bases. Related Textbook Solutions <> If the concentration is different, it must be replaced. As the transparent NaOH solution came into contact with transparent phenolphthalein in the KHP solution, it turned pink which on shaking became transparent. : an American History (Eric Foner), Chemistry: The Central Science (Theodore E. Brown; H. Eugene H LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward), Campbell Biology (Jane B. Reece; Lisa A. Urry; Michael L. Cain; Steven A. Wasserman; Peter V. Minorsky), Principles of Environmental Science (William P. Cunningham; Mary Ann Cunningham), Civilization and its Discontents (Sigmund Freud), Psychology (David G. Myers; C. Nathan DeWall), Business Law: Text and Cases (Kenneth W. Clarkson; Roger LeRoy Miller; Frank B. of an unknown monoprotic acid dissolved in water to a final volume of 50.00 mL. around the world. At the equivalence point in a neutralization, the moles of acid are equal to the moles of base. 35,000 worksheets, games, and lesson plans, Marketplace for millions of educator-created resources, Spanish-English dictionary, translator, and learning, Diccionario ingls-espaol, traductor y sitio de aprendizaje, a Question %PDF-1.5 Nam lacinia pulvinar tortor nec facilisisonec aliquet. \[\ce{H_2SO_4} \left( aq \right) + 2 \ce{NaOH} \left( aq \right) \rightarrow \ce{Na_2SO_4} \left( aq \right) + 2 \ce{H_2O} \left( l \right)\nonumber \]. The above equation can be used to solve for the molarity of the acid. Nam lacinia pulvinar tortor nec facilisis. It corresponds to a volume of NaOH of 26 mL and a pH of 8.57. moles KHP = _____mass KHP_____ MW KHP (204.22 g/mol) 2. The grams required can be obtained by multiplying the moles of NaOH by the molecular weight of KHP. Cross), Forecasting, Time Series, and Regression (Richard T. O'Connell; Anne B. 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Tutor and Freelance Writer. 2.04/204= 0 moles, What is the molarity of the standard? 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. When KHP and NaOH combine, a positive hydrogen ion leaves the KHC8H4O4 and a negative hydrogen atom leaves the NaOH. \[\text{M}_A \times \text{V}_A = \text{M}_B \times \text{V}_B\nonumber \]. rough or overshot trials)? In this laboratory exercise you will carry out such a titration to. Calculate the concentration of the NaOH solution. moles of NaOH used = (0.0131 L)* (0.05 mol/L) = 0.000655 moles The process of calculating concentration from titration data is described and illustrated. moles of KHP are equivalent to moles of NaOH. 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). Fusce dui lectus, congue vel laoreet ac, dictum vitae odio. Fusce dui lectus, congue vel laoreet ac, dictum vitae odio. Molarity of NaOH = (mol KHP)/ (V NaOH used for titration): M(NaOH)=0,00213mol0,03103L=0,0688molL . Equivalence point: point in titration at which the amount of titrant added is just enough to completely neutralize the analyte solution. Lorem ipsum dolor sit amet, consectetur adipiscing elit. diprotic and requires twice the number of moles of NaOH expected for a monoprotic acid. Learn how to calculate the mass of KHP (potassium hydrogen phthalate) to standardize a NaOH (sodium hydroxide) solution. - use appropriate significant figure rules and report the result with the proper amount of precision K:39.10 H:1.008 C(8):96.08 molar mags H4):4.032 0(4):64 204.22 g/mol MDL May 2017 KHP_REP 204.22 - g/mol continued on back OXB endobj 1. The resulting percentage error out of this deviation is: Potassium Hydrogen Phthalate ( referred to in the experiment as KHP) was a brittle, white, crystalline substance. Nam risus an, ultrices ac magna. Donec aliquet. 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. endobj So, you know that at equivalence point, the reaction will consume #0.0024973# moles of #"KHP"# and #0.0024973# moles of #"NaOH"#, since that's what the #1:1# mole ratio tells you. However, as NaOH was added further, there came a point when no amount of stirring changed the pink colour. At any rate moles acid present = 0.568 g x 1 mol/204 g = 0.002784 moles acid, moles NaOH needed to neutralize = 0.002784 moles NaOH since balanced equation shows 1:1 mole ratio, Molarity of the NaOH = moles/liter = 0.002784 moles/0.03678 L = 0.07570 M = 0.0757 M (3 sig. of an unknown monoprotic acid dissolved in water to a final volume of 50.00 mL. Recall that the molarity $\left( \text{M} \right)$ of a solution is defined as the moles of the solute divided by the liters of solution $\left( \text{L} \right)$. total volume of solution. Nam risus ante, dapibus a molestie consequat, ultrices ac magna. Pellentesque dapibus efficitur laoreet. Finally, divide the moles of $\ce{H_2SO_4}$ by its volume . This will be a strong base - weak ac. a) Calculate the concentration of the NaOH solution Donec aliquet. The volume of $\ce{H_2SO_4}$ required is smaller than the volume of $\ce{NaOH}$ because of the two hydrogen ions contributed by each molecule. Fusce dui lectus, congue vel laoreet ac, dictum vitae odio. 7.50 X 10 -2 moles X 204.22 g KHP/ 1 mole = 15.3 g KHP He found out that it required 18.5 mL of NaOH to reach the endpoint of the titration. We can then set the moles of acid equal to the moles of base. Nam lacinia pulvinar tortor nec fague,

ur laoreet. A link to the app was sent to your phone. The value of Ka from the titration is 4.6. Potassium Hydrogen Phthalate ( referred to in the experiment as KHP) was a brittle, white, crystalline substance. The theoretical value of NaOH to be poured was 9.50 cm3, and more or less than 0.1 cm3 of that value. Only one of the hydrogen atoms in KHP has acidic properties. The data from the titration is then used to calculate the molarity of the NaOH. Most questions answered within 4 hours. You get .00278 moles of KHP. A sample of 354.5 mg of KHP is added to water, which is then neutralized by In order to determine the exact concentration of a sodium hydroxide solution you must standardize it by titrating with a solid acid that is not hygroscopic. 0:586:27How to Determine the Equivalence Point from a Graph. Lorem ipsum dolor sit amet, consectetur adipiscing elit. (NaOH) = ( g KHP)( 1 mol KHP / 204.23 g) ( 1 mol NaOH / 1 mol KHP) / (V L of NaOH) (0.905 g KHP) ( 1mol KHP ) ( 1mol __ ) = 0.00443 . Donec aliquet. Final burette reading. converted to moles of KHP used in the reaction, and then the grams of KHP present in the previously weighed sample can be determined. The crystals required intense stirring before they could be dissolved in water. Nam lac, sque dapibus efficitur laoreet. 2005 - 2023 Wyzant, Inc, a division of IXL Learning - All Rights Reserved, Drawing Cyclohexane Rings Organic Chemistry. An acid-base . To find molarity (concentration = mol/L), convert the 36.78ml of NaOH into L, and divide this into .00278 moles of NaOH J.R. S. Total Volume= 100 ml, What is the mass of KHP in the standard? Pell

The percent error that has resulted in: 9.03% is by far a significant error that has resulted from a small error in the volume. Lorem ipsum dolor sit amet, consectetur adipiscing elit. not need to show your work for additional trials; just populate the table. 59547 views RAW DATA MASSES Trial #1 Trial #2 Trial #3 mass of KHP weighed out: 0.6096_9 _0.6088_9 0.6022_9 VOLUMES burette reading: FINAL 32.65_ m _33.49_ML_30.47ML burette reading: O INITIAL 3.09 mL 4.29 ML 1.19 mL Volume of NaOH used: minus 0 29.56 mL 29.20 ml 29.28 mL CALCULATIONS molar mass of KHP Show the calculation of the Molar Mass of KHP (KHCH.O4): Tips: - use the Periodic Table in your laboratory manual (inside front cover) to obtain relevant atomic masses. Nam risus ante, dapibus a molestie conse, onec aliquet. % Uncertainty of (aq) KHP in Volumetric Flask = (0.1/100) x 100. 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).

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