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During NaOH + H2SO4 titration we should use Phenolphthalein as the indicator for the acid-base titration. The use of volumetric flask, burette and pipette in determining the concentration of NaOH solution. and sodium hydroxide had the neutral pH at the equivalence point, being 7. The solubility of sodium chloride does not change much with temperature, so simply cooling the solution is unlikely to form crystals. Then the samples of Introduction The titration of a weak acid with a strong base involves the direct transfer of protons from the weak acid to the hydoxide ion. 2a Determination of the reacting volumes of solutions of a strong acid and a strong alkali by titration. By observing the titration of a strong acid and strong base and a strong, base and weak acid one can see how the shapes in the titration curves dif, moles of acid and base have been added. How do I calculate the concentration of sulphuric acid by a titration experiment with sodium hydroxide? 0000004174 00000 n All of these are of course desirable traits to be developed in students, but there has to be some degree of basic competence and reliability before using a burette with a class. Na+ ions form ionic bonds with sulphate ions to form Na2SO4 (salt). The HCl solution, added with a few drops of phenolphthalein, is placed into the Erlenmeyer flask and the NaOH solution is slowly added from the burette into the HCl solution in small drops. The goal of the experiment is to examine how the rate of reaction between Hydrochloric acid and Sodium thiosulphate is affected by altering the concentrations. Suppose that a titration is performed and 20.70 mL of 0.500 M NaOH is required to reach the end point when titrated against 15.00 mL of HCl of unknown concentration. In part two of the experiment 3 samples of impure KHP were obtained all weighing Apparatus for titrating sodium hydroxide with hydrochloric acid to produce sodium chloride. We then calculated the average volume at each temperature. Will this affect the amount of NaOH it takes to neutralize a given amount of sulfuric acid? 2 3 3 () + () .() + 2 3 3 () (2) You will be using the buret calibrated in Part 1 of this exercise and the data provided in Table 2 report the standardized concentration of the NaOH solution. Thus, it can be inferred that the molarity is proportional to the mL of HCl dropped. Hydrochloric acid, a strong acid was used with sodium hydroxide a strong, base. time of the indicator color change and the time at the equivalence point agree? After finding the mean of the concentration, the standard deviation was found to be 0. We used a Buchner funnel to collect benzocaine. The process of balancing chemical equations involves matching the number of atoms in a reactant and product. Lets take an example of NaOH + H2SO4 titration for determining the concentration of NaOH or H2SO4. By clicking Accept all cookies, you agree Stack Exchange can store cookies on your device and disclose information in accordance with our Cookie Policy. unknown KHP sample. Titration is a crucial laboratory technique used to determine the concentration of an unknown solution, and the use of a pH indicator allows scientists to visually determine the equivalence point, at which the . The reading obtained for the first experiment has a big difference when compared to the other three readings. Button opens signup modal. 0000005620 00000 n Had the mL of HCl recorded been a little larger, the molarity of the solution would be larger, whereas if it were smaller, the molarity would be smaller. neutral at the equivalence point. Learn more about Stack Overflow the company, and our products. Practical experiment where learners produce gold coins by electroplating a copper coin with zinc, includes follow-up worksheet. 0000017322 00000 n The concentration of the solution does not need to be made up to a high degree of accuracy, but should bereasonably close to the same concentration as the dilute hydrochloric acid, and less than 0.5 M. Dilute hydrochloric acid, HCl(aq) see CLEAPSSHazcardHC047a and CLEAPSSRecipe Book RB043. In a titration of sulfuric acid against sodium hydroxide, 32.20mL of 0.250MNaOH is required to neutralize 26.60mL of H 2SO 4. Trail 1 0 33 0 2. What questions could I answer and elaborate on in my acid base titration lab conclusion We used NaOH base amp H2SO4 acid Acid and base titration lab report CTC Software March 29th . Titrating V#z\stWUp:(j7 L1 %kx$3 combinations is pH=9 on the vertical region? What PHILOSOPHERS understand for intelligence? The results do not support the hypothesis that a higher surface area to volume ratio would result in sulphuric acid being diffused into the agar cubes in the shortest amount of time. This process is performed three times. The titration reaction of KHP with NaOH is as follows: \[\ce{C8H5KO4 (aq) + NaOH (aq) H2O + C8H4NaKO4 (aq)}\nonumber\]. The volume of acid used in this experiment is 25 cm. 0000002062 00000 n Each activity contains comprehensive information for teachers and technicians, including full technical notes and step-by-step procedures. Practical Chemistry activities accompanyPractical PhysicsandPractical Biology. That means the number of moles of sulfuric acid used is half that of sodium hydroxide. Another reason is that we did not catch the end point. However, if you wanted to solve for moles of $\ce{H2SO4}$ in $50~\mathrm{mL}$, you would have to multiply the number of moles in the $10~\mathrm{mL}$ sample by $5$. 0000005963 00000 n Then, we did reflux for 75 minutes. That means number of moles of sulfuric acid is half that of number of moles of sodium hydroxide used. Phenolphthalein indicator is used to determine the end-point of the titrated solution. By using the ionic equation, we can find out the spectator ions by splitting each reactant and product molecule. There was also no consistent trend evident in the results. However, the dishes should not be allowed to dry out completely, as this spoils the quality of the crystals. This is evident in the results as the exact opposite to what was predicted occurred. We used three 10 ml of water to wash the product. . The information collected The buret was A primary standard is characterized as a reagent of higher purity and is typically a stable solid such that a measurement of mass accurately representative of the number of moles of the standard. Become Premium to read the whole document. It was made by adding According to our results, all the readings fell far short of the original reading. The volume of the solution was then calculated by subtracting the initial volume from the final volume. If a third titration was required, average the two closest values. (review sheet 4), (8) Making freebase with ammonia cracksmokers, Entrepreneurship Multiple Choice Questions, Assignment 1 Prioritization and Introduction to Leadership Results, Wong s Essentials of Pediatric Nursing 11th Edition Hockenberry Rodgers Wilson Test Bank, Who Killed Barry mystery game find out who killed barry, Philippine Politics and Governance W1 _ Grade 11/12 Modules SY. Add the hydrochloric acid to the sodium hydroxide solution in small volumes, swirling gently after each addition. Use this practical to investigate how solutions of the halogens inhibit the growth of bacteria and which is most effective. 5.9C Carry out an accurate acid-alkali titration, using burette, pipette and a suitable indicator, 3.18 Describe how to carry out an acid-alkali titration, using burette, pipette and a suitable indicator, to prepare a pure, dry salt. Acid + Base Salt + water(Neutralization reaction), When strong acid(H2SO 4)reacts with a strong (NaOH) base a neutralization reaction is observed. Titration Of Acids Bases Lab Report Answers YouTube. With knowing the moles of NaOH, the We can calculate ionic reaction as follows: Na+ + (OH) + 2H+ + (SO4)2- Na+ + HSO4 + H2O. Whe, The pH indicator used in this lab was phenolphthalein which is clear in acidic soluti, in basic solutions. This experiment taught the skill of how to perform a proper titration, and how salts act in : an American History - Chapters 1-5 summaries, Analytical Reading Activity 10th Amendment, 446939196 396035520 Density Lab SE Key pdf, Test Bank Varcarolis Essentials of Psychiatric Mental Health Nursing 3e 2017, 1.1 Functions and Continuity full solutions. Mandatory eexperiment 4.2A - A hydrochloric acid/sodium hydroxide titration, and the use of this titration in making the sodium salt. = = >? Trial 3 0 31 0 2. . This is because NaOH is very hygroscopic. sample of potassium hydrogen phthalate, also known as KHP. This is a titration of sulfuric acid with sodium hydroxide with the pH graphed as the experiment progresses. Burets are commonly used when performing titration reactions. How do I solve for titration of the $50~\mathrm{mL}$ sample? Acid-base titration is a method often used to determine the concentration of a basic solution, given the concentration of an acidic solution is known and vice versa. Titration is a laboratory analytical method to determine the concentration of a solution or a reactant when the concentration of another solution is known. instead of hydroxide. 1. To obtain the moles of Calculate the molarity of a sodium hydroxide solution if 25.00 mL 0.100 M maleic acid requires 22.10 ml of NaOH to reach the endpoint. However, if you wanted to solve for moles of $\ce{H2SO4}$ in $50~\mathrm{mL}$, you would have to multiply the number of moles in the $10~\mathrm{mL}$ sample by $5$. @A (3) resulted in a faint pink the procedure of titration was repeated three times. KHP is commonly used as a primary standard because it is a solid at room temperature, is stable in air, and is not hygroscopic, which makes it possible to accurately determine the mass of KHP using a balance. In practice it does not matter if the end-point is overshot, even by several cubic centimetres, but the aim is to find the proportions for a roughly neutral solution. The experiment required a solution to be made to use as the base. Finding valid license for project utilizing AGPL 3.0 libraries. Titration of H2SO4 w NaOH: Solving for the molarity of H2SO4? Sodium sulphate is salt(product of neutralization reaction). 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. titration curves found in the chemistry with vener folder. When the solid KHP is dissolved Question 6: How should the concentration of NaOH be reported? Discussion According to our results above, the readings obtained for the 4 titrations are not very constant. Which combinations of acid and base have the lower initial pH values? So you get 2 moles of NaOH for every 1 mole of H2SO4. Obviously I can use the formula: 69 sec 99 sec 8 2 11. This is critical in successfully conducting both fundamental and applied research as well as quality control measures in various industries. Is this problem about acid-base titration wrong? From this lab, we proved the validity of the rules of stoichiometry and the molarity formula, while also seeing firsthand the neutralization of a substance through an acid-base reaction. For which acid-base combinations does the strong acid with sodium hydroxide, a strong base and acetic acid, a weak acid with sodium The titration results using standardized NaOH solution are listed in Table 2. You should consider demonstrating burette technique, and give students the opportunity to practise this. Yes, it is a complete reaction, NaOH + H2SO4 Na2SO4 + Hb>2O. The What screws can be used with Aluminum windows? What is the pH at both equivalence points of titration between diprotic tartaric acid and NaOH? of NaOH in We used Pasteur pipet to add concentrated sulfuric acid (1.0 mL) to the flask. I am given $\ce{H2SO4}$ in a reaction vessel of about $50~\mathrm{mL}$. The NaOH is dissolved by filling the volumetric flask to the mark. ** (The "end point" of a titration is the point in the titration at which an indicator . 514 24 75mL of sodium hydroxide and approximately 675mL of DI water into a 1L Nalgene bottle. NaOH (aq) + HCl (aq) NaCl (aq) + H2O (l) Using a small funnel, pour a few cubic centimetres of 0.4 Mhydrochloric acid into the burette, with the tap open and a beaker under the open tap. Improving the copy in the close modal and post notices - 2023 edition, New blog post from our CEO Prashanth: Community is the future of AI. 4. Question 2: Why might mass measurements using an analytical balance to measure about 25 g of water be considered more accurate than a volume measurements of 25 mL with volumetric glassware, such as burets or transfer pipets? Figure A3: The LoggerPro graph of the CH 3 COOH and NaOH titration. Then they were gently warmed until all the impure KHP was dissolved. Manage Settings reaction it very close to the equivalence point, which means the moles or acid with be the same repeated two more times with the other sample. Sodium hydroxide solution, NaOH(aq), (IRRITANT at concentration used) see CLEAPSS HazcardHC091a and CLEAPSS Recipe BookRB085. This collection of over 200 practical activities demonstrates a wide range of chemical concepts and processes. What is the cost of 1.00 g of calcium ions as provided by this brand of dry milk? identify with pH indicator works best. As with Part 1, it is recommended that you utilize Microsoft Excel to manipulate data and perform the necessary mathematical operations. Introduction: Acid-Base titration labs are often done to determine the amount or concentration of an acid or base in a substance. This may be cause by the extra amount of phenolphthalein indicator added into the acid, causing it to turn pink faster. pKa = 5.4 What follows here assumes that teachers have judged the class to be capable of doing this experiment using a burette with reasonable expectation of success. The equation is now a balanced chemical equation. Can we create two different filesystems on a single partition? We swirled the mixture until the solid dissolved completely. Abstract: The purpose of this experiment is to observe the titration of hydrochloric acid, a The experiment is also part of the Royal Society of Chemistrys Continuing Professional Development course:Chemistry for non-specialists. Summary: Prepare a single PowerPoint slide or Word document that summarizes the key results or points from this exercise. This will find the molarity of the $10~\mathrm{mL}$ sample of $\ce{H2SO4}$. We added sodium carbonate until the pH of the mixture was 8. Note that the first measurement for each trial is the starting volume of water in the buret and prior to delivering any water to the flask. After reflux, we removed the reaction mixture from the apparatus and cooled it for several minutes. 0000004792 00000 n Asking for help, clarification, or responding to other answers. E:w00LYygrT*pH85[$D,CIK]?::@F.PP3DAC&60GP6=cAng``^vh`P0X0(6I10= F= Acid and base titrations are an extremely common approach to using stoichiometry to quantitatively measure the concentration of an analyte in solution. HC 9 H 7 O 4 + NaOH ---> H 2 O + Na(C 9 H 7 O 4). Connect the ph sensor to the computer and on the loggerpro program open file 23: Carefully add the same volume of fresh hydrochloric acid as you used in stage 1, step 3,to another 25 (or 20) cm, Pour this solution into an evaporating basin. As the net ionic equation is 2H+ + 2(OH) 2H2O. Homework Equations Balanced chemical equation: H2SO4 + 2NaOH --> 2H2O + Na2SO4 [NaOH] = 0.0939M The Attempt at a Solution I determined the amount of diluted H2SO4 to be 18.9 mL (I used 18 mL) 20mL NaOH(1L/1000mL)(0.0939M NaOH)(1 mol H2SO4/2 mol NaOH) = 0.0945M H2SO4 Molarity is the number of moles in a Litre of solution. two lists the same? flask by drops until the solution resulted in a faint pink. If crystallisation has occurred in shallow solution, with the crystals only partly submerged, hopper-shaped crystals may be seen. happens instantaneously when they are mixed. I need to solve for the molarity of $\ce{H2SO4}$. Use basic output from an analytical tool (buret) to calibrate that tool. Awesome A-Level Chemistry Essays & Coursework Examples that have been Marked by Teachers and Peers allowing for the best possible results. Question 5: If random or systematic errors are observed, hypothesize a source of the error(s). 0 The following data were collected in the titration of 10.0 mL of 0.10 M weak acid, HA, with 0.10 M NaOH . REFERENCES Experiment #10/11:Part 1 Acid Base Titration. In this experiment a pipette is not necessary, as the aim is to neutralise whatever volume of alkali is used, and that can be measured roughly using a measuring cylinder. %%EOF Theoretically, the volume of base needed to neutralize the acid should be the same as the volume of the acid. the beaker. We added boiling stone and assembled the reflux. 3. Use the data in Table 1 to calibrate the buret. Use MathJax to format equations. By recording the weight of the sample of KHP, molarity of NaOH can be found. A titration is a controlled chemical reaction between two different solutions. Finding Ka of an Acid from incomplete titration data. equivalence point. When NaOH reacts with H2SO4, their is formation of salt takes place and water molecules are also released as a side product. The general equation for calculation of molarity of given solution: Firstly we calculate No. The above equation can be used to solve for the molarity of the acid. 0000005234 00000 n Legal. The purpose of this lab was to determine the concentration of a sodium hydroxide solution by titrating it with a standard solution of known concentration. The data from the first part of the lab can be found on table 1. Neutralization occurred in the titration process: Add 100mLs of distilled H20 and add 3 drops of the indicator. pure KHP (M). the point at which the amount of titrant added is just enough to completely neutralize the analyte solution.The point at which the indicator changes color is called the endpoint. This is an acid-Base reaction which is called a neutralization reaction and the formation of salt as a product takes place. Leave the concentrated solution to evaporate further in the crystallising dish. EXPERIMENTAL #%() + +() 2.() (1). Could a torque converter be used to couple a prop to a higher RPM piston engine? Are these the expected results? Phenolphthalein is usually used when the solution is strong base and weak acid. Following are the steps to writing the Net ionic equation: (aq) (aq) (aq) (l), 2H+ + (SO4)2- + 2Na+ + 2(OH) 2Na+ +(SO4)2-+ 2H2O. Students need training in using burettes correctly, including how to clamp them securely and fill them safely. The KHP is then titrated by delivering the NaOH solution from the calibrated buret from part 1. Thanks for contributing an answer to Chemistry Stack Exchange! Hg (O Ac) 2, HO 2. Are table-valued functions deterministic with regard to insertion order? Titration is used to determine, accurately, the volumes of solution required to reach the end-point of a chemical reaction. Question 4: What evidence exists for the presence of random and systematic errors? DATA Ring stand titration (4). The students were also able to apply the information to the theoretical value of copper in malachite to determine the percent error of the mineral mass percent. The titration reaction of KHP with NaOH is as follows: C 8 H 5 KO 4 ( aq) + NaOH ( aq) H 2 O + C 8 H 4 NaKO 4 ( aq) The NaOH solution is prepared by measuring out about 25 g of NaOH (s), which is then transferred to a 1 L volumetric flask. An example of data being processed may be a unique identifier stored in a cookie. Conclusion This study demonstrates that the titration method relying on visual detection of the end 0000005367 00000 n Standardize a sodium hydroxide (NaOH) solution using titration of potassium hydrogen phthalate (KHP) using a calibrated buret. To perform each titration approximately 2.5 g of KHP is transferred into a 100 mL beaker. H2O2, NaOH ISelect to Edit Select to Edit 1. Comment Button navigates to signup page (26 votes) Upvote. 0000006113 00000 n In this process, 2 moles (the molecular weight of a substance expressed in grams) of sodium hydroxide (NaOH) combine with one mole of sulfuric acid (H 2 SO 4 ). Throughout the course of the lab, we utilized an acid-base titration of 10mL of an unknown solution (NaOH) as to determine its molarity. 752. endstream endobj 536 0 obj<>/Size 514/Type/XRef>>stream Once the concentration of NaOH is found, it will help t, hydroxide against a very pure grade of KHP, The Methodology of the Social Sciences (Max Weber), Psychology (David G. Myers; C. Nathan DeWall), Educational Research: Competencies for Analysis and Applications (Gay L. R.; Mills Geoffrey E.; Airasian Peter W.), Give Me Liberty! hydroxide against a very pure grade of KHP and determine the percent purity of an impure 1. 0000009049 00000 n H2SO4 + 2NaOH Na2SO4 + 2H2O. 0000002603 00000 n 2 utility clamps Aspirin is the generic name for the compound called acetylsalicylic acid. rev2023.4.17.43393. An indicator can be added to show the end-point of the reaction. 3. DI water. This is a resource from thePractical Chemistry project, developed by the Nuffield Foundation and the Royal Society of Chemistry. In the round-bottom flask (100 mL), we placed p-aminobenzoic acid (1.2 g) and ethanol (12 mL). Now, how do I find the molarity of the $50~\mathrm{mL}$ sample of $\ce{H2SO4}$ from this? If your school still uses burettes with glass stopcocks, consult the CLEAPSS Laboratory Handbook, section 10.10.1, for their care and maintenance. The best answers are voted up and rise to the top, Not the answer you're looking for? This also shows Double displacement reactions, this occurs when two compounds react together by exchanging ions, resulting in the formation of two new compounds. A titration is an analytical procedure used to determine the accurate concentration of a sample by reacting it with a standard solution. Indicator: For the purposes of this tutorial, it's good enough to know that an indicator is a weak acid or base that is added to the analyte solution, and it changes color when the equivalence point is reached i.e. It can be determined when the colourless titrated solution changes to pink colour Use data to perform error analysis (identify the presence of random and/or systematic errors). Answer: When comparing the curve of a weak specie with a strong specie, the strong NaOH + h2so4 titration calculations Na 2 CO 3 (aq) + HCl (aq) NaHCO 3 (aq) + NaCl (aq) %PDF-1.4 % What does a zero with 2 slashes mean when labelling a circuit breaker panel? Sulphuric acid is a strong acid, and sodium hydroxide is a strong base. The clock will continues for 250 seconds, when it stops close the stopcock. When you add a hydrochloric acid (HCl) solution to a solution of sodium carbonate (Na 2 CO 3 ), the hydrogen ion in HCl switches places with one of the sodium ions in Na 2 CO 3 to produce sodium hydrogencarbonate, also known as sodium bicarbonate (baking soda), and sodium chloride (salt). This lab consists of finding the concentration of the reaction, but there is a sodium hydroxide Amount of NaOH used in titration (mL) Moles of KHP (mol) Concentration of NaOH in pure KHP (M) Trail 1 0 33 0 2. This is also an Acid-base reaction or we called it neutralization reaction and double displacement reaction. 5. Take II, III, IV result, From this experiment, we can analyze concentration of base when the concentration of acid is known. Questions: Draw the titration curve for a strong base added to a strong acid. Once the tip of the burette is full of solution, close the tap and add more solution up to the zero mark. Example 21.18.1. Producing a neutral solution free of indicator, should take no more than 10 minutes. After neutralize, we collected benzocaine by vacuum filtration. After we recorded the readings from the burette, we need to calculate using the given formula and the average volume of NaOH solution used from the results. The titration process involved the repetitive dropping of .5 mL of .2M HCl into the unknown solution and the recording of the solution's pH as each drop was added. Unit 2: CHEMICAL BONDING, APPLICATION OF CHEMICAL REACTIONS and ORGANIC CHEMISTRY, (j) titration as a method to prepare solutions of soluble salts and to determine relative and actual concentrations of solutions of acids/alkalis, Unit 1: THE LANGUAGE OF CHEMISTRY, STRUCTURE OF MATTER AND SIMPLE REACTIONS, 1.7 Simple equilibria and acid-base reactions, Demonstrate intermolecular forces with colourful separations, Improving our Classic chemistry demonstrations collection, Gold coins on a microscale | 1416 years, Practical potions microscale | 1114 years, Antibacterial properties of the halogens | 1418 years, Small (filter) funnel, about 4 cm diameter, Microscope or hand lens suitable for examining crystals in the crystallising dish. Carbonic acid is a weak acid which will react with a strong base to form a basic (pH > 7) solution. Titration of a standard acid, such as KHP, with the NaOH solution can be used to accurately determine the concentration of the NaOH solution. Students doing a titration experiment in a school science laboratory. 4. 50-mL buret Table 1: Buret Calibration Data (Buret volume and mass of water dispensed). The measurements for the calibration data include reading the volume level of DI water in a buret as successive volumes of DI water are delivered into a flask. Why hasn't the Attorney General investigated Justice Thomas? In conclusion, acetic acid and NaOH are two important chemicals with a variety of applications, including in the process of titration. Should the alternative hypothesis always be the research hypothesis? Burette stands and clamps are designed to prevent crushing of the burette by over-tightening, which may happen if standard jaw clamps are used. For a weak acid there's only partial ionization. Develop a consensus for the questions in the exercise, Chad Kinney, University of Colorado Pueblo (. To calculate sulfuric acid solution concentration use EBAS - stoichiometry calculator. 204.22 g mol-1 The purpose of this lab was to . BACK TITRATION. Accurately determining the amount of an analyte (unknown), in terms of concentration, is largely dependent on the quality (accuracy) to which standards are known and the quality of the tools (sensitivity and calibration accuracy) used to make the determination. First, two grams on an unknown white compound were given. This directly refutes the hypothesis. Phenolphthalein changes from clear to red at a pH value of about 9. This means that NaOH will absorb water in the atmosphere, and as a result when you measure the mass of NaOH on a balance you are likely measuring NaOH plus some amount of water. During the neutralization reaction, the base neutralized the acid, and heat is released thus the reaction is called an Exothermic reaction and a new bond formation takes place. differ from the shape of a curve with a strong specie (NaOH or HCl)? 0000004546 00000 n Read more facts on H2SO4:H2SO4 + KClO3H2SO4 + NaHH2SO4 + NaOClH2SO4 + K2SH2SO4 + MnO2H2SO4 + HCOOHH2SO4 + Mn2O7H2SO4 + MgH2SO4 + Na2CO3H2SO4 + Sr(NO3)2H2SO4 + MnSH2SO4 + NaHSO3H2SO4 + CaCO3H2SO4 + CH3COONaH2SO4 + SnH2SO4 + Al2O3H2SO4 + SO3H2SO4 + H2OH2SO4 + Fe2S3H2SO4 + Cl2HCl + H2SO4H2SO4 + FeCl2H2SO4 + Li2SO3H2SO4 + KOHH2SO4 + CH3CH2OHH2SO4 + Li2OH2SO4 + K2Cr2O7H2SO4 + NaOHH2SO4+ AgH2SO4 + Mn3O4H2SO4 + NaH2PO4H2SO4 + SrH2SO4 + ZnH2SO4-HG2(NO3)2H2SO4 + Pb(NO3)2H2SO4 + NaH2SO4 + Ag2SH2SO4 + BaCO3H2SO4 + PbCO3H2SO4 + Sr(OH)2H2SO4 +Mg3N2H2SO4 + LiOHH2SO4 + Be(OH)2H2SO4 + AlCl3H2SO4 + Na2S2O3H2SO4 + KIH2SO4 + Fe(OH)3H2SO4 + Al(OH)3H2SO4 + NaIH2SO4 + K2CO3H2SO4 + NaNO3H2SO4 + CuOH2SO4 + Fe2O3H2SO4 + AgNO3H2SO4 + AlH2SO4 + K2SO4H2SO4-HGOH2SO4 + BaH2SO4 + MnCO3H2SO4 + K2SO3H2SO4 + PbCl2H2SO4 + P4O10H2SO4 + NaHCO3H2SO4 + O3H2SO4 + Ca(OH)2H2SO4 + Li3PO4H2SO4 + Na2HPO4H2SO4 + ZnCl2H2SO4 + BeOH2SO4 + KMnO4H2SO4 + CH3NH2H2SO4 + CH3COOHH2SO4 + PbH2SO4 + CH3OHH2SO4 + Fe2(CO3)3H2SO4 + Li2CO3H2SO4 + MgOH2SO4 + Na2OH2SO4 + F2H2SO4 + Zn(NO3)2H2SO4 + CaH2SO4 + K2OH2SO4 + Mg(OH)2H2SO4 + Sb2S3H2SO4 + NH4NO3H2SO4 + AlBr3H2SO4 + CsOHH2SO4 + CuSH2SO4 + BaSO3H2SO4 + Na2SH2SO4 + AlPO4H2SO4 + As2S3H2SO4 + FeH2SO4 + HCOONaH2SO4 + CuH2SO4 + PbSH2SO4 + P2O5H2SO4 + CuCO3H2SO4 + LiH2SO4 + K2CrO4H2SO4 + NaClH2SO4 + Ag2OH2SO4 +Mg2SiH2SO4 + Mn(OH)2H2SO4+ NACLO2H2SO4 + KH2SO4 + Li2SH2SO4 + SrCO3H2SO4 + H2O2H2SO4 + NH4OHH2SO4 + KBrH2SO4 + BeH2SO4 + Fe3O4H2SO4 + Fe3O4H2SO4 + Al2(SO3)3, SN2 Examples: Detailed Insights And Facts, Stereoselective vs Stereospecific: Detailed Insights and Facts.