Determination of the End Point of the Acid Base Titration

Determination of the End Point of the Acid Base TitrationTable of Contents (Jump to)IntroductionAcids and BasesProperties of sultryStrengths of Acids and BasesHow to detect dose and Bases?pKa and Dissociation EquilibriumEquipmentProcedureResults and conclusionBibliographyIntroductionAcids and BasesEvery liquid we see willing probably have either prefatorial or acidic properties. Water can be a base and acid, it dep displaces on the reaction you add with water. It can be a base in some reaction and an acid in some reactions. Also water can react with itself to form bases and acids but it happens in small quantities so it will not change your experiments.2 piss H3O++ OH-The hydrogen ion was transferred to form Hydronium ion. The negative and positive ions in water argon equal and cancel each some other. Most of water we beverage from the tap has others ions in it. Those ions in stem make something basic or acidic. For example, in our Bodies, there are small compounds called am ino acids and in fruits there something called citric acid.According to Sant Arrhenius, in 1887, he came up with new definitions of acids and bases. He said when we mix water to molecules , they break down and gives a hydrogen ion and at other times it gives hydrated oxide. In general, a hydrogen positive ion is released, the acidic solution increases. When a hydroxide ion is released, the solution become baseFor exampleHA +H2O H3O + + AHydronium ion is formed and it is acid.That hydrogen ion is the reason it is called an acid. Chemists use the word dissociated to describe the breakup of a compoundProperties of acidAcids taste sourAcids react potently with metals (Zn + HCl) laborious Acids are dangerous and can burn your skinBasesBases are ionic compounds that break apart to form a negatively charged hydroxide ion (OH-) in water.The medium of a base is determined by the absorption of Hydroxide ions (OH-). The greater of the concentration of OH ions the stronger the base.Example NaOH in waterNaOH Na+ + OHStrengths of Acids and BasesStrong Acids and Weak AcidsStrength of acid is related to ionization of acids in water. Some of the acids can ionize 100 % in water solutions we call them strong acids. HCL are examples of strong acids.in other hand, some of the acids cannot ionize like strong acids. We call acids part ionize in solutions weak acid. CH3COOH, HF, H2CO3 are examples of weak acid that partially ionize in solutionStrong and Weak BasesBases ionize completely in solutions are called strong bases. NaOH and bases including OH- ion are strong bases. Bases that ionize partially in solutions are called weak bases. For example NH3Ionization of WaterWater ionizes givesH2O(l) H+(aq) + OH(aq)In pure water concentrations of H+ and OH ions are equal to each other and at 25, they have concentration 110-7 M. then concentration of ion in pure water is too outset, it is a bad electric conductor.As in the case of pure water mediums having H+ = OH concentration a re called neutral mediums. In water solutions multiplication of H+ and OH is constant and at 25 0C it is 110-14. This number is also called ionization constant of pure water.If concentration of H+ ions equal OH-= 10 -7M, then solution is neutral.If concentration of H+ ions OH- or H+ 10 -7M and OH- -7 M, then solution is acidic.If concentration of OH- ions H+ or H+ -7 M and OH- 10-7 M, then solution is basic.How to detect acid and Bases?Scientists use something called pH scale to measure how basic or acidic the liquid is. Also there are many types of ions in a solution, pH focus on concentration of hydrogen ions and hydroxide ions. The scale measures values from 0 to 14. Distilled water is 7 in the middle. The strength of an acid or base in a solution is measured on a scale called a pH scale.Any pH number greater than 7 is considered a base and any pH number less than 7 is considered an acid. 0 is the strongest acid and 14 is the strongest base.The acid strength dep contains on t he concentration of positive hydrogen ions in the solution. The greater and to a greater extent hydrogen ions is the stronger acids likes Hydrochloric acid HCL and Sulphuric acid.pH=-logH+ and pOH=-logOH-If 7pH0 acidic solutionIf 14pH7 basic solutionIf pH=7 neutral solutionpKa and Dissociation Equilibrium1. pHWhen acids is added to water, the pH scale decreases. The acidity of a solution is examined by the hydrogen ion concentration (H+), where pH provides a simple exponent for expressing the H+ level., when pH is small which means that the smaller the number of pH , the stronger acid.pH=-log10HpKa and Dissociation EquilibriumStrong acid , which they are dissociate in solution, and weak acids that partially dissociate in solution. When dissociation of strong acid happens, it gives a proton In which make the solution more acidic, However, weak acids have a dissociated state (A-) and undissociated state (AH) that appears according to the following dissociation equilibrium equation.AH A + H+. The definition of Ka isKa=The brackets of the product to the brackets of the reactantspKa was introduced as an index to express the acidity of weak acids, where pKa is defined as follows.pKa= log10KaRelation between Ka and Pka , it is inversely proportional so when ka is high which means storng acid which means pKa is low and vice versaEquipmentBuretteBeakerMagnetic stirrerPh meterAcid and BasesPure waterProcedureClean all equipment in order to buy off accurate conductivityAdd some of NaOH into the receiving cup and then add slightly 1 ml of HCL and make sure you adding the receiving cup on the magnetic stirrerRepeat this steps to get the conductivity from volume 0 ml to 17 mlGet titration curve ,the differential curve and the exterminate pointFor CH3COOH + NaOHWe will make same steps and record the conductivity pHResults and conclusionNaOH + HCLResults of volume of HCL and the conductivityMl pHis clear that end point occurs at 10 ml of HCL which pH drops to 6.34Titratio n curveDifferential curveCh3COOH +NaohIt is clear that end point at 10 ml of Naoh the end point occur , the ph difference is very bigTitration curveDifferential curveBibliographyhttp//www. alchemytutorials.org/content/acids-and-bases/ph-poh-and-ionization-of-water/58-acids-and-bases-cheat-sheethttp//www.sciencebuddies.org/science-fair-projects/project_ideas/Chem_AcidsBasespHScale.shtmlhttp//www.elmhurst.edu/chm/vchembook/184ph.htmlhttp//lrs.ed.uiuc.edu/students/erlinger/water/background/ph.htmlhttp//www.humboldtmfg.com/graduated_glass_beaker.htmlhttp//www.shimadzu.com/an/hplc/support/lib/lctalk/29/29intro.htmlhttps//www.boundless.com/chemistry/acids-and-bases/strength-of-acids/the-acid-dissociation-constant/http//www.princeton.edu/achaney/tmve/wiki100k/docs/Acid_dissociation_constant.html