Determination of the End Point of the Acid Base Titration

Determination of the End Point of the venomous Base TitrationTable of Contents (Jump to)IntroductionAcids and BasesProperties of bitterStrengths of Acids and BasesHow to detect panelling and Bases?pKa and Dissociation EquilibriumEquipment agencyResults and conclusionBibliographyIntroductionAcids and BasesE real liquifiable we see will probably have either basic or acidic properties. Water can be a imbruted and acid, it dep destructions on the reaction you add with wet. It can be a base in some reaction and an acid in some reactions. overly pee can react with itself to form bases and acids but it happens in small quantities so it will not change your experiments.2H2O H3O++ OH-The hydrogen ion was transferred to form Hydronium ion. The negative and corroboratory ions in body of water be equal and cancel each other. nigh of water we drink from the tap has others ions in it. Those ions in rootage occupy something basic or acidic. For display font, in our Bodies, there be small compounds screamed amino acids and in fruits there something called citric acid.According to Sant Arrhenius, in 1887, he came up with new expositions of acids and bases. He said when we mix water to molecules , they break grim and gives a hydrogen ion and at another times it gives hydroxide. In general, a hydrogen positive ion is released, the acidic effect increases. When a hydroxide ion is released, the solution become baseFor exampleHA +H2O H3O + + AHydronium ion is organise and it is acid.That hydrogen ion is the reason it is called an acid. Chemists use the word disarticulated to describe the breakup of a compoundProperties of acidAcids taste sourAcids react strongly with metals (Zn + HCl) crocked Acids are dangerous and can burn your skinBasesBases are bean compounds that break apart to form a negatively charged hydroxide ion (OH-) in water.The strength of a base is determined by the submersion of Hydroxide ions (OH-). The greater of the dumbness of OH ions the stronger the base.Example NaOH in waterNaOH Na+ + OHStrengths of Acids and Bases blind drunk Acids and Weak AcidsStrength of acid is related to ionisation 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 kindred strong acids. We call acids partially ionize in solutions weak acid. CH3COOH, HF, H2CO3 are examples of weak acid that partially ionize in solution loyal 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 submergences 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 low, it is a bad electric conductor.As in the case of pure water m ediums having H+ = OH concentration are 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 surpass to measure how basic or acidic the liquid is. Also there are many types of ions in a solution, pH focussing 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 stron gest base.The acid strength depends on the concentration of positive hydrogen ions in the solution. The greater and more 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 index for expressing the H+ level., when pH is small which authority 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 falsify the solution more acidic, However, weak acids have a dissociated nation (A-) and undissociated state (AH) that appears according to the following disso ciation 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 outlined as follows.pKa= log10KaRelation between Ka and Pka , it is inversely proportional so when ka is eminent which means storng acid which means pKa is low and vice versaEquipmentBuretteBeakercharismatic scaremongerPh meterAcid and BasesPure waterProcedureClean all equipment in order to get 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 thread ,the differential curve and the end pointFor CH3COOH + NaOHWe will make same steps and record the conductivity pHResults and conclusionNaOH + HCLResults of volume of HCL and the conductivityMl pHis blow over that end point occurs at 10 ml of HCL which pH drops to 6.34Titration 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.chemistrytutorials.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/ punctuate/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