![]() It is also the largest change in pH per change in volume as can be seen when the change in pH/change in volume vs the volume of teh titrant is added. Equivalence Point This is where the curve changes from a positive to a negative slope. The change in pH becomes very rapid here and it is important to add the titrant in smaller amounts as the observed pH starts to increase faster. ![]() titration curve Titration of a strong acid and strong base Titration of a weak acid with strong base This is reached when chemically equivalent amounts of acid and base are reacted. pH meter or colorimetric indicator This can be generated from these data pairs by plotting the pH on the y axis versus the volume of titrant on the x axis. These can be used to make the measurement of exact proton concentration or the acidity in a chemical system Titrations To monitor the extent of the reaction between acid and base, the pH is monitored with either a _ or _. Any substance that can donate a proton, H+ ionĪKA: hydrogen ion donors or proton donors Bronsted Lowry Acid Any substance that can accept a proton, H+ ionĪKA: hydrogen ion acceptor or proton donors Bronsted Lowry Base Electron pair acceptorĮx: NH3 Lewis Base The mathematical definition is the negative log of the H3O+ concentration pH Laboratory method which involves the adding of a known amount of acid to react with an unknown amount of base, or vice versa so that the unknown amount of base or acid can be quantified. It did not classify bases that did not contain OH-, did not explain why substances like Na2CO3 behaved like bases, or why hydrogen containing compounds such as NaHCO3 did as well. It did not explain the fact that many compounds containing hydrogen did not provide an acidic solution when dissolve in water. Arrhenius Acid Substnace that ionizes when dissolved in water to yield the OH- ion Arrhenius Base What were the limitations to the Arrhenius theory? It did not account for observed acid base behavior in nonaqueous solutions. Acids Bitter, slippery, changed litmus from red to blue and were reactive with acids Alkalis (Bases) This is a substnace that ionizes when dissolved in water to yield H+ ions. Determine the molarity of the methylamine solution.0519 M These are sour, corrosive, capable of changing litmus paper from blue to red, reactive with alkalis. ![]() ![]() 119 M This graph shows the titration of 35.0 mL of methylamine solution with a 0.0865 M HCl. If 19.45 mL of NaOH is required to neutralize 0.472 g of KHP, what is the concentration of the NaOH?. H3O+ = 1.0 x 10^-11 M pH= 11 Potassium hydrogen phthalate (KHP, molar mass = 204.22 g/mol) is often used as a primary standard in acid-base titration. Calculate the pH for the H3O+ concentration. ![]()
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