A sample consisting of 50. mL of 0.400 M solution of the acid, HClO4, is titrated with a 0.200 M solution of the base, LiOH. Write the balanced chemical reaction for neutralization reaction: Write th

AP Chem AB FRQQuestion 1A sample consisting of 50. mL of 0.400 M solution of the acid, HClO4, is titrated with a 0.200 M solution of the base, LiOH.Write the balanced chemical reaction for neutralization reaction: HClO4 (aq) + LiOH (aq) _ LiClO4 (aq) + H2O (l)Write the NET ionic equation for the neutralization reaction.OH_ (aq) + H_ (aq) _ H2O (l)Compute the pH of the titration solution. Show your work i) before any of the base is added ii) after 25. mL of base is added iii) after 50. mL of base is addedA student performs the titration with the same chemicals but with smaller volumes of each chemical . Which of the following titration curves could represent the titration. ExplainA because this entails a strong acid and a strong base. Question 2A student performs a titration of an unknown acid with a strong base and gets the following titration curve:a) The student consults the list of pKa of acids shown below. If the acid is listed in the table below, which is the most likely identity of the unknown acid? Explain.Acid KaHF 7.2 x 10-4CH3COOH1.8 x 10-5H2CO34.3 x 10-7HBrO2.0 x 10-9The unknown acid is HBrO because the calculated Ka is in between 50^-4 and 50^-6 and 2.0 x 10^-9 lies in between them.b) What is the initial molarity of the acid?10^-3 = 0.001MQuestion 3a) Describe the components and the composition of an effective buffer solution. Explain how the components of the buffer allow the buffer to maintain its pH.An effective buffer solution has a weak acid and its conjugate base or a weak base and its conjugate acid. A buffer solution is most effective when the ratio of its component concentrations is close to 1, also when the pH is equal to the pka of the acid.; The components of the buffer allow the buffer to maintain its pH because buffers can absorb excess H+ions or OH ions. An employer is interviewing four applicants for a job as a laboratory technician and asks each how to prepare a buffer solution with a pH of 5.0. The following constants may be helpful: hydrazoic acid, pKa = 4.74 Boric acid, pKa = 9.23Archita A. says she would mix equal molar solutions of hydrazoic (HN3) and sodium azide (NaN3) solutions.Bradley B. says she would mix equimolar Boric acid (H3BO3) and HCl solutions.Carlos C. says he would mix equimolar Boric Acid (H3BO3) and sodium dihydrogen borate (NaH2BO3) solutions.Delia D. says he would mix equimolar hydrazoic Acid (HN3) and NaOH solutions.b) Which of these applicants has given an appropriate procedure? Explain your answerDelia because she is using Sodium hydroxide which results in a pH of 5. NaOH is a strong base and in order to have an effective buffer a weak acid must be incorporated which is the HN3.c) Explain what is wrong with the erroneous procedures. The rest all incorporate a strong acid and a strong base or a weak acid and a weak base which don result in an effective buffer.d) The applicants have access to the 1 Liter volumes of each of the solutions listed above. They have access to graduated cylinders. In order to make 1.0 Liter of the correct 5.0 buffer solution, what volumes of the two chemicals must be mixed?

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