This is all the information given ar 19, 2023 at 10:09 PMBuffers IObjectivesThe goal of this lab experiment is to investigate the inherent properties of a buffer system.From this lab you will:Prepare a buffer and measure pH before and after changes to the systemFind the limits of a buffer system. Compare a buffer system to a non-buffer systemDesign a buffer system given a particular pH using two different methodsTheoryA buffer simply consists of a weak acid and its conjugate base, or a weak base and itsconjugate acid. For example, an important buffer in our bloodstream consists of H₂CO3 andHCO3 as shown in Eq 1.(1)H₂CO3(aq) + H₂O(1) H3O* (aq) + HCO3(aq)The main function of this buffer is to resist pH changes. This buffer acts of hold the pH ofblood in the narrow range of 7.36 to 7.42 to allow proteins in our blood to functionproperly. To be more specific, the buffer will neutralize added base (Eq 2) by reacting withthe weak acid in the system and producing more conjugate base.H₂CO3(aq) + OH(aq) → H₂O(1) + HCO3(aq)In contrast, the addition of acid (Eq 3) to the buffer system will react with the conjugatebase and form more weak acid.(2)HCO3(aq) + H3O+ (aq) → H₂CO3(aq) + H₂O (1)One toxic compound that has been known to destroy this blood buffering system isethylene glycol, the main component of antifreeze. When metabolized ethylene glycol isconverted to glycolic acid, and then it rapidly enters the bloodstream. At first, thebicarbonate ion, HCO3, neutralizes the added acid; however, the conjugate base is rapidlyconsumed, and the pH of the blood begins to drop to dangerously low levels. In any buffersystem, the addition of large amounts of acid or base will eventually destroy theneutralizing power of the buffer. This is called exceeding the buffer capacity. Buffercapacity will be further investigated in next week's lab.(3)When studying different living organisms, it is often important to work within the livingsystems' pH range. The pH of a buffer is established by the relative concentrations of weakacid and conjugate base in the solution. The acid dissociation constant, Ka, is a great tool toestablish the relationship between these concentrations using Eq 1. The Ka of the carbonicacid-bicarbonate system is shown below (Eq 4).1 rs I prelab handout F22023 at 10:09 PMa.Buffers 1 prelab1. Keeping in mind the definition of a buffer, predict the resulting pH in the following scenarios:Start with 50 mL of buffer at pH 9.00. Add 5 drops of 0.10 M KOH.b. Start with 50 mL of buffer at pH 9.00. Add 5 drops of 0.10 M HCI.e.Name:f.Hailey GaryC. Start with 50 mL of buffer at pH 9.00. Add 10 mL of 0.10 M KOH.d. Start with 50 mL of buffer at pH 9.00. Add 10 mL of 0.10 M HCI.Start with 50 mL of pure water at pH 7.00. Add 5 drops of 0.10 KOH.Start with 50 mL of pure water at pH 7.00. Add 5 drops of 0.10 HCI.pH =pH =pH =pH =pH =pH =

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Buffer- It is defines as the buffer solution is a solution able to maintain its Hydrogen…