nC SUIUIOn CHEMISTRY OVERVIEW the previous experiment you study the titration cu
ID: 950184 • Letter: N
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nC SUIUIOn CHEMISTRY OVERVIEW the previous experiment you study the titration curve of a weak monoprotic acid and you In observed that at ½ the equivalent point pH = pKa. In this experiment a buffer solution of the weak acid will be prepared using the data of the previous experiment. BUFFER SOLUTIONS are solutions that resist a change in pH when small amounts of acid or base are added. Buffers resist changes in pH because they contain both acidic species to neutralize OHf ions basic species to neutralize H. These acid and basic species must not consume ea other through the neutralization process. Some common but important buffers are HPO,2/H2PO, and CO, HCO These buffers are involved IN biological functions of the body. The phosphate buffer is the principal buffer nside cells, it consists of the pair of ions, HPO and H2PO the monohydrogen and the dihydrogen phosphate ions. Notice that the buffer's two component ions differ by only one proton; this is always true of buffer pairs. Of the two, H2PO4 has more protons and so is the better proton - donating member of the pair and the compound that nieutralizes hydroxide ons. Thus, if the cell receives more OH than normal because of some change in metabolism, the following reaction neutralizes OH and prevents the pH increasing. ly, this is the forward reaction of an equilibrium in which the pair is the product. Buffer duties in blood are consists of dissolved carbon dioxide, CO2 (aq), and bicarbonate ion, HCo second member of the handled largely by the carbonate buffer ion, HCO. Although Actual buffer pair which carbon dioxide oxide has no proton to donate, it is still a neutralizer of: rs with hydroxide ion to form the bicarbonate, ion, the other member of the buffer pair. Thus, buffers are usually prepared by mixing a weak acid or weak cause it reacts with hydroxide ion to form the with a salt of that acid or base. 63Explanation / Answer
Buffer solutions are solutions that are meant for resisting the change in pH when a small amount of acid or base is added to the solution, Important buffers include phosphate buffer and carbonate buffer. Phosphate buffer is the principal buffer inside the cells while Carbonate buffer handles the function related to blood.
Buffers are prepared by mixing a weak acid or weak base with a salt of that acid or base. For a weak monobasic acids the Ka= [H3O+] [A-]/ [HA]
[H3O+] =Ka[HA]/ [A-]
From Henderson Hasselbach equation can be represented as pH = PKa+log[A-]/[HA]. Pka can be measured by knowing the pH at [A-] =[HA] where pH=pKa
The equilibrium constant for the related to temperature By Van’T Hoff equation as lnK=-(delH/R)*(1/T)
T is temperature in K. The plot of lnK VS 1/T gives a straight line whose slope is -deH/ R where R is gas constant.
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