A solution is prepared by adding 0.10 mol of lithium nitrate, LiNO_3 to 1.00 L o

Question

A solution is prepared by adding 0.10 mol of lithium nitrate, LiNO_3 to 1.00 L of water. Which statement about the solution is correct? A)The solution is basic. B) The solution is C) The solution is weakly acidic. D) The solution is strongly acidic. E The values for K_a and K_b for the species in solution must be known before a prediction can be made. The pH of blood is 7.35. It is maintained in part by the buffer system composed of carbonic acid (H_2CO_3) and the bicarbonate (hydrogen carbonate, HCO_3) ion. What is the ratio of bicarbonate]/[carbonic acid] at this pH? For carbonic acid, K = 4.2 times 10^-2. A) [bicarbonate]/[carbonic acid] = 0.11 B) [bicarbonate]/[carbonic acid) = 0.38 C [bicarbonate]/[carbonic acid] = 2.65 D) [bicarbonate]/[carbonic acid] = 9.4 E) None of the above ratios is correct. A diprotic acid H_2A has K_a1 = 1 times 10^-4 and K_a2 = 1 times 10 The corresponding base A^2- is titrated with aqueous HCl, both solutions being 0.1 mol L^-1 .Which one of the following diagrams best represents the titration curve which will be seen? Increasing the concentrations of the components of a buffer solution will increase the buffer range. If the pH of a buffer solution is greater than the pk_a value of the buffer acid, the buffer will have more capacity to neutralize added base than added acid. The equivalence point in a titration is defined as the point when the indicator changes color. For a diprotic acid H_2A, the relationship K_a1 > K_a2 is always true.

Explanation / Answer

(8) Since LiNO3 is a salt formed by stron base (LiOH) and strong acid (HNO3), when it dissolved in water it forms a neutral solution because both can undergo complete ionisation. No hydrolysis takes place.

(B)

(9)

pH = pKa + Lg[salt]/[acid]

7.35 = - Log(4.2*10-7) + Log[salt]/[acid]

7.35 = 6.38 + Log[salt]/[acid]

Log[salt]/[acid] = 0.970

[salt]/[acid] = 9.33

(D)

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