Is a solution of KCIO_2 acidic, basic, or neutral? Explain by selecting the sing

Question

Is a solution of KCIO_2 acidic, basic, or neutral? Explain by selecting the single best answer. Neutral, because KCIO_2 is a salt formed when chlorous acid is neutralized by KOH. Basic, because the chloride ion hydrolyzes in water. Neutral, because the KCIO_2 does not dissolve in water. Acidic, because the chloride ion will cause water to form H_3O^+? acidic, because the chloride ion will cause the pH to decrease. pKa of HN_3 is 4.60 and that of HOCN is 3.7 which is the stronger base? N_3^- OCN they are the same strength which one of the following is a buffer solution? 0.10 M NaCI 0.40 HNO_3 0.04 M KF and 0.10 M HF 0.40 M CH_3COONa 0.40 M HBr and 0.10 M NaBr A 0.400 M solution of an acid, HA, has a pH = 2.101, what is the value of the ionization constant Ka for this acid? 1.67 times 10^-2 2.0001 times 10^-1 1.57 times 10^-4 7.14 times 10^-3 6.37 times 10^-11 in which of the following would PbI-2 be the least soluble? 0.2 M MgI_2 0.2 MKI 0.2 MPb(NO_3)_2 0.2 M NaCI H_2O write the chemical equation for the reaction that takes place when a small amount is added to a buffer made with NAC_3H_7O_2(aq) and HC_3H_7O_2(aq). HCN acid has Ka 6.2 times 10^-10; calculate the pKb of CN^- at 25 degree C

Explanation / Answer

9. KClO2 solution is,

B. basic, as chlorite ion hydrolyzes in water

10. Stronger base would have lowest pKa, thus,

B. OCN-

11. Buffer is weak acid-conjugate base or weak base-conjugate acid, thus,

C. 0.4 M KF and 0.1 M HF

12. Ka = [H+][A-]/[HA]

pH = -log[H+] = 2.101

[H+] = [A-] = 7.92 x 10^-3 M

Ka = (7.92 x 10^-3)^2/0.4 = 1.57 x 10^-4

Answer : C. 1.57 x 10^-4

13. PbI2 east soluble in solution which has highest I- concentration,

A) 0.2 M MgI2

14. Addition of acid to buffer

C3H7O2- + H+ <==> GC3H7O2

Addition of base to buffer

HC3H7O2 + OH- <==> C3H7O2- + H2O

15. HCN Ka = 6.2 x 10^-10

Kb = 1 x 10^-14/6.2 x 10^-10 = 1.613 x 10^-5

pKb = -log[Kb] = 4.79

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