The concentration of each of the aqueous solutions of NaCl, `NH_(4)Cl, NaCn and HCl` is 0.1(M). Arrange these solutions in the increasing order of their pH.

The increasing order of pH of 0.1M solution of NaCl, NH_4Cl , NaCN and HCI is

Sodium salts of three monobasic acids, HA, HB and HC are HaA, NaB and NaC, respectively. The concentration of each of the aqueous solution of the aqueous solution of these salts is 0.1(M) and the pH of their solutions are 7,9 and 10, respectively. Among HA, HB and HC, which is (are) strong acid(s)?

pK_(a) values of three weak acids HA, HB and HC are 4.74, 3.35 and 5.24 respectively. The concentration of aqueous solutions of each of the three acids is 0.01 (M). Arrange them in order of increasing pH values.

The concentration of an aqueous solution of the weak acid, HA is 0.1(M). Calculate the pH and concentrations of A^- ion and HA at equilibrium in the solution. Given: K_b(HA)=1.35xx10^(-3)

The concentration of an aqueous solution of a weak monobasic acid is 1(M) and its degree of ionisation is 1.32%. Determine the pH of the solution.

The concentration of an aqueous solution of ammonia is 0.01(M). What is the pH of the solution? If 0.001 mol of NH_4Cl is added to 100 mL of that solution, state whether the pH of the solution will increase or decrease. Mention the change in the value of pH. [pK_b(NH_3)=4.74]

A,B and C are three buffer solutions, each of which composed of a weak acid and its salt. For increasing the pH by 0.02 units, it is found that 1.0, 1.4 and 1.2 millimol of NaOH are required for A,B and C, respectively. Arrange the solutions in the increasinng order of their buffer capacity.

An aqueous solution of (NH_(4))_(2)SO_(4) is acidic. Explain.

The molar concentration of an aqueous CH_3COONa solution is 0.01(M). Calculate pH of the solution. [Kea=1.8xx10^(-5)]