ONLY FOR MISS HASHMI

GENERAL CHEMISTRY 0

Course title: General Chemistry II

Course Code: CHM 151

Student Name:

Submission Date: th April 2017

18.Calculate the pH and the pOH of each of the following solutions at 25 °C for which the substances ionize completely:

(a) 0.200 M HCl

(b) 0.0143 M NaOH

(c) 3.0 M HNO3

(d) 0.0031 M Ca(OH)2

36.What is the ionization constant at 25 °C for the weak acid (CH3)2 NH2 +,the conjugate acid of the weak base (CH3)2NH, Kb = 7.4 × 10−4?

52.Which of the following will increase the percent of HF that is converted to the fluoride ion in water?

(a) addition of NaOH

(b) addition of HCl

(c) addition of NaF

60.Calculate the ionization constant for each of the following acids or bases from the ionization constant of its conjugate base or conjugate acid:

(a) F−

(b) NH4 +

(c) AsO4 3−

(d) (CH3)2NH2+

(e) NO2−

(f) HC2 O4 – (as a base)

14.4 Hydrolysis of Salt Solutions

78.Determine whether aqueous solutions of the following salts are acidic, basic, or neutral:

(a) Al(NO3)3

(b) RbI

(c) KHCO2

(d) CH3NH3Br

90.What is [H3O+] in a solution of 0.075 M HNO2 and 0.030 M NaNO2? HNO2(aq) + H2 O(l) ⇌ H3 O+(aq) + NO2 −(aq) Ka = 4.5 × 10−5

98.Calculate the pH of a buffer solution prepared from 0.155 mol of phosphoric acid, 0.250 mole of KH2PO4, and enough water to make 0.500 L of solution.

114. Draw a curve similar to that shown in Figure 14.23 for a series of solutions of NH3. Plot [OH−] on the vertical axis and the total concentration of NH3 (both ionized and nonionized NH3 molecules) on the horizontal axis. Let the total concentration of NH3 vary from 1 × 10−10 M to 1 × 10−2 M.

Fig 14.23 see attached