Question

Consider two aqueous solutions of nitrous acid (HNO2). Solution A has a concentration of (HNO2] = 0.25 M and solution B has a concentration of (HNO2] = 1.55 M. You may want to reference (Page 743) Section 16.6 while completing this problem. Part A Which statement about the two solutions is true? O Solution B has the higher percent ionization and the higher pH. O Solution A has the higher percent ionization and the higher pH. O Solution B has the higher percent ionization and solution A has the higher pH. O Solution A has the higher percent ionization and solution B has the higher pH. Submit Request Answer

Answer 1

part- A 2 option b' is correct The ionization of Neak and decreases with increase in concentration. This is due to tess Ho is availible for each weak aaed molecule to realt at high concentration to lonize. More concentration - less ionizations less acide morph less concentration more ionsation more acidic less pt pH of benzoic and concentration - 0.314 ph cooh 2 phcootit Ka 26.5X155 c(1-2) d a 2 is very small So, neglisable Ka= [phoco- ] [t] cd² ch - car [phcoolt ] ccl 2) - 1) = ka - CM2 → 22 - Kq - 0.31 = ? 6.5tos = 2.096104 2 ²2.094104 - 2=2.09x104 = 1.44 +10e TH+] = ca 20.314 1.440152 = 4.46x103 pH = -log(H) a- log 4.46810 3 2 5x10g 4.46 = 3x0.649 2=1.49x1ö? pH = 1.947 1.22 1.44% pH = 1.95 1.4.7. 2020

pH of weak mono protic aug - 0.15 kaz 2x105 HA-HA- cat) cd ct de-ka = 2410 - 1.33410 0.15 d=11.337154 = 1.154152 H+ 2 ca [ht] = 0.15x1154102 = 10734153 pH= -109 1.77+153 371091-73 - 34 0.238 pH = 0.714 %2=1.2 [PH - 0.71) part - B 2 Weakaid (C) - 0.15 pka = 1x103 kazde - 2² – ka = 1110 = 6.66x10. - 16.66 xã3 - 0.0816 - 8:16 x 162 17d- 0.0816 X100 8.164 8:27 %. Ion = x xloof 2= 1.158102 %22 1st 10²x100 - 1.15 - 3 0:15 JA 8.46 -* x 1920 Too Tools 0.0816 = x 015 2e =0808 16 X6:15 ge=0.0122

0.15 o.15 part -D c = 0.15 Ka=0.15 = 1.5420 ar ko 1 2 = 1 L = = 1 x=1 de 1x100 = 100%, (H+] = ca = 0.1541 -0.15 [H +] = 0.15 H = -logo.15 = -109x15x10 = 10915 pH = 0.176 pH 20.18 porta 1.2 = 1000/.