C Choose a chemical equation showing how the following species can behave as indicated when dissolved in water: HN202 as an acid. O HN202 (aq) + H2O(1) H,N2O2(aq) + OH (aq) O HN202 (aq) + H20(1) = N2O2² (aq) + H3O*(aq) O HN202 (ag) + H2O(1) = N2O2² (ag) + H* (aq) O HN2O2 (ag) + H20(1) = H,N2O2 (aq) + H30* (aq) d Choose a chemical equation showing how the following species can behave as indicated when dissolved in water: PO3 as base. O PO3 (aq) + Hz0(1) = H2PO3(aq) + OH (aq) O POs (ag) + H20(1) = HPO3(ag) +H* (aq) O PO3 (ag) + H2O(1) HPO3 (ag) + OH (ag) O PO3 (ag) + H20(1) = H,PO3 (aq) +H* (aq)

C Choose a chemical equation showing how the following species can behave as indicated when dissolved in water: HN202 as an acid. O HN202 (aq) + H2O(1) H,N2O2(aq) + OH (aq) O HN202 (aq) + H20(1) = N2O2² (aq) + H3O(aq) O HN202 (ag) + H2O(1) = N2O2² (ag) + H (aq) O HN2O2 (ag) + H20(1) = H,N2O2 (aq) + H30* (aq) d Choose a chemical equation showing how the following species can behave as indicated when dissolved in water: PO3 as base. O PO3 (aq) + Hz0(1) = H2PO3(aq) + OH (aq) O POs (ag) + H20(1) = HPO3(ag) +H* (aq) O PO3 (ag) + H2O(1) HPO3 (ag) + OH (ag) O PO3 (ag) + H20(1) = H,PO3 (aq) +H* (aq)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Ammonium nitrate NH4NO3 is a salt used in fertilizers and in making matches. The salt is made by the reaction of ammonia, NH3 and nitric acid, HNO3. Calculate the pH of a 0.15 M solution of ammonium nitrate at 25o Ka=5.6×10-10 NH4+ (aq) +H2O(l) → NH3 (aq) +H3O+ (aq) pH=-log[H3O+]
Match the acid to the correct chemical equation showing its reaction with water. hydrochloric acid hypochlorous acid chlorous acid chloric acid perchloric acid A. HClO2(aq) + H2O(l) ⇌ ClO2−(aq) + H3O+(aq) B. HCl(aq) + H2O(l) ⇌ Cl−(aq) + H3O+(aq) C. HClO2(aq) + H2O(l) → ClO2−(aq) + H3O+(aq) D. HClO3(aq) + H2O(l) ⇌ ClO3−(aq) + H3O+(aq) E. HClO(aq) + H2O(l) → ClO−(aq) + H3O+(aq) F. HClO(aq) + H2O(l) ⇌ ClO−(aq) + H3O+(aq) G. HClO4(aq) + H2O(l) → ClO4−(aq) + H3O+(aq) H. HClO3(aq) + H2O(l) → ClO3−(aq) + H3O+(aq) I. HClO4(aq) + H2O(l) ⇌ ClO4−(aq) + H3O+(aq) J. HCl(aq) + H2O(l) → Cl−(aq) + H3O+(aq)
How many mL of 0.15 M HCl(aq) are needed to neutralize a 249.5 mL solution of 1.1 M NaOH?
Identify the acid-base reaction: Group of answer choices ClO (g) + ClO (g) → Cl2O2 (g) C2H4 (g) + HCl (g) → C2H5Cl (g) 2HCl (aq) + Na2CO3 (aq) → 2NaCl (aq) + CO2(g) + H2O (ℓ) I2 (aq) + 2S2O32- (aq) → 2I- (aq) + S4O62- (aq)
2. HPO42taq) + H2Ou) = H2PO4°(aq) + OH 3. CH3COOH(aq) + H2O) = CH3COOH2*(aq) + OH(aq)
Phthalic acid (H 2 C 8 H 4 O 4 , abbreviated H 2 Ph ) is a diproticacid. Its ionization in water at 25°C takes place in twosteps: H 2 Ph ( a q ) + H 20 (1)2H 30+ ( a q ) + HPh – ( a q) Ка1-1.26 х 10- 3Н2 Ph - (аq)+H20(1) нзо+(аq) + Ph 2 - (aq) If 0.0100 mol of phthalic acid is dissolved per liter ofwater, calculate the equilibriumconcentrations of H 2 Ph , H P h-, Ph Ка 2-3.10х 10 - 6 2 -, and H 30 +.
H2SO4(aq) + H2O(l) → H3O+ (aq) + HSO4 (aq) O H2O is the acid (proton acceptor); H2SO4 is the base (proton donor). OH2SO4 is the acid (proton acceptor); H2O is the base (proton donor). OH2SO4 is the acid (proton donor); H2O is the base (proton acceptor). O H2O is the acid (proton donor); H2SO4 is the base (proton acceptor).
What is the pH of 0.1510 M selenious acid solution, H2SeO3? H2SeO3(aq) + H2O(l) → HSeO3−(aq) + H3O+(aq) Ka1 = 3.5000e-2 HSeO3−(aq) + H2O(l) → SeO32−(aq) + H3O+(aq) Ka2 = 5.0000e-8