The balanced molecular equation for complete neutralization of H2SO4 by KOH in aqueous solution is: Group of answer choices 2H+ (aq) + 2OH- (aq) → 2H2O (l) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (aq) H2SO4 (aq) + 2OH- (aq) → 2H2O (l) + SO42- (aq) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (s) 2H+ (aq) + 2KOH (aq) → 2H2O (l) + 2K+ (aq)

= O ACIDS AND BASES Identifying Bronsted-Lowry acids and bases For each chemical reaction in the table below, decide whether the highlighted reactant is a Brønsted-Lowry acid, a Brønsted-Lowry base, or neither. reaction NH(aq) + OH (aq) → NH3(aq) + H₂O(1) NH3(aq) + H₂O(1)→ NH(aq) + OH(aq) NH4(aq) + OH (aq) ► NH3(aq) + H₂O(1) NH3(aq) + H₂O(1)→ NH(aq) + OH(aq) 1 highlighted reactant Bronsted-Lowry Bronsted-Lowry acid base O O O O O neither O O 0 0/5 O

In the following net ionic equation, identify each reactant as either a Bronsted-Lowry acid or a Bronsted-Lowry base. C6H1503N(aq) + H₂O(1) B-L B-L +C6H1503NH+ (aq) + OH*(aq) The formula of the reactant that acts as a proton donor is The formula of the reactant that acts as a proton acceptor is

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+]

Complete and balance the following double-displacement chemical equation: NaOH(aq) + HCl(aq)

Identify the reactant that is a Brønsted-Lowry acid and the reactant that is a Brønsted-Lowry base in each of the following: Part C 2- CO3² (aq) + H₂O = HCO3(aq) + OH-(aq) H₂O is the acid (proton donor); CO3² is the base (proton acceptor). H₂O is the acid (proton acceptor); CO² is the base (proton donor). O CO3²- is the acid (proton acceptor); H₂O is the base (proton donor). O CO² is the acid (proton donor); H₂O is the base (proton acceptor). Submit Part B Request Answer H₂SO4 (aq) + H₂O(1)→ H3O+ (aq) + HSO4 (aq) O H₂O is the acid (proton donor); H₂SO4 is the base (proton acceptor). O H₂SO4 is the acid (proton acceptor); H₂O is the base (proton donor). O H₂SO4 is the acid (proton donor); H₂O is the base (proton acceptor). O H₂O is the acid (proton acceptor); H₂SO4 is the base (proton donor). CH3-COO (aq) + H3O+ (aq) = H₂O(1) + CH3-COOH(aq) CH3-COO is the acid (proton acceptor); H3O+ is the base (proton donor). O H3O+ is the acid (proton donor); CH3-COO is the base (proton acceptor). O…

Consider the following chemical equilibrium: HCOOH(aq) + H_2O(aq) \rightleftharpoons HCOO^-(aq) + H_3O^+(aq). Which of the following graphs represents the perturbation on the system and the change of pH when water is evaporated from the container?

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)

HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kb for A−? Group of answer choices HA(aq) + H2O(l) ⇌  H2A+(aq) + OH− A−(aq) + H3O+(aq) ⇌ HA (aq) + H2O(l) HA(aq) + OH−(aq) ⇌ H2O(l) + H+(aq) A−(aq) + H2O(l)   ⇌  HA(aq) + OH−(aq) A−(aq) + OH−(aq)  ⇌ HOA2−

Calculate the concentration of each species present in a 0.010-M solution of phthalic acid, C6H4(CO2H)2. C6 H4(CO2H)2(aq) + H2 O(l) ⇌ H3 O+(aq) + C6 H4(CO2H)(CO2)−(aq)                                                                                                                                Ka = 1.1 × 10−3C6 H4(CO2H)(CO2)(aq) +H2 O(l) ⇌H3 O+(aq) +C6 H4(CO2)22−(aq)       Ka = 3.9 × 10−6