When the following reaction goes in the reverse direction (from products to reactants), what is the base and the conjugate base, respectively? HF(aq) + H2O(l) ⇌ F−(aq) + H3O+(aq) Group of answer choices F− and H2O HF and F− H2O and HF H3O+ and H2O F− and H3O+

Label the Bronsted-Lowry acids and bases in the following equations, and tell which substances are conjugate acid-base pairs. Check all that apply. H,PO, (aq) + N2H (aq) =HPO; (aq) +N,H (aq) H,PO, (aq) base HPO? (aq) conjugate acid O HPO? (áq) conjugate base O N;H,(aq) acid O N,H, (aq) base O H,PO, (aq) acid O N,H, (aq) conjugate acid O N,H, (aq) conjugate base Submit Request Answer 80°F

Idendify ALL of the the TRUE statements (there may be more than 1) A) NH4^(1+)  and OH^(1-) form a conjugate acid-base pair B) HCO3^(1-) can act like a base or an acid C) H2O is the conjugate base of a Hydroxide ion D) NaHSO4(aq)+Na2CO3(aq)-->Na2SO4(aq)+NaHCO3(aq) is classified as a acid-base reaction

Identify the conjugate base in the reaction below.  HClO2 (aq) + H2O (aq) ⇌ H3O+ (aq) + ClO2- (aq)

Label the conjugate acid–base pairs in each equation.

1. Determine whether the following solutions are Bronsted-Lowry acids or bases. Then, write out the chemical equation for the dissociated solution. Additionally, determine the conjugate acid/ conjugate base of each dissociated ion. Solution: Acid/base: Chemical equation: Conjugate Acid Conjugate base: а) HBr (aq) HBr (aq) + H2O (1) = b) OH (aq) ОН (аq) + Н2О (1) c) NH4* (aq) NH4* (aq) + H2O (1) =

In the following Bronsted-Lowry acid-base reactions identify the acids and the bases on each side of the equation and predict the favored direction of the reaction: 1. C2H5O- + CH3COOH ⇄ C2H5OH + CH3COO- 2. HF + H2O ⇄ F- + H3O+ 3. C-C≡C- + NH3 ⇄ C-C≡C-H + NH2-

What is the most important part of the Bronsted-Lowry theory that is not in the Arrhenius theory of acids and bases? acids create H30* in aqueous solution bases create OH in aqueous solution O acids donate H* to water, bases accept H* from water strong acids have complete dissociation, weak acids have equilibrium dissociation ions can act as weak acids or bases

answer with it either pH increase, pH decrease, no change, or cann't determine. a. What is the effect on pH that results from the addition NH4NO3 to NH3 solution? Use the equation below to answer the question: NH3 (aq) + H2O (l) ⇆ NH4+ (aq) + OH− (aq) b. Initially only 0.5 M HF solution is present: HF (aq) + H2O (l) ⇆ F− (aq) + H3O+ (aq). What happen if 0.5 mol of solid NaF is added to the initial HF solution? c. What is the effect on pH that results from the addition HCOONa to HCOOH solution? Use the equation below to answer the question: HCOOH (aq) + H2O (l) ⇆ HCOO− (aq) + H3O+ (aq)

What is the pOH of a solution of 0.376 M CH3NH2 and 0.111 M CH3NH3Cl?CH3NH2(aq)+H2O(l)⇌CH3NH3+(aq)+OH−(aq)                 Kb=4.4×10−4