Consider the following reactions: HOAc + H*(aq) + OAc(aq) K=1.8-10-5 M NH3(aq) + H₂O(l) + NH4 (aq) + OH(aq) K = 1.8-10-5 M H₂O(l) H*(aq) + OH(aq) K=1.0-10-14 M² What is the value of K for the reaction HOAc(aq) + NH3(aq) + OAC (aq) + NH4*(aq) K=

= 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

(a) Using the expression Ka=[H+][A−]/[HA], explain how to determine which solution has the lower pH, 0.10MHF(aq) or 0.10MHC2H3O2(aq). Do not perform any numerical calculations. (b) Which solution has a higher percent ionization of the acid, a 0.10M solution of HC2H3O2(aq) or a 0.010M solution of HC2H3O2(aq) ? Justify your answer including the calculation of percent ionization for each solution.

Calculate the K of A" given HA(aq) + H2O(l) = H₂O† (aq) + A¯¯(aq) K = 5.90×108

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…

HA is a weak acid. Select the correct dropdown value to correctly complete the incomplete concentration table below being used to determine the equilibrium concentrations of HA, H3O*, and A¯ of a 0.1300 M HA solution that has a pH of 3.60 at 25°C. HA(aq) + H,0(1) = H,0^(aq) + A-(aq) Initial 0.1300 Change Equilibrium (b) (a] The value for a is [ Select ] The value for b is [ Select ] What is the Ka of this weak acid? [ Select]

What is the pOH for a solution at 25 °C that has a H3O+ concentration of 6.57 ×10-6 M?    A 34.1 % (NH4 )2SO4   (molar mass = 132.1 g mol−1) has a density of 1.15 g mL−1. What is the molarity of this solution?  (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3)     Determine the boiling point of a solution that contains 78.5 g of compound W (molar mass = 132.5 g mol–1) dissolved in 1088.6 g benzene (C6H6; molar mass = 84.156 g mol–1; Kb = 2.53 °C m–1; boiling point of pure benzene = 80.1 °C). (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3)   NEED HELP ASAP NO WORK NEEDED

5) Find the concentration of H30*(aq) in a 1.75 M solution of lactic acid, HC3H5O3, at 25°C. Ka= 1.38 x 10*. 6) Write the equilibrium expression for the ionization of HOI, and calculate the concentration of HOI(aq) in solution if [H3O*]=2.3 x 10° M and pKa = 10.7 at 25°C.

What is [OH-] in a solution of 1.25 M NH3 and 0.85 M NHANO3? NH3 (aq) + H20 (1) = NH4+ (aq) + OH- (aq) Kp=1.8x10-5 Write your answer with 2 significant digits.

At 25 oC, Ammonia is a weak base that reacts with water according to this equation: ​NH3(aq) + H2O(aq) ⇌ NH4+(aq) + OH−(aq) Briefly explain how the equilibrium will shift (to get back to equilibrium) if the following perturbations are made to the system: (a) Addition of HCl
 (b) Addition of NaOH
 (c) Addition of NH4Cl