In the following reaction in aqueous solution, the acid reactant is ___________ and the base reactant...
#2 & 3 Identify the following species in water, as Bronsted Acids [A] or Bronsted Bases [B]: H_3O^+; H_2SO_4; OH^-; HCN; CH_3COOH; CH_3NH_2 WRITE NET Ionic Equations for the reactions of H_2PO_4^-, an amphiprotic ion, with aqueous solutions of HCl KOH Give the conjugate base for each of the following acids: HI HSO_4^- H_2CO_3 C_2H_5NH_3^+ Give the conjugate acid for each of the following bases: NH_3 O^2- H_2O PO_4^3- Identify the conjugate acid-base pairs in each of the following reactions:...
Write an equation for the reaction of each of the following with water a) HNO_3 b) HCOOH c) NaOH d) NH_3 (2) Identify the conjugate acid-base pairs in each of the following chemical reactions: a) NH_4^+(aq) + CN^-(aq) NH_3(aq) + HCN(aq) b) CO_3^2-(aq) + HCI(aq) HCO_3^-(aq) + CI^_(aq) c) HCI(aq) + OH^-(aq) H_2O(aq) + CI^-(aq) (3) Classify each of the following as Bronsted acid, Bronsted base, or both in aqueous solution: a) NH_4^+ b) NH_3 c) H_2CO_3 d) HCO_3^- e)...
Write a balanced chemical equation (including phases) to describe the following reactions of sulfuric acid and nitric acid: Nitric acid reacts with ammonia in aqueous solution. HNO_3(aq) + NH_3(aq) implies NH^+_4(aq) + NO^-_3(aq) Sulfuric acid reacts with ammonia in aqueous solution. H_2SO_4(aq) + 2 NH_3(g) implies (NH_4)_2 SO_4(aq) Sulfuric acid dissolves in water. Step 1 (1st proton): H_2SO_4(aq) + H_2O(l) implies H_3O^+(aq) + HSO^-_4(aq) Step 2 (2nd proton): HSO^-_4(aq) + H_2O(l) implies H_3O^+(aq) + SO^2-_4(aq)
Which of the following are strong electrolytes: BaSO_4, AgNO_3, HBr, HNO_2 and HC_2H_2O_2 6. Which of the following are weak electrolytes: HNO_3, HF, HI, NH_3(aq) and KOH? 7. For each of the following water-soluble compounds indicate the ions present in an aqueous solution: Nal, K_2SO_4, NaCN, Ba(OH)_2, and (NH_4), SO_4. 8. Write a balanced chemical equation showing how you could prepare each of the following suits from an acid-base reaction: KNO_3, NaBr, and CaS.
What is K_eq for the following reaction: HPO_4^2-(aq) + H_3O^+(aq) H_2PO_4^-(aq) + H_2O(l) Some possibly useful equilibrium constants are: 0.0070, 6.2E-8, and 4.7E-13, for the K_a1, K_a2, and K_a3 of phosphoric acid.
Identify the conjugate base of formic acid (HCOOH) HCOO^- HCOO^-COOH HCOOH_2^+ Complete the balanced equation for the reaction that occurs when formic acid (HCOOH) dissolves in water. Please include the state of matter for all chemical species. HCOOH(aq) + H_2O(l)
Consider the following Bronsted-Lowry acid-base reaction: C6H5NH2 + HCOOH = C6H5NH3+ + HCOO Which of the following is a conjugate acid-base pair? O a. C6H5NH3+ and HCOO- O b. HCOOH and C6H5NH3+ a C6H5NH2 and HCO2H هنا Od. C6H5NH3 and C6H5NH2 e. HCOO and C6H5NH2
Predict the direction for each of the following acid-base reactions. Circle the right choice. a. H_3O^+ + CO_3^2- HCO_3^- + H_2O Forward/Backward b. NO_3^- + HF HNO_3 + F^- Forward/Backward c. HS^- + NH_4^+ H_2S + NH_3 Forward/Backward
Calculate the pH of a 0.0167 M aqueous solution of formic acid (HCOOH, K, = 1.8x10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH [HCOOH)equilibrium [HCOO equilibrium
Identify acid,base,conjugate acid, and conjugate base For the following equation, identify the acid, base, conjugate acid, & conjugate base. HCIO_4 + H_2O rightarrow H_3O^+ + CIO_4^-