a]
H2SO4 ----> H+ + HSO4-
HSO4- ----> H+ + SO4-2
b]
H3AsO4 ---> H+ + H2AsO4-
H2AsO4- ---> H+ + HAsO4-2
HAsO4-2 ----> H+ + AsO4-3
c]
C6H4[COOH]2 ----> C6H4 [COOH] COO- + H+
C6H4 [COOH] COO- -----> C6H4 [COO-]2 + H+
Write the stepwise proton transfer equilibria for the deprotonation of: sulfuric acid, H_2SO_4 arsenic acid, H_3AsO_4...
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)
9. Sulfuric acid (H2S04), a diprotic acid, is a strong acid in its first deprotonation (deprotonation- loss of H'). The first deprotonation is considered complete (complete ionization). It is, however considered a weak acid for its second deprotonation with a Ka value of 1.2 X 102, For a 0.0456 M H2S04(aq) solution determine: (16 pts total) a. The chemical reaction equations for the successive loss of protons. (4 pts b. The concentration of HSO4-1 and H (H30') after the first...
A 12.0 mL sulfuric acid solution, H_2SO_4(aq), was titrated using 0.250 M KOH. If the complete neutralization of the acid required 18.6 mL of the KOH solution, what was the molarity of sulfuric acid? Answer. 0.775 M
Upload answers in PDF, WORD or JPG format: (a) Supply the arrows for deprotonation (proton transfer) (b) draw and label the resultant conjugate acid and conjugate base. Show formal charges to receive full credit 0 H OH .. base acid Hс сну, 0 н— CH3 + base acid H3C N.CH CH3 H-ö—H base acid Attach File Browse My Computer Browse Content Collection > A Moving to another question will save this response.
Aqueous sulfuric acid (H_2SO_4) reacts with solid sodium hydroxide (NaOH) to produce aqueous sodium sulfate (Na_2SO_4) and liquid water (H_2O). What is the theoretical yield of water formed from the reaction of 7.8 g of sulfuric acid and 3.7 g of sodium hydroxide? Be sure your answer has the correct number of significant digits in it.
The most produced chemical in the world (by weight and volume!) is sulfuric acid, H_2SO_4 Commercial production of H_2SO_4 proceeds following the reaction mechanism below. Use this information to answer the next two (2) questions. step 1 S_(s) + O_2 (g) rightarrow SO_2(g) step 2 SO_2(g) + NO(g) rightarrow SO_3(g) + NO(g) step 3 NO(g) + 1/2 O_2(g) rightarrow NO_2(g) step 4 H_2O_(l) + SO_3(g) rightarrow H_2SO_4(aq) Which of the following correctly categorizes the components in this mechanism? a) catalyst...
8. Being a triprotic acid, the acidity of arsenic acid is described by three equilibria. K HAO, + HO = H AsO; +H0 H, ASO, + H,0 = HASO +H,09 HASO + HO = AsO+H,0 -6.510* K2 =1.1x107 K -3.2x10-2 Determine whether solutions containing the following salts will be acidic, basic or neutral Show all calculations. (6 pts) KASO4 K HASO4 KHAsO4
HF can act as a base in sulfuric acid and an acid in liquid ammonia. Write the balanced equations, with correct physical states, that represent these equilibria. Choose one of the two process and describe how it illustrates the solvent-system concept of acid-base chemistry.
Please solve step by step Automobile batteries contain aqueous sulfuric acid, H_2SO_4. A 3.75 M solution of aqueous sulfuric acid has a density of 1.230 g/mL. What is the mass percent H_2SO_04 in this solution? What is the molality of this solution?. When 0.500 g of an unknown nonelectrolyte is dissolved in 25.00 g of camphor, the freezing point of the solution is 8.68 degree C lower than the freezing point of pure camphor. Determine the molar mass of the...
Write the equation for the proton transfer reaction involving a Brønsted-Lowry acid or base, and show how it can be interpreted as an electron-pair transfer reaction, clearly identifying the donor and acceptor.