Ans 17 :
a)
HSO4- acts as an acid when it donates its proton. The reaction is given as :
HSO4- = H+ + SO42-
b)
HSO4- acts as a base when it accepts a proton. The reaction is given as :
HSO4- + H+ = H2SO4
17. The hydrogen sulfate or bisulfate ion HSO4 can act as either an acid or a...
17. The hydrogen sulfate or bisulfate ion HSO4 can act as either an acid or a base in water solution (a) Show the reaction where HSO4 acts an acid (Ka) (b) Show the reaction where HSO4 acts a base (Kb)? 18. Show the chemical equilibrium processes for Kal and Ka2 for diprotic H2SO3 and justify which Ka is the larger value 19. A buffer contains a weak acid, HA, that is twice the concentration of its conjugate base, A. If...
24. The dihydrogen phosphate ion HSO3 can act as an acid or a base in water solution. Label each species physical state [(s), (liq), (g), (aq)]. Show all work for full credit. (a) Write the reaction where HSO3" acts as an acid (K): (2 pts) (b) Write the reaction where HSO3" acts as a base (Kb): (2 pts)
Which of the following statements is true about the bisulfate anion HSO4-? Select one: 0 a. It can behave as either an acid or a base O b. It can only behave as an acid. O c. It can only behave as a base. d. It does not react with water. o e. It is a salt. So, it is neither an acid nor a base.
Like water, the hydrogen carbonate ion (HCO31-) is amphiprotic. That is, it can act like a Bronsted-Lowry acid or as a Bronsted-Lowry base. Write equations to show both of these reactions with water
The acid dissociation constant Ka equals 1.26 x 10-2 for HSO4- and is 5.6 x 10-10 for NH4+. Which statement about the following equilibrium is correct? HSO4-(aq) + NH3(aq) = SO4 2-(aq)+ NH4+(aq) a. The reactants will be favored because ammonia is a stronger base than the sulfate anion. b. The products will be favored because the hydrogen sulfate ion is a stronger acid than the ammonium ion. c. Neither reactants nor products will be favored because all of the...
The hydrogen sulfite ion (HSO3ˉ) is amphiprotic. Write the reaction of HSO3ˉ with water, in which the ion acts as an acid. Write the reaction of HSO3ˉ with water, in which the ion acts as a base.
1) Based on your experimental rate law, is it possible that the decomposition of hydrogen peroxide over a platinum catalyst (2H2O2(aq) → 2H2O(l) + O2(g)) occurs in a single step? Briefly justify your response. 2) A student is preparing a sulfate buffer to maintain a pH of approximately 2.0. Given that the pKa of sodium bisulfate (NaHSO4) is 1.2, what ratio of sulfate (SO4 2- ) to bisulfate (HSO4 - ) would create a buffer of pH 2.0? The acid...
Label Each substance as either Hydrogen Ion Hydroxide ion arrthenius acid arrhenius base Use the drop down menus to label each substance. HKNO3 → H+ + NO3- KOH → K+ + OH-
1. A hydrogen atom in the organic base pyridine, CsHsN, can be substituted by various atoms or groups to give XCsH4N, where X is an atom such as Cl or a group such as CH3. The following table gives K, values for the conjugate acids of a variety of substituted pyridines. Atom or Group X (aq) + HCl(aq) → (aq) + Cl-(aq) NO K, of Conjugate Acid 5.9 x 10-2 1.5 x 10-4 6.8 x 10-6 1.0 x 10-6 н....
The ion HCO3- is amphoteric (can act as both a base and an acid when placed into water). Write the reaction that occurs in both instances. Include the correct charges on all ionic species. HCO3- acting as an acid HCO3- acting as a base