Chemistry

The reaction:
H2PO4- + HAsO42 ---> HPO4- + H2AsO4-

Which one of the sets above lists both of the base species involved in the equilibrium?
I'm confused and couldn't identify the conjugate acids and bases properly. Could Dr.Bob explain abt this problem ? Thank you

  1. 👍
  2. 👎
  3. 👁
  1. Acids give away H^+. Bases add them. Look for the one that give them away and accepts them.
    H2PO4^- on the left and HPO4^2- on the right must be one pair. H2PO4^-has given one H away to something.
    HAsO4^2- and H2AsO4^- must be the other pair.
    So H2PO4^- has given a H to HAsO4^2-. In the process, H2PO4^- becomes HPO4^2- and HAsO4^2- becomes H2AsO4^-. It isn't that complicated. Just follow the H. It's easy to see which is missing and which has been added.

    1. 👍
    2. 👎
  2. So,the answers are HAsO42- & HPO4- rite?
    Because from what I found,HAs04 2- is weakly basic and HPO4 2- is a conjugate base. So the bases are these two species above. M I rite?

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chem 2

    Which of the following has the highest buffer capacity? A. 0.10M H2PO4-/0.10M HPO4 2- B. 0.50M H2PO4-/0.10M HPO4 2- C. 0.10M H2PO4-/0.50M HPO4 2- D. 0.50M H2PO4-/0.50M HPOr 2- E. They all have the same buffer capacity. Double

  2. Chemistry

    A critical reaction in the production of energy to do work or drive chemical reactions in biological systems is the hydrolysis of adenosine triphosphate, ATP, to adenosine diphosphate, ADP, as described by ATP(aq) +H2O (l)

  3. Chemistry(Please check)

    1) Which of the following is not amphiprotic? H20, NH4^+^, HSO4^-^, H2PO4^-^, all choices are amphiprotic. I think that all of these are amphiprotic. I know for sure that H20 and H2PO4^-^ are. 2) The ion HPO4^-^ has both a

  4. chem

    Arsenic acid (H3AsO4) is a triprotic acid with Ka1 = 5 10-3, Ka2 = 8 10-8, and Ka3 = 6 10-10. Calculate [H+], [OH -], [H3AsO4], [H2AsO4-], [HAsO42-], and [AsO43-] in a 0.20 M arsenic acid solution. i cant do this. i don't even

  1. chemistry 12

    Identify the two conjugate acid-base pairs in each of the following. a.) H2PO4-(aq)+HSO4-(aq) H2PO4(aq)+ SO4^-2(aq) b.) HI(aq)+ CN-(aq)HCN-(aq)+ I-(aq)

  2. Chemistry

    In which direction will the net reaction proceed. X(g) + Y(g) Z(g) .. Kp = 1.00 at 300k for each of these sets of initial conditions? 1) [X] = [Y] = [Z] = 1.0 M a] net reaction goes to the left [this one?] b] net reaction goes to

  3. Chemistry

    Write a balanced equilibrium equation and kb expression for the reaction of the hydrogen phosphate ion (HPO4^2-) with water. Answer: HPO4^2-(aq) +H2O(l) PO4^3-(aq) +H3O+ (aq) kb= [PO4^3-][H3O+]/ [HPO4^2-] is that right?

  4. Chemistry- Dr.Bob222

    Which if the folowin species is not amphoteric? a) H2SO4 b) H2PO4- c) HPO4 2- d) HSO4- e) H2O

  1. Chemistry

    Identify the acid or base behavior of each substance in this reaction: H2PO4 + H2O H3O+ + HPO4-

  2. chemistry buffers

    What molar ratio of HPO4 2- to H2PO4 - in solution would produce a pH of 7.0? Phosphoric acid (H3PO4), a triprotonic acid, has pKa values: 2.14, 6.86, and 12.4. Only one of the pKa values is relevant here. how do i know which pka

  3. Chemistry

    Which is a conjugate pair in the following equilibrium? H2C2O4(aq) + HPO4(aq) 2- HC2O4(aq)- + H2PO4(aq)-

  4. Chemistry

    Given that HSO4- is a stronger acid than HPO4^2-, what is the chemical reaction if solutions containing these ions are mixed together? (Hints: One of these must act as an acid and the other as a base. Use the Brønsted-Lowry

You can view more similar questions or ask a new question.