posted by .

Calculate the [H3O+] of each of the following H2SO4 solutions.
For a 0.50 M soln
How do I reach the answer? Do I have to use a ice table?

  • Chemistry -

    Not for the first H^+ since it is 100% ionized. The second H^+ is not 100% ionized (k2 is about 10^-2) and you need an ICE table for that. But it's a little more complicated than that.

  • Chemistry -

    As dilute as that is, assume all dissociation has taken place (you get two protons for each H2SO4 molecule)

    So the concentration of the H ions is 2*.5=1M
    and the answer.

    Now for more concentrated solutinos, you would have to use Keq and an ice table. I would do that for anything over 8M solutions.

    Remember: STrong acids (HCl, HNO3, H2SO4) "completely" dissociate in water solutions. IT is not exactly so, but it is very close.

  • Chemistry -

    how do i reach the answer then? what are my k values if i need to use a ice table

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    Please judge my answer, thank you Question: What is the pH of a 1.24 mol/L solution of HCN(aq) if its Ka = 6.2 x 10-10?
  2. Chemistry

    The question says write a reaction for the ionization of the following compound in water. Identify the acid, the base, the conjugate acid, and the conjugate base in each of them. 1. H2SO4 2. KOH 3. CH3COOH 4. NH3 5. HNO3 My guesses …
  3. Chemistry

    I have another similar problem. I have calculated everything given (Correctly), but I can't seem to get the right pH for the stoichiometric point (I keep getting 7.16) Question: Suppose that 50.0 mL of 0.25 M CH3NH2(aq) is titrated …
  4. chemistry

    calculate [h3o] in solutions. 0.040 of HCl and 0.080 HOCl. 2. calculate OH for the solutions of 0.0063 ba (OH)2 and 0.0110 of BaCl2
  5. Chemistry 102

    For a question like “calculate the pH of an aq.solution that is 1.0 M CH3COOH and 1.0 M CH3COONa, how do you know to write the equation like this: CH3COOH + H2O => H3O+ + CH3COO- and not like H3O+ + CH3COO- => CH3COOH + H2O …
  6. Help Chemistry

    Can you please tell me if these are right?
  7. chem

    Calculate the pH of each of the following solutions. (a) [H3O+] = 2.9 10-10 M- I got 9.5 but its wrong. I used the equation pH= -log[H3O+] Is this the wrong equation?
  8. Chemistry

    Calculate the OH - concentration present in water under the following conditions. Enter your answer in scientific notation. A)[H3O+] = 9.4 x 10-10 M B)[H3O+] = 5.5 x 10-3 M C)[H3O+] = 6.2 x 10-12 M
  9. chemistry

    You have .1 moles of H3PO4 in a soln with a total volume of 250 mL. You then add .15 moles of NaOH and dilute the soln to a total volume of 1L calculate the pH of the resulting soln and the concentrations of all aqueous species. Thanks!!!!
  10. Chemistry

    Solve an equilibrium problem (using an ICE table) to calculate the of each of the following solutions. .16M CH3NH3Cl

More Similar Questions