Chemistry

posted by .

Why is the reaction rate of a given metal with a stronger acid is faster than with weaker acid?
Which one required more volume to produce neutral solution, a strong acid or strong base,or are they just the same? Can you explain it to me please coz I can't figure it out.

Thanks in advance!

  • Chemistry -

    I don't agree with the supposition that a given metal will react faster with a strong acid than a weak one. I think the supposition is based on the fact that weak acids are not completely ionized; therefore, there are more hydrogen ions in a strong acid (one that ionizes completely). And the sentence, as you have expressed it, may intend to talk about acid strengths (that is one is more concentrated or dilute than the other). If that is the intent, then a metal reacts faster with more concentrated acids generally because they contain more hydrogen ions. But no general rule can be observed for that. For example, concentrated H2SO4 is hardly ionized at all since there is little water to form the hydronium ion. For the second part of your question, the answer is not obvious either because you don't specify how much of one versus the other or the concentrations. Volume for volume, and comparing the same kind of acid (monoprotic or diprotic or triprotic) as well as the same strength, then a neutral solution is present when the volume of one solution equals the volume of the other solution.

  • Chemistry -

    The net reaction is between hydronium, H3O+, ions and the metal, producing metal anions and hydrogen gas. A strong acid solution has a higher concentration of hydronium ions that a week acid. The rate is higher when the concentration of any one of the reactants is higher.

  • Chemistry -

    For part 1, then why is the reaction rate of a given metal with HCl is faster than with acetic acid?

    For part 2. how about 1.0M HCl and 0.5MNaOH? Which one needs more volume to produce a neutral solution?

  • Chemistry -

    1. HCl is highly dissociated since it is a strong acid. It produces a high concentration of hydrogen ions, H+(aq) in a water solution which are the same as hydronium ions, H3O+. Acetic acid, HC2H3O2, is made of molecules that do not dissociate. Its concentration of hydrogen (hydronium) ions is low. That is why acetic acid reacts more slowly than HCl with metals.

  • Chemistry -

    Why does more hydrogen ion results a faster reaction rate?
    Thanks

  • Chemistry -

    I got it. Thanks for both of you :)

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. CHEMISTRY

    HOW CAN U TELL IF HNO3 +KNO3 IS A BUFFER SOLUTION A buffer solution must contain a weak acid and its conjugate base OR a weak base and its conjugate acid. HNO3 is a strong base and KNO3 is the salt of a strong base (KOH) and a strong …
  2. Chemistry

    If an equal number of moles of the weak acid HOCN and the strong base KOH are added to water, the resulting solution will be acidic, basic or neutral?
  3. Chemistry

    which of the following statements are true?
  4. chemistry

    If the acid base reaction HA(aq)+B^-(aq)---> HB(aq)+A^-(aq) <--- has a k = 10^-4,which of the following statements are true & why?
  5. Chemistry

    Strong base is dissolved in 675 ml of 0.200 m weak acid (ka=3.25x10^-5) to make a buffer with a ph of 3.95. Assume that the volume remains constant when the base is added. HA + OH ---> H2O + A^- calculate the pka value of the acid …
  6. Chemistry(Please just check, thank you)

    1) The approximate pH of a 3.0 X 10^-3 M solution of the strong acid H2SO4 is?
  7. Chemistry

    You have two buffer solutions 1) weak acid and its conjugate base 2)weak base and its conjugate acid. Write explicitly ( considering generic formula for acid and base) the equations of neutralization when you: a) add strong acid and …
  8. chemistry

    A 1.0 M acetic acid solution (CH3COOH, pKa = 4.7) is neutralized by dissolving NaOH(s) (a strong base) in the solution. Estimate the pH at the equivalence point of the neutralization process: 4.7 7.0 9.3 Which one of the following …
  9. AP Chemistry

    A solution is prepared by titrating a 100.0 mL sample of 0.10 M HF (Ka = 7.2 × 10-4) with 0.10 M NaOH a. Does the solution contain a strong acid with a strong base, a strong acid with a weak base, a weak acid with a strong base, or …
  10. AP Chemistry

    A solution is prepared by titrating a 100.0 mL sample of 0.10 M HF (Ka = 7.2 × 10-4) with 0.10 M NaOH a. Does the solution contain a strong acid with a strong base, a strong acid with a weak base, a weak acid with a strong base, or …

More Similar Questions