chemistry

When referring to percent ionization values given in a acid/base table,

how to determine what is the hydrogen ion concentration of a 0.10 mol/L solution of hydrofluoric acid?

  1. 👍 0
  2. 👎 0
  3. 👁 39
asked by Jay
  1. The following answers the question but it doesn't involve percent ionization unless you want to calculate it from the Ka values in the table.
    HF ==> H^+ + F^-

    Use the ICE table.
    Initial concentration
    Change in conen and
    Equilibrium concn.

    Iinitial concn:
    (HF) = 0.1 M
    (H^+) = 0
    (F^-) = 0

    Change in concn:
    (H^+) = +x
    (F^-) = +x
    (HF) = -x

    Equilibrium concn:
    (HF) = 0.1-x
    (H^+) = 0 + x = x
    (F^-) = 0 + x = x

    Write the Ka expression. For HF it is
    (H^+)(F^-)/(HF) = Ka.
    Look up Ka in your tables, plug in the equilibrium concn from above, and solve for x. That is the (H^+).

    1. 👍 0
    2. 👎 0
    posted by DrBob222

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    Hi there, ok, my question stated "Use information from acid/base table and the value of Kw t ocalulate the base ionization constant, Kb, of the following bases: a)hypochlorite ion b) nitrite ion c) benzoate ion I looked at my

    asked by Jay on April 8, 2008
  2. chemistry

    For a week acid whose ionization constant is 1.75 x 10(-5), the pH of its solution is 3.0. Determine its degree of ionization and its percent ionization.

    asked by chris on October 13, 2011
  3. chemistry

    A 0.185 M solution of a monoprotic acid has a percent ionization of 1.55%. Determine the acid ionization constant (Ka) for the acid.

    asked by cindy on April 24, 2012
  4. Stupid Chemistry

    Ok, blonde moment here, Kb is the same as Ka but just for bases and Ka is for acids correct? right. Ka is the ionization constant for acids, Kb is the ionization constant for bases. BUT, we can change one into the other this way.

    asked by Taasha on August 4, 2007
  5. chem help

    a. Determine the percent ionization for a 1.00M phosphoric acid solution at 25.0 oC given the following (assume the small x approximation is valid) H3PO4(aq) H2PO4(aq)H+(aq) ΔGf (kJ/mol) -1142.6| -1130.2 | 0 b. Assuming ΔGf does

    asked by Mall on April 19, 2015
  6. Chemistry130

    Can someone please help me with this? Are these substances acids or bases? 1. Tums- Base, right? 2. Vitamin C- Acid, right? 3. Nail Polish Remover- Base or Acid? 4. Coca Cola Pop- Acid, right? 5. Cream of Tarter- Acid, right? 6.

    asked by Adam on October 13, 2009
  7. chemistry

    What is the percent ionization of a 1.38 mol/L weak acid if its Ka = 2.7 x 10-6? Answer to two (2) decimal places. I know what steps to use but have difficulty applying them to the quesiton Can someone please complete the question

    asked by Anna on April 18, 2008
  8. Chemistry

    What will happen if a small amount of hydrochloric acid is added to a 0.1 M solution of HF? A) The percent ionization of HF will increase. B) The percent ionization of HF will decrease. C) The percent ionization of HF will remain

    asked by Robby on March 7, 2013
  9. Chem

    What simplifying assumptions do we usually make in working problems involving equilibria of salts of polyprotic acids? Why are they usually valid? Answer by selecting all true statements. Are the answers: a,b,d,and f A)If the two

    asked by Lenny on February 27, 2015
  10. chemistry

    What is the percent ionization of 0.025 M chlorous acid, HClO2 solution? Ka HClO2 = 1.1*10^(-2) Answer: 48% What I did: HClO2(aq) + H2O(l) ->

    asked by % ionization on July 30, 2011

More Similar Questions