chemistry

posted by .

Calculate the [OCl-] of a 7.03×10-2 M solution of the weak acid HClO (make an approximate calculation assuming that initial concentration is equal to the equilibrium concentration). Round your answer to 3 significant digits.

HClO = OCl- + H+

  • chemistry -

    .....HOCl ==> H^+ + OCl^-
    I...7.2E-2....0.....0
    C....-x.......x.....x
    E..7.2E-2 -x..x......x

    Ka = (H^+)(OCl^-)/(HClO)
    Substitute and solve for x

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. college chemistry

    Calculate the [CH3NH3+] of a 7.02×10-3 M solution of the weak base CH3NH2 (make an approximate calculation assuming that initial concentration is equal to the equilibrium concentration). Round your answer to 3 significant digits. …
  2. chemistry

    In a 1.0x10^-4 M solution of HClO(aq), identify the relative molar amounts of these species:HClO, OH-, H3O+, OCl-, H2O
  3. Chemistry

    In a 1.0× 10–4 M solution of HClO(aq), identify the relative molar amounts of these species from most to least: HClO, OCl, OH^-, H30^+, H20
  4. Chemistry

    In a 1.0× 10–4 M solution of HClO(aq), identify the relative molar amounts of these species. (most to least) H2O HClO H3O OH- OCl-
  5. Chemistry

    Estimate the equilibrium constant for the weak acid HCN, if a 4.68×10-3 M aqueous solution of HCN has a [H+] 0.00000151 M (make an exact calculation assuming that initial concentration is not equal to the equilibrium concentration). …
  6. chemistry

    Calculate the pH of a 5.75×10-2 M solution of the weak acid HCN (make an approximate calculation assuming that initial concentration is equal to the equilibrium concentration). Round your answer to 3 significant digits. HCN = CN- …
  7. chemistry

    Estimate the equilibrium constant for the weak acid HCO2H, if a 2.19×10-3 M aqueous solution of HCO2H has a pH 3.21 (make an approximate calculation assuming that initial concentration is equal to the equilibrium concentration). HCO2H …
  8. chemistry

    Calculate the equilibrium constant for the weak base C5H5N, if a solution of the base with an initial concentration of 5.74×10-3 M has a [C5H5NH+] of 0.00000283 M (make an approximate calculation assuming that initial concentration …
  9. chemistry

    A solution of HClO is mixed and found to have a pH of 4.53. Find what the initial concentration of HClO was for this solution. Ka = 3.00 × 10−8 for HClO. Answer in units of mol/L please help this is due in 1 hour
  10. Chemistry

    You have 1.0 liter of .45 M HCLO (aq). At 25 degrees Celsius, Ka= 3.5x10^8 for this acid. Calculate the pH of .45 M HCLO and the concentration of CLO- at equilibrium. Thank you very much for any amount of help you are willing to give …

More Similar Questions