chemistry

Determine the equilibrium constant, Ka of 0.12 mole HNO2 is dissolved to make 1 L which has a hydronium ion (Hydrogen ion) concentration of 0.00115 mole/liter?

I have it as Ka= [H+] [NO2-] / [HNO2]

  1. 👍
  2. 👎
  3. 👁
  1. ..........HNO2 ==> H^+ + NO2^-
    I..........0.12..........0...........0
    C..........-x.............x...........x
    E.........0.12-x.......x...........x

    You have the correct Ka expression. Substitute the E line into the Ka expession you've written like this.
    Ka = (H^+)(NO2^-)/(HNO2)
    Ka = (x)(x)/(0.12-x)
    The problem tells you x = 0.00115, Plug than in for x and solve for Ka.
    Post your work if you get stuck.

    1. 👍
    2. 👎
    👤
    DrBob222

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry chemical equilibrium

    1.25 mol of NOCl was placed in a 2.50 L reaction chamber at 427 celciciu degre . After equilibrium was reached, 1.1 mole of NOCl remained. Calculate the equilibrium constant Kc for the reaction

  2. chemistry

    Concerning the following reaction at equilibrium: 3Fe(s) + 4H2O(g) Fe3O4(s) + 4H2(g), increasing the concentration of the Fe(s) would: Answer A. Shift the equilibrium to the right B. Shift the equilibrium to the left C. No change

  3. Chemistry

    Consider the following equilibrium process at 700°C: 2H2 + S2 ↔ 2H2S Analysis shows that there are 2.50 moles of H2, 1.35x10^-5 mole of S2, and 8.70 moles of H2S present in a 12.0-L flask. Calculate the equilibrium constant Kc

  4. chemistry

    Which of the following solutes dissolved in 1000 g of water would provide a solution with the LOWEST freezing point? A. 0.030 mole urea, CO(NH2)2 B. 0.030 mole acetic acid, CH3COOH C. 0.030 mole ammonium nitrate, NH4NO3 D. 0.030

  1. chemistry

    given the reactant amounts specified in each chemical eguation, determine the limiting reactant in each case: a. HCL+NaOH->NaCl+H2O 2.0 mole of HCl 2.5 mole NaOH b. Zn+2HCl->ZnCl2+H2 2.5 mole Zn 6.o mole HCl c.

  2. A.P. Chemistry

    You have solutions of 0.200 M HNO2 and 0.200 M KNO2 (Ka for HNO2 = 4.00  10-4). A buffer of pH 3.000 is needed. What volumes of HNO2 and KNO2 are required to make 1 liter of buffered solution?

  3. Chemistry (please help me!)

    H2(g) + CO2(g) H20(g) + CO(g) When H2(g) is mixed with CO2(g) at 2,000K, equilibrium is achieved according to the equation above. In one experiment, the following equilibrium concentrations were measured: [H2]=0.20 M [CO2]=0.30 M

  4. Chemistry

    Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO2(g). 2SO2(g)+O2(g)=2SO3(g) Kc=1.7*10^8 [SO3]aq=0.0034 M [O2]aq=0.0018

  1. CHEMISTRY HELP!

    Consider the following reactions and their equilibrium constants. (NO(g) + 0.5Br2(g) NOBr(g) Kp = 5.3 2NO(g) N2(g) + O2(g) Kp = 2.1 x 1030 Use these equations and their equilibrium constants to determine the equilibrium constant

  2. Analytical Chemistry

    Carbon dioxide dissolves in water to form carbonic acid, which is primarily dissolved CO2. Dissolved CO2 satisfies the equilibrium equation. CO2(g) CO2(aq) The acid dissociation constants listed in most standard reference texts

  3. Chemistry

    1.5 mole of PCl5 are heated at constant temperature in a closed vessel of 4 litres capacity.At the equilibrium,PCl5 is 35percent dissociated into PCl3 and Cl2.calculate the equilibrium constant.

  4. chemistry

    Stearic acid, nature's most common fatty acid, dimerizes when dissolved in hexane: 2C17H35COOH Picture (C17H35COOH)2; ΔH°rxn = -172 kJ The equilibrium constant for this reaction at 28°C is 2900. Estimate the equilibrium

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