chemistry

Find a pH of a 0.100 M solution of the weak acid HA. The pKa for the acid 5.0

  1. 👍
  2. 👎
  3. 👁
  4. ℹ️
  5. 🚩
  1. ...............HA ==> H^+ + A^-
    I...............0.1.........0.......0
    C..............-x..........x........x
    E...........0.1-x........x.........x

    Ka = (H^+)(A^-)/(HA)
    Plug in values for Ka and the E line for the others. Solve for (H^+) which is x, then pH = -log(H^+)
    Post your work if you get stuck.

    1. 👍
    2. 👎
    3. ℹ️
    4. 🚩

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    pls help. A weak acid HA (pKa = 5.00) was titrated with 1.00 M KOH. The acid solution had a volume of 100.0 mL and a molarity of 0.100 M. Find the pH at the following volumes of base added and make a graph of pH versus Vb: Vb = 0,

  2. chemistry

    a 5.55g sample of a weak acid with ka=1.3*10^-4 was combined with 5.00ml of 6.00 M NAOH and the resulting solution was diluted to 750mL. The measured pH of the solution was 4.25. what is the molor mass of the weak acid. if used

  3. AP CHEM

    What is the pKa for the acid HA if a solution of 0.65 M HA and 0.85 M NaA has a pH of 4.75? ~~~I know you find the ph by doing -log of pka; how do you do the reverse when you have molarity? I am completely lost. :-(

  4. chemistry

    A. Strong Base 1.) What is the concentration of a solution of KOH for which the pH is 11.89? 2.) What is the pH of a 0.011M solution of Ca(OH)2? B. Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. Calculate the Ka

  1. chemistry

    A 15.00 mL sample of an unknown monoprotic weak acid solution is titrated with 0.35 M NaOH. The initial buret reading is 0.23 mL. The phenolphthalein indicator turns the solution light pink when the buret reads 29.58 mL. A. what

  2. AP Chemsitry

    A solution of an unknown monoprotic weak acid was titrated with 0.100 M NaOH. The equivalence point was reached when 37.48 ML of base had been added. From a second buret, exactly 18.74 of 0.100 M HCl were added to the titration

  3. chemistry

    Lactic acid is a weak acid with the formula , HCH3H5O3, the Ka for lactic acid is 1.38 x 10-4. In aqueous solution, lactic acid partially dissociates according to the following reaction: HCH3H5O3 ⇔ CH3H5O3- + H+ Use the Ka

  4. Chemistry

    Write the balanced NET IONIC equation for the reaction that occurs when ammonium chloride and calcium hydroxide are combined. This reaction is classified as A. Strong Acid + Strong Base B. Weak Acid + Strong Base C. Strong Acid +

  1. Chemistry-Dr Bob help!!

    0.100 M solution of a weak acid, HX, is known to be 15% ionized. The weak acid has a molar mass of 72 g/mol. 1. What is Ka for the weak acid? 2. What is the pH of the buffer prepared by adding 10.0 g of the sodium salt of the acid

  2. chemistry

    The Ka for a weak acid, HA, is 1.6x10-6. What are the (a) pH and (b) degree of ionization of the acid in a 10-3 M solution? (c) Calculate pKa and pKb

  3. Chemistry

    A 100 mL sample of 0.40 M hydrofluoric acid is mixed with 100.0 mL of 0.2M lithium hydroxide. Find the pH of the final solution. pKa for HF is 3.2.

  4. Chemistry

    A new potential heart medicine, code-named X-281, is being tested by a pharmaceutical company, Pharma-pill. As a research technician at Pharma-pill, you are told that X-281 is a monoprotic weak acid, but because of security

View more similar questions or ask a new question.