Chemistry

posted by .

Calculate pH when 0.060 mols of HCl are added to 1.000 L of a buffer containing 0.499M KH2PO4 and 0.193M K2HPO4

  • Chemistry -

    Use the Henderson-Hasselbalch equation and the ICE chart below.
    moles HPO4^2- = 0.193
    moles H2PO4^- = 0.499

    ...........HPO4^2- + H^+ ==> H2PO4^-
    initial....0.193......0.......0.499
    add..................0.06...............chchange.....-0.06.....0.06......+0.06
    equil.......0.133......0........0.493

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. CHEMISTRY

    A BUFFER SOLUTION IS MADE FORM 0.10 MOLES NaF AND 0.25 MOLES OF HF IN 1 LITER OF WATER ----WHAT WILL THE BUFFER CAPACITY BE IF 1.0M HCL IS ADDED -----WHAT IF 2.0 M OF NAOH IS ADDED?
  2. Chemistry - Buffers

    A buffer is formed by adding 500mL of .20 M HC2H3O2 to 500 mL of .10 M NaC2H3O2. What would be the maximum amount of HCl that could be added to this solution without exceeding the capacity of the buffer?
  3. Chemistry

    A buffer is made up of .300 L each of .500 M KH2PO4 and .317 M K2HPO4. Assuming tha the volumes are additive, calculate a) the pH of the buffer b) the pH of the bugger after the addition of .0500 mol of HCl to .600 L of the buffer. …
  4. chem

    I posted a question earlier that I was having trouble with, but I was unable to attempt to try it again for several days after posting. The question was: A buffer is made up of .300 L each of .500 M KH2PO4 and .317 M K2HPO4. Assuming …
  5. Chemistry

    You need to prepare 1.000 L (in a volumetric flask) of 0.50 M phosphate buffer, pH 6.77. Use the Henderson Hasselbalch equation with a value of 6.64 for pK2 to calculate the quantities of K2HPO4 and KH2PO4 you need to add to the flask. …
  6. Chemistry

    A pH = 7.6 buffer is needed in the lab. This buffer is made by first dissolving 17.42 g K2HPO4 in 600 mL of water. What is the pH of this salt solution?
  7. Chemistry

    A phosphate buffer solution contain 0.08 M K2HPO4 and 0.12 M KH2PO4. pKa values for H3PO4 are 2, 6.8, and 12.2. Calculate the concentrations of a) H3PO4 b) H2PO4- c) HPO42- d) H+ e) OH- f) K+
  8. Biochem

    Calculate the pH of the buffer system of 0.20M K2HPO4/0.25M KH2PO4
  9. Analytical Chemistry

    This question pertaining to buffer systems! How would you prepare 10.0mL of 0.0100M phosphate buffer, pH = 7.4 0, from stock solution of 0.100M KH2PO4 and 0.250M K2HPO4, pKa of KH2PO4 is 7.20. Please help me in figuring out how I even …
  10. Chemistry

    how would you prepare 250 mL solution containing the following: 0.30 M mannitol, 0.025 M phosphate buffer pH 7.5?

More Similar Questions