Chemistry (Acids and Bases)

posted by .

I just did a lab on Acids and Bases and I am having trouble with the lab questions I was given to complete.

Concentration of NaOH: 0.09999 M
Volume of NaOH: 3.25 mL
# moles of NaOH: 0.325 moles
Initial Concentration of Weak Acid: ? (How do we calculate this)

Part 2: Hydrolysis of Salts
a) Potassium Chloride has a pH of 7 and a yellow-green universal colour indicator. Explain with an equation to show hydrolysis
b) Sodium Acetate has a pH of 8 and a dark green universal colour indicator. Explain using equation
c) Ammonium Chloride has a pH of 5.5 and orange universal colour indicator. Explain using equations.

Part III: Buffers
Concentration of acetic acid (0.1 M volume used) : 20 mL
Concentration of sodium acetate (0.1 M volume used) : 25 mL
Concentration of hydrochloric acid (0.1 M volume used) : 5 mL

pH Measured of buffer solution: 4.55
pH Measured of buffer +5 mL of 01 M HCl: 4.20
We have to now determine the pH calculated for both solutions above.

I would greatly appreciate the help or any guidance to these questions. Thanks!

  • Chemistry (Acids and Bases) -

    Concentration of NaOH: 0.09999 M
    Volume of NaOH: 3.25 mL
    # moles of NaOH: 0.325 moles
    Initial Concentration of Weak Acid: ? (How do we calculate this)

    There isn't enough information to work the problem here. (weak acid) = moles NaOH/volume weak acid used in the titration. All this is ok if the acid is a monoprotic acid.

    Part 2: Hydrolysis of Salts
    a) Potassium Chloride has a pH of 7 and a yellow-green universal colour indicator. Explain with an equation to show hydrolysis
    b) Sodium Acetate has a pH of 8 and a dark green universal colour indicator. Explain using equation
    c) Ammonium Chloride has a pH of 5.5 and orange universal colour indicator. Explain using equations.
    KCl doesn't hydrolyze; therefore, the pH is 7.0.
    Part b. Sodium acetate. Sodium is not hydrolyzed but acetate is producing acetic acid and hydroxide ion. You can write the equation and see that the solution is basic.
    part c. NH4Cl. Cl is not hydrolyzed. NH4^+ is. I will let you write the equation to obtain H3O + ?? showing that the solution is acidic.


    Part III: Buffers
    Concentration of acetic acid (0.1 M volume used) : 20 mL
    Concentration of sodium acetate (0.1 M volume used) : 25 mL
    Concentration of hydrochloric acid (0.1 M volume used) : 5 mL

    pH Measured of buffer solution: 4.55
    pH Measured of buffer +5 mL of 01 M HCl: 4.20
    We have to now determine the pH calculated for both solutions above.

    Use the Henderson-Hasselbalch equation.

  • Chemistry (Acids and Bases) -

    Thanks for the help

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. --- Chemistry ---

    What is the most common chemical method for removing H_30^+ ions in aqueous solution?
  2. chemistry

    Because solution pH is a measurement of either [H3O+] or [-OH] concentration, the acidic or basic nature of the acids and bases used in this experiment can be ascertained by inspecting just the density (electrostatic) potentials from …
  3. General Chemistry-Acids/Bases

    I'm stuck on a couple of similar problems involving pH and acids/bases 1) What is the final pH of a 1L solution that is initially .15 M HF and .2 M NaF after 10 mL of .02 M HCl has been added?
  4. Chemistry

    I just did a lab on Acids and Bases and I am having trouble with the lab questions I was given to complete. Concentration of NaOH: 0.09999 M Volume of NaOH: 3.25 mL # moles of NaOH: 0.325 moles Initial Concentration of Weak Acid: ?
  5. chemistry

    Question about titration calculations in analysis of antacids lab. We did a lab yesterday with antacids, HCl and NaOH and I'm having trouble doing the calculations. The information known is the following: 1)0.10M NaOH 2)0.10M HCl 3)Mass …
  6. Chemistry

    Could someone please help me complete my lab experiment. Antacid Brand: Life Concentration of HCl: 0.1845 M Concentration of NaOH: 0.1482 M Trial 1: 1.Mass of Table: 1.2173g 2.Volume of HCl added: 75.0 mL 3.Milliomoles of HCl added:mmoles …
  7. Chemistry - Acids and Bases

    What's a good example of a balanced neutralization reactions involving strong acids and bases?
  8. Chemistry

    A concept map was to be created on acids and bases. The concept terms that were given to use were: aqueous solution,bases,acids,ions,weak bases, strong bases, strong acids, weak acids,dissociation, weak electrolyte, strong electrolyte,reaction,salt, …
  9. Chemistry - Acid and Bases

    In aqueous solution, classify these compounds as strong acids, weak acids, strong bases, weak bases, or other. HNO3 HBr HF CH3COOH H3PO4 NaOH Ba(OH)2 (CH3)3N NH3 NaCl
  10. Chemistry (molarity) (sorta an emergency)

    I'm doing a titration lab and writing a lab report where I'm sort of stuck on how exactly to find the concentration of HCl. These are the following info I have from the lab, Equation: HCl(aq)+NaOH(aq)-> H2O(l)+NaCl(aq) -Calculated …

More Similar Questions