college chem

a. According to the Henderson-Hasselbalch equation, how many grams of sodium acetate will you need to add to 125 mL of 0.100 M acetic acid to make a pH=4.74 buffer?

b. What is the actual pH of the resulting buffer when you add that many grams of sodium acetate to 125 mL of 0.100 M acetic acid?

c. If I want to make the buffer by adding 0.100 M NaOH instead of sodium acetate, how many milliliters of NaOH are needed to reach pH=4.74?

d. If I add enough water to the above buffer to make the total volume 1.00 L, what's the new pH?

e. How many milliliters of 0.25 M HCl will be needed to change the pH of the dilute buffer by 1 pH unit?

  1. 👍
  2. 👎
  3. 👁
  1. 1.025

    im trying to get last two as well

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    use the Henderson-Hasselbalch equation to calculate the pH of a buffer solution prepared by mixing equal volumes of 0.20 M NaHCO3 and 0.10M Na2CO3.(Ka=5.6x10^-11). how would you prepare NaHCO3-Na2CO3 buffer solution that has the

  2. chemistry

    A buffer is prepared using acetic acid, CH3COOH, (a weak acid, pKa = 4.75) and sodium acetate, CH3COONa (which provides acetate ions, the conjugate base), according to the following proportions: Volume of CH3COOH(aq): 100.0 mL

  3. AP Chemistry

    A 0.3500 MHCl solution was used to titrate a 21.60 mL sodium acetate solution. The endpoint was reached after 25.75 mL of titrant were added. Find the molar concentration of sodium acetate in the original solution.

  4. Science- Chemistry

    How many grams of sodium acetate( molar mass 82.03 g/mol) must me added to 1.00L of a 0.200M acetic acid solution to form a buffer of 4.20?Ka value for aceic acid is 1.8 x 10^-5. How do I go about finding the grams from the given

  1. Chemistry

    Write the following into a balanced equation. a) When a mixture of copper (II) oxide and carbon is heated, elemental copper forms and carbon monoxide evolves into the atmosphere. b) When a concentrated solution of sodium hydroxide

  2. Chemistry

    Identify the salt that is produced from the acid-base neutralization reaction be- tween sodium hydroxide and hydrocyanic acid (HCN). 1. sodium cyanide 2. sodium acetate 3. sodium amide 4. sodium formate

  3. Chemistry

    What mass in grams of a 0.500 m(molal) solution of sodium acetate, CH3CO2Na, in water would you use to obtain 0.200mol of sodium acetate?

  4. Chemistry

    Use the Henderson-Hasselbalch equation to calculate the pH of each solution: a solution that contains 1.05% C2H5NH2 by mass and 1.10% C2H5NH2Br by mass

  1. school

    What is the pH of 0.1 M formic acid solution? Ka=1.7„e10-4? What is the pH value of buffer prepared by adding 60 ml of 0.1 M CH3COOH to 40 ml of a solution of 0.1 M CH3COONa? What is the pH value of an acetate buffer (pK=4.76)

  2. Chemistry

    A buffer solution contains HC2H3O2 at a concentration of 0.225 M NaC2H3O at a concentration of 0.164 M. The value of Ka for acetic acid is 1.75 × 10-5. Calculate the pH of this solution using the Henderson-Hasselbalch equation.

  3. chemistry

    Write the balanced chemical equation for the reaction of sodium bicarbonate with aqueous acetic acid to produce carbon dioxide, water, and sodium acetate. Follow the example set by the sodium bicarbonate.

  4. Chenistry

    Be able to calculate the pH of a solution prepared by mixing 50.0mL of 0.200M NaH2PO4 (pKa2=7.20) with 50.0mL of 0.120M NaOH. I did work out a pH of 7.38 but I am not sure if i need to take into account any dilution of the mixing

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