Question

In: Chemistry

If you had a liter of buffer that originally consisted of 0.150 M acetic acid (Ka...

If you had a liter of buffer that originally consisted of 0.150 M acetic acid (K_a = 1.76 X 10^-5) and 0.250 M sodium acetate and then added 0.020 mol of NaOH, what would then be the final pH? Assume the volume of the added NaOH to be negligable.

Expert Solution

no of moles of CH3COOH = molarity * volume in L

= 0.15*1 = 0.15 moles

no of moles of CH3COONa = molarity * volume in L

= 0.25 *1 = 0.25 moles

Ka = 1.76*10^-5

PKa = -logKa

= -log1.76*10^-5

= 4.7544

PH = PKa + log[CH3COONa]/[CH3COOH]

= 4.7544 + log0.25/0.15

= 4.7544 + 0.2218 = 4.9762

no of moles of NaOH = 0.02moles

no of moles of CH3COOH by the addition of 0.02moles of NaOH = 0.15-0.02 = 0.13 moles

no of moles of CH3COONa by the addtion of 0.02 moles of NaOH = 0.25+0.02 = 0.27moles

PH = Pka + log[CH3COONa]/[CH3COOH]

= 4.7544 + log0.27/0.13

= 4.7544 + 0.3174 = 5.0718 >>>>answer

queen_honey_blossom answered 2 years ago

Calculate the percent ionization of 1.50 M aqueous acetic acid solution. For acetic acid, Ka =...

Calculate the percent ionization of 1.50 M aqueous acetic acid solution. For acetic acid, Ka = 1.8 × 10−5 . (a) 2.71% (b) 3.55% (c) 1.78% (d) 0.35% (e) None of the above

A 35.0-mL sample of 0.150 M acetic acid (CH3COOH) is titrated with 0.150 MNaOHsolution. Calculate the...

A 35.0-mL sample of 0.150 M acetic acid (CH3COOH) is titrated with 0.150 MNaOHsolution. Calculate the pH after the following volumes of base have been added. 35.5 mL Express your answer using two decimal places.

For the titration of 50.0 mL of 0.150 M acetic acid with 0.100 M sodium hydroxide,...

For the titration of 50.0 mL of 0.150 M acetic acid with 0.100 M sodium hydroxide, determine the pH when: (a) 50.0 mL of base has been added. (b) 75.0 mL of base has been added. (c) 100.0 mL of base has been added.

For the titration of 40.0 mL of 0.200 M acetic acid with 0.150 M sodium hydroxide,...

For the titration of 40.0 mL of 0.200 M acetic acid with 0.150 M sodium hydroxide, determine the pH when: (a) 40.0 mL of base has been added. (b) 53.3 mL of base has been added. (c) 66.6 mL of base has been added.

A 35.0-mL sample of 0.150 M acetic acid (CH3COOH) is titrated with 0.150 MNaOH solution. Calculate...

A 35.0-mL sample of 0.150 M acetic acid (CH3COOH) is titrated with 0.150 MNaOH solution. Calculate the pH after the following volumes of base have been adde Part A 35.5 mL Express your answer using two decimal places Part B 50.0 mL Express your answer using two decimal places

The Ka of acetic acid, CH3COOH, is 1.8 × 10-5. A buffer solution was made using...

The Ka of acetic acid, CH3COOH, is 1.8 × 10-5. A buffer solution was made using an unspecified amount of acetic acid and 0.30 moles of NaOOCCH3 in enough water to make 1.50 L of solution. The pH of the solution is 4.55. How many moles of CH3COOH were used? Could you please showing working on how to get the answer of 0.47.

pH of acetic acid solutions. Remember, acetic acid is a weak acid, with a Ka =...

pH of acetic acid solutions. Remember, acetic acid is a weak acid, with a Ka = 1.8 x 10−5. Obtain 10.0 mL of 0.10 M acetic acid and place in a clean dry 50.0 mL beaker. Predict the value of the pH. Measure the pH with the pH meter. Record the value. Take 1.00 mL of the 0.10 M CH3COOH(aq) in the previous step, and put it in another clean beaker. Add 9.00 mL of deionized water and stir. What...

Calculate the pH and pOH of a 0.50 M solution of Acetic Acid. The Ka of...

Calculate the pH and pOH of a 0.50 M solution of Acetic Acid. The Ka of HOAc is 1.8 x10-5 [H3O+]/(0.50-0.00095)=1.8x10-5 where did they get the .00095, its said to take that as the second assumption [H3O+]=9.4x10-4 [H3O+]/(0.50-0.00094)=1.85x10-5 [H3O+]=9.4x10-4 (this is said to be the third assumption) Please, please help I really dont understand this, please show all steps and be as descriptive as possible.

You have 500.0 mL of a buffer solution containing 0.20 M acetic acid and 0.30 M...

You have 500.0 mL of a buffer solution containing 0.20 M acetic acid and 0.30 M sodium acetate. What will the pH of the solution be after the addition of 20.0 mL of 1.00 M NaOH solution. Ka (CH3COOH) = 1.8x105 Please answer the question using ICE tables, I am unsure of whether to use 1 ICE table or 2 ICE Tables. Thank you.

Suppose you are titrating 50.00 mL of 0.1752 M acetic acid (CH3COOH; Ka = 1.76 ×...

Suppose you are titrating 50.00 mL of 0.1752 M acetic acid (CH3COOH; Ka = 1.76 × 10^-5) with 0.1998 M sodium hydroxide (NaOH). Calculate the pH of a titree solution when: (a) 15.25 mL of NaOH is added. (3 pts) (b) the equivalent volume (equivalence point) of NaOH is added. (4 pts) (c) a half of the equivalent volume is added (3 pts) (d) 46.00 mL of NaOH is added. (3 pts)