Calculate the change in pH that occurs when 0.00100 mol of gaseous HCl is added to a buffer solution that is prepared by dissolving 0.492 g of sodium acetate (molar mass = 82.03g/mol) in 250mL of 0.0150mol/L of acetic acid solution? Assume no change in volume upon addition of either the sodium acete or HCl. (Ka for acetic acid = 1.8x10^-5).

answer

watching

350

views

For unlimited access to Homework Help, a Homework+ subscription is required.

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

Deanna HettingerLv2

29 Jun 2019

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

Calculate the change in pH that occurs when 0.00100 mol of gaseous HCl is added to a buffer solution that is prepared by dissolving 4.92 g of sodium acetate ( molar mass= 82.03 g/mol) in 250 mL of 0.150 mol/L of acetic acid solution? Assume no change in volume upon addition of either the sodium acetate or HCl. (Ka for acetic acid = 1.8x10^-5) *please explain!*

Calculate the change in pH that occurs when 0.00100 mol of gaseous HCL is added to a buffer solution that is prepared by dissolving 4.92 g of sodium acetate (molar mass = 82.03 g/mol) in 250 ml of 0.150 mol/L of acetic acid solution?Assume no change in volume upon addition of either the sodium acetate or HCl. (Ka for acetic acid = 1.8 x 10^-5)

A 2.50 mL buffer solution is .250 mol in acetic acid and .250 molin sodium acetate. (Ka=1.8x10 to the -5).

A. What is the initial pH to the buffer solution?
B. What is the pH after addition of 0.010 moles of HCl?