you add 1 ml of 0.1M HCl to a solution containing 10ml of 0.2M acetic acid...

you add 1 ml of 0.1M HCl to a solution containing 10ml of 0.2M acetic acid (Ka = 1.8x10-5) and 10ml of 0.2 M sodium acetate. What is the resulting pH?

Expert Solution

no of moles of CH3COOH = molarity * volume in L

= 0.2*0.01 = 0.002moles

no of moles of CH3COONa = molarity * volume in L

= 0.2*0.01 = 0.002 moles

no of moles of HCl = molarity * volume in L

= 0.1*0.001 = 0.0001moles

no of moles of CH3COOH after addition of 0.0001 moles of HCl = 0.002+0.0001 = 0.0021 moles

no of moles of CH3COONa after addition of 0.0001 moles of HCl = 0.002-0.0001 = 0.0019 moles

PKa = -logKa

= -log1.8*10^-5

=4.74

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

= 4.74 + log0.0019/0.0021

= 4.74 -0.04346

= 4.6965 >>>>answer

queen_honey_blossom answered 1 year ago

How do you calculate the molarity of 40 mL of 0.1M acetic acid (HC2H3O2) solution if...

How do you calculate the molarity of 40 mL of 0.1M acetic acid (HC2H3O2) solution if 12.76 mL 0.35 NaOH was added to reach the equivalence point?

If you started with an acetic acid solution of 2.0 mL of 0.84M Acetic acid and...

If you started with an acetic acid solution of 2.0 mL of 0.84M Acetic acid and shifted it with 0.2mL of 0.01M HCl (4 drops), what is the new pH?. Initial pH Final pH Ka of acetic acid = 1.8 x 10-50.3 Start by finding the equilibrium concentrations of the acetic acid solution. Calculate the Ph based on this initial concentration (initial Ph). Calculate the moles of everything (compounds in the equilibrium AND the acid). Shift the equilibrium with the...

What is the pH of 10ml of 0.1M NH3, with 5ml of 0.1M of HCL. kb=1.8*10^-5

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.

QUESTION 10 Calculate the change in pH if 10mL of 0.1M HCl is added to the...

QUESTION 10 Calculate the change in pH if 10mL of 0.1M HCl is added to the buffer made by mixing 25 mL of 1.0 M CH3COOH and 25 mL of 0.5 M CH3COONa. For these types of questions where a strong acid or base is added to a buffer solution, first write out the chemical reaction. What will the HCl react with: CH3COOH or CH3COO−? Since HCl is an acid, it will react with CH3COO-. Because HCl is a strong...

If you add strong acid (such as HCl) to the Tris solution above(25mM solution in 200mL)...

If you add strong acid (such as HCl) to the Tris solution above(25mM solution in 200mL) you can lower the pH. Using the Henderson-Hasselbalch equation (H-H), calculate how much strong acid in mM is need to lower the pH from 10.4 to 8.0. Remember pKa is 8.2. You might start by determining the amount of acid and base you have at each pH using the H-H equation. Then compare the differences in this ratio between the two pH values.

what is the ph of a 0.1M hydrochloric acid solution? A 1.0×10^-3M HCl solution? A 1.0...

what is the ph of a 0.1M hydrochloric acid solution? A 1.0×10^-3M HCl solution? A 1.0 × 10^-8 M HCl solution?

You measured the pH of a 0.1M HCl solution. If you had diluted this solution by...

You measured the pH of a 0.1M HCl solution. If you had diluted this solution by adding 100mL of water, what happens to the concentration of H3O+?

A 15.3 mL sample of vinegar, containing acetic acid, was titrated using 0.809 M NaOH solution....

A 15.3 mL sample of vinegar, containing acetic acid, was titrated using 0.809 M NaOH solution. The titration required 24.06 mL of the base. Assuming the density of the vinegar is 1.01 g/mL, what was the percent (by mass) of acetic acid in the vinegar?

Consider the titration of a 12.0 mL solution containing 0.200 mol/L acetic acid (CH3COOH, Ka =...

Consider the titration of a 12.0 mL solution containing 0.200 mol/L acetic acid (CH3COOH, Ka = 1.8 x 10-5 ), with a solution of 0.250 mol/L KOH. (12 points total) i) Determine the pH of the solution when 4.80 mL of KOH has been added. ii) Determine the pH of the solution when 14.00 mL of KOH has been added.

Question