Question

In: Chemistry

A 100 mL solution of .400 M Sodium Acetate (NaOAc) mixed with 100 ml of .400 M HCl.

Determine the [H3O+] and [OH-] for the following:

A 100 mL solution of .400 M Sodium Acetate (NaOAc) mixed with 100 ml of .400 M HCl.

Solutions

Expert Solution

When we add HCl to the Sodium Acetate (NaOAc) solution,it forms a buffer solution.

pH for the buffer solution can be calculated by using Handerson's equation.

pH = pKa + log [salt]/[acid]

for acetic acid buffer , pKa = 4.74

we need to calculate [salt] and [acid]

                     NaOAc                     +             HCl                      ------------------>            AcOH         + NaCl

                100ml x 0.4M                        100ml x 0.4M                                                    0                   0

at t=0       = 0.1L x 0.4M                            0.1L x 0.4M                                                  0                   0

                = 0.04moles                              0.04moles                                                     0                   0

after the reaction

                   (0.04-0.04) moles                (0.04-0.04) moles                                          0.04moles   

Hence salt NaOAc reacts completely after the reaction.

We cannot calculate the pH and then [H3o+] and [OH-]

queen_honey_blossom answered 1 year ago
Next > < Previous

Related Solutions

A solution of 100 mL of .200M sodium chromate is mixed with a solution of 200...
A solution of 100 mL of .200M sodium chromate is mixed with a solution of 200 mL of 0.150M strontium nitrate. What is the is the limiting reagent or reacting? How many grams of percipitate forms? What is the concentration of spectator ions in the final mixture? What is the concentration of the excess ion?
A 100. ml sample of 0.10 M HCl is mixed with 50. ml of 0.10 M...
A 100. ml sample of 0.10 M HCl is mixed with 50. ml of 0.10 M NH3. What is the resulting pH? Thank you!
Add 10 mL of 0.1 M HCl to one liter of a 0.10 M sodium acetate...
Add 10 mL of 0.1 M HCl to one liter of a 0.10 M sodium acetate buffer, pH 6.76 (pKa = 4.76 for acetic acid). Does the pH of the solution change? Determine the effect of the addition of 20.0 mL of 0.100 M HCl?
A 200 mL solution of .100 M solution of Ammonia, NH3, is slowly mixed with .100...
A 200 mL solution of .100 M solution of Ammonia, NH3, is slowly mixed with .100 M HCl. Determine the pH after addition of: 0 ml of HCl, 50 mL of HCl, 100 mL of HCl, 200 mL of HCl, and 250 mL of HCl.
A 200 mL solution of .100 M solution of Ammonia, NH3, is slowly mixed with .100...
A 200 mL solution of .100 M solution of Ammonia, NH3, is slowly mixed with .100 M HCl. Determine the pH after addition of: 0 ml of HCl, 50 mL of HCl, 100 mL of HCl, 200 mL of HCl, and 250 mL of HCl.
What is the pH of solution if 40 mL 0.1 M HCl is mixed with 60...
What is the pH of solution if 40 mL 0.1 M HCl is mixed with 60 mL 0.2 M HAc?
If 100.mL of 0.035 M HCl solution is added to 220.mL of a buffer solution which...
If 100.mL of 0.035 M HCl solution is added to 220.mL of a buffer solution which is 0.20M in NH3 and 0.18M in NH4Cl, what will be the pH of the new solution? The Kb of NH3 is 1.8x10^-5. Please explain how the answer was obtained. Thank you!
A 250.00 mL buffer solution is 0.250 M acetic acid (CH3COOH) and 0.100 M sodium acetate...
A 250.00 mL buffer solution is 0.250 M acetic acid (CH3COOH) and 0.100 M sodium acetate (NaCH3COO). The Ka of acetic acid is 1.8 • 10-5 at 25 o C. Calculate the pH of the resulting buffer solution when 10.00 mL of a 0.500 M aqueous HCl solution is added to this mixture.
A 168.5 mL sample of 0.087 M HCl is mixed with 50.2 mL of 0.089 M...
A 168.5 mL sample of 0.087 M HCl is mixed with 50.2 mL of 0.089 M NH3. What is the resulting pH? (The Kb for NH3 = 1.8 x 10^5).
250. mL of 0.600 M HCl is mixed with 250. mL of 0.600 M NaOH ,...
250. mL of 0.600 M HCl is mixed with 250. mL of 0.600 M NaOH , resulting in a neutralization reaction with net ionic equation: H+ (aq) + OH- (aq) → H2O(ℓ) ∆Hrxn = -57.0 kJ Assume the solutions have specific heat capacity of 4.18 J/g C , and the solutions have a density of 1.00 g/mL. The reaction takes place in a coffee-cup calorimeter, and all heat transfer occurs within the confines of the calorimeter. If the initial temperature...
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT