(a) What is the pH of a solution that contains 0.100 M HClO and 0.300 M KClO? (b) If 50.00 mL of 0.100 M HCl is added to 1.00 L of the above buffer, what is the new pH?
(b) If 50.00 mL of 0.100 M HCl is added to 1.00 L of the above buffer, what is the new pH?
pKa for HClO = 7.53
From Henderson equation
pH = pKa + log {[Conjugate base] / [Acid]}
pH = 7.53 + log {[KClO] / [HClO]} = 7.53 + log ( 0.300 M / 0.100 M ) = 7.53 + log 3 = 7.53 + 0.477 = 8.00
pH = 8.00
b) Concentration of HCl added = 0.100 M = 0.100 mol/L
Volume of HCl solution added = 50.00 ml = 50.00 L / 1000 = 0.05 L
Number of moles of HCl added = 0.100 mol/L * 0.05 L = 0.005 mol
Concentration of KClO = 0.300 M = 0.300 mol/L
Concentration of HClO = 0.100 M = 0.100 mol/L
Volume of buffer solution = 1.0 L
Number of moles of HClO = 0.100 mol/L * 1.0 L= 0.100 mol
Number of moles of KClO = 0.300 mol/L * 1.0 L = 0.300 mol
After addition of HCl,
Number of moles acid = (0.100 + 0.005) mol = 0.105 mol
Number of moles of conjugate base = ( 0.300 - 0.005) mol = 0.295 mol
From Henderson equation,
pH = 7.53 + log ( 0.295 / 0.105) = 7.53 + log 2.81 = 7.53 + 0.4487 = 7.98
New pH after addition of HCl = 7.98
(b) question a and b are same.
(a) What is the pH of a solution that contains 0.100 M HClO and 0.300 M...
A a 50.00-mL sample of bleach solution contains 0.289 M HClO and 0.602 M NaClO. The Ka of hypochlorous acid is 3.0 ✕ 10−8. Find the pH of the solution. The solution is then divided in half. A) To one half of the original solution, 10.00 mL of 0.100 M NaOH is added. What is the final pH of this solution? B) To the other half of the original solution, 1.00 mL of 0.100 M HCl is added. What is...
A a 50.00-ml sample of bleach solution contains 0.233 M HClO and 0.499 M Nacio. The K, of hypochlorous acid is 3.0 x 10-8 Find the pH of the solution. C The solution is then divided in half. A) To one half of the original solution, 10.00 mL of 0.100 M NaOH is added. What is the final pH of this solution? B) To the other half of the original solution, 1.00 mL of 0.100 M HCl is added. What...
A buffer solution is made that is 0.455 M in HClO and 0.455 M in KClO. (1) If Ka for HClO is 3.50×10-8, what is the pH of the buffer solution? (2) Write the net ionic equation for the reaction that occurs when 0.102 mol HCl is added to 1.00 L of the buffer solution. Use H3O+instead of H+.
a 50.0 mL solution initially contains 0.300 M HCIO and 0.250 M KClO. what is the new pH after 1.0 mL of 2.0 M HBr is added ? Ka = 2.9 x 10^-8
You are given a 100.0 mL buffer that is 0.50 M HClO and 0.76 M in NaClO (Ka for HClO= 3.5x10^-8). What would the pH of the buffer solution change to if we added 10.0 mL 1.00 M HCl?
A buffer with a pH of 3.92 contains 0.19 M of sodium benzoate and 0.36 M of benzoic acid. What is the concentration of [H3O+] in the solution after the addition of 0.054 mol HCl to a final volume of 1.7 L? Assume that any contribution of HCl to the volume is negligible. [H3O+] = M Allerede C., Calculate the change in pH when 7.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that...
a) Calculate the pH of 0.500 L of a buffer solution that contains 0.200 M of benzoic acid C6H5CO2H and 0.100 M sodium benzoate NaC6H5CO2. Ka = 6.3 x 10-5. b) Calculate the pH after .10 mL of 1.00 M H+ has been added. c) Calculate the pH after 10 mL of 1.00 M OH- has been added.
1 . If a buffer solution is 0.260 M in a weak acid (?a=8.3×10−5)and 0.480 M in its conjugate base, what is the pH? pH= 2. If a buffer solution is 0.200 M in a weak base (?b=5.0×10−5) and 0.530 M in its conjugate acid, what is the ph 3. Phosphoric acid is a triprotic acid (?a1=6.9×10−3, ?a2=6.2×10−8 , and ?a3=4.8×10−13 To find the pH of a buffer composed of H2PO4 - (aq) ) and HPO4 2− (aq) , which...
Calculate the change in pH when 3.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3 (aq) and 0.100 M in NH4CI(aq). Consult the table of ionization constants as needed ДрН Calculate the change in pH when 3.00 mL of 0.100 M N2OH is added to the original buffer solution. АрН -
A 60.0 ml simple of 0.100 m nabob is t if rated with 0.300 m hcl what is the initial ph prior to the stand of the traction (before any HCL is added)? what is the ph at the equivalence point for the above in g.