1) Calculate the pH of a solution produced by mixing 100.0 mL of 0.10 M HCl(aq) and 100.0 mL of 0.20 M NaOH(aq).
2) Calculate the pH of an aqueous solution made by mixing 100.0 mL of 0.40 M NH4Cl and 50.0 mL of 0.40 M NaOH. The pKa of NH4+ is 9.24.
Therefore, (1) pH = 12.70 (strong base involved; higher pH).
(2) pH = 9.54 (base involved, is weak; lower pH).
1) Calculate the pH of a solution produced by mixing 100.0 mL of 0.10 M HCl(aq)...
Quick Please! Calculate the pH of a solution produced by mixing 100.0 mL of 0.10 M HCl(aq) and 100.0 mL of 0.20 M NaOH(aq). O 12.7 1.00 O O 1.30 O 13.0 O 12.0
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 NH4Cl(aq). NH3 Kb=1.8x10^-5 Calculate the change in pH when 3.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution.
As 50.0 mL of 0.10 M HCl is added to 100.0 mL of 0.10 M NaOH, what happens to the pH of the NaOH solution?
A)Calculate the change in pH when 8.00 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 NH4Cl(aq). A list of ionization constants can be found here. B)Calculate the change in pH when 8.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution.
2) a) Calculate the change in pH when 8.00 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 NH4Cl(aq). delta pH= ? b) Calculate the change in pH when 8.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution. delta pH= ?
Calculate the pH of a solution made by mixing 100.0 mL of 0.874 M NH3 with 100.0 mL of 0.100 M HCl. (Kb for NH3 = 1.8 10
3. (a) Calculate the change in pH when 5.00 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 NH4Cl(aq). (b) Calculate the change in pH when 5.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution.
Calculate the pH of a solution made by mixing 100.0 mL of 0.355 M NH3 with 100.0 mL of 0.100 M HCl. (Kb for NH3 = 1.8 10–5) Select one: a. 9.66 b. 8.85 c. 4.34 d. 9.26
3) Calculate the pH of the following solutions: a. 100.0 mL of 0.20 M HCH3CO2 (acetic acid), ka = 1.8x10 b. 100.0 mL of 0.20 M HCH,CO, plus 25.0 mL of 0.40 M NaOH c. 100.0 mL of 0.20 M HCH3CO, plus 50.0 mL of 0.40 M NaOH d. 100.0 mL of 0.20 M HCH,CO2 plus 75.0 mL of 0.40 M NaOH
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 NH, (aq) and 0.100 M in NHCl(aq). Consult the table of ionization constants as needed. ApH = Calculate the change in pH when 3.00 mL of 0.100 M NaOH is added to the original buffer solution. ApH =