Calculate the pH after .02 mol of HCl is added to 1 liter of a mixture containing .1M NH3 and .1M NH4Cl
Calculate the pH after .02 mol of HCl is added to 1 liter of a mixture...
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.
Calculate the pH of a mixture, 31.25 mL of 0.225 M NaOH, after 15.00 mL of 0.350M HCl is added to the solution. Write the answer in 4 significant figures.
Calculate the change in pH when 7.00 mL of .100 M HCL (aq) is added to 100.0 mL of a buffer solution that is .100 M in NH3 (aq) and .100 M in NH4CL. plse help
Calculate the pH after 0.020 mol NaOH is added to 1.00 L of each of the solutions below. (a) 0.115 M HONH2 (K, -1.1 x 108) 402 (b) 0.115 M HONH3C 402 12:30 (d) a mixture containing 0.115 M HONH2 and 0.115 M HONH3cl 402
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= ?
numbers 8-10 8. Determine the pH of a solution in which 1.00 mol H2C03 (Ka 4.2 x 10-) and 1.00 mole NaHCOs are dissolved in enough water to form 1,00 L of solution. 9. How many moles of NaHCO3 should be added to one liter of 0.100 M H2CO3 (Ka4.2x 10-7) to prepare a buffer with pH 7.00? 10) Determine the pH of 0.01 M NH3 (Kb= 1.8 x 10-5) when an equal volume of 0.05 M NH4Cl is added....
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.
Given a 1.00 L solution that is 0.60 M HF and 1.00 M KF, calculate the pH after 0.060 mol NaOH is added, and calculate the pH after 0.20 mol HCl is added to the original solution. Ka = 7.2x10-4 pH = when NaOH is added pH = when HCl is added
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.
What is the pH after 0.29 moles of NaOH is added to a 1.00L buffer containing 1.00 moles of NH3 and 1.00 moles NH4Cl ? Kb NH3 = 1.8 x 10-5