We have 500.0 mL of a buffer solution that is 0.636 M in NH3 and 0.345 M in NH4Cl. We add 500.0 mL of a solution 0.249 M in HCl. The final volume is 1.0000 L. The Kb value for NH3 is 1.8 x 10-5. What is the pH of the final solution?
We have 500.0 mL of a buffer solution that is 0.636 M in NH3 and 0.345...
1) For the reaction A(aq) ---> B(aq) the change in the standard free enthalpy is 3.39 kJ at 25 oC and 5.34 kJ at 45 oC. Calculate the value of this reaction's equilibrium constant at 75 oC. 2) We have 500.0 mL of a buffer solution that is 0.657 M in NH3 and 0.319 M in NH4Cl. We add 500.0 mL of a solution 0.238 M in HCl. The final volume is 1.0000 L. The Kb value for NH3 is...
Question 1 : For the reaction A(aq) ---> B(aq) the change in the standard free enthalpy is 3.37 kJ at 25 oC and 4.81 kJ at 45 oC. Calculate the value of this reaction's equilibrium constant at 75 oC. Question 2 : A container encloses 33.0 g of CO2(g). The partial pressure of CO2 is 2.44 atm and the volume of the container is 28.8 L. What is the average, or root mean square, speed (in m/s) of the CO2molecules...
if 155 mL of 0.043 M HCl solution is added to 235 mL of a buffer solution which is 0.33 M in NH3 and 0.56 M in NH4Cl, what will be the pH of the new solution? the Kb of NH3 is 1.8*10^-5
You have a 750mL of a buffer solution that is composed of NH3 and NH4Cl with a Kb value 1.8x 10^5 and a pH 9.43...... How many mL 6.00M HCl can be added before the buffer is exhausted?
What is the pH of a buffer formed from 50 mL of 15.0 M NH3 and 53.5 g of NH4Cl in enough water to make 500 mL of solution? (Kb = 1.8 x 10-5)
A 130.0 −mL buffer solution is 0.110 M in NH3 and 0.135 M in NH4Br. The Kb value for NH3 is 1.76×10−5. If the same volume of the buffer were 0.270 M in NH3 and 0.390 M in NH4Br, what mass of HCl could be handled before the pH falls below 9.00?
38. A buffer solution is 0.40 M NH3 and 0.60 M NHACI. Kb for NH3 is 1.8 x 10-5 a) Calculate the pH for the buffer system. b) Calculate the pH of the solution after adding 0.00600 moles of NaOH to 400.0 mL of the buffer. c) Calculate the pH of the solution after adding 0.050 moles of HCl to 600.0 mL of the buffer.
A 130.0 −mL buffer solution is 0.105 M in NH3 and 0.135 M in NH4BrNH4Br. The Kb value for NH3 is 1.76×10−5 Part A What mass of HCl can this buffer neutralize before the pH falls below 9.00? Part B If the same volume of the buffer were 0.265 M in NH3 and 0.390 M in NH4Br, what mass of HCl could be handled before the pH falls below 9.00? Express the mass in grams to three significant figures.
What volume of 0.200 M HCl must be added to 500.0 mL of 0.250 M NH3 to have a buffer with a pH of 8.81? Ka for NH4+ is 5.6x10-10. Volume =. L
3) Kb for NH3 1.8 x 10-5 a) Calculate the pH of a buffer solution that is 0.100 M NH3 and 0.120 M NHANO3. b) What is the pH after 60.0 mL of 0.010 M HCl is added to 90.0 mL of the buffer solution in 2(a). Assume the change in volume is additive. c) What is the pH after 60.0 mL of 0.010 M Ca(OH)2 is added to 90.0 mL of the buffer solution in 2(a). Assume the change...