Calculate the pH of a 500.0 mL solution that is 0.30 M NH3 and 0.50 M NH4Br. For NH3, Kb = 1.76 × 10-5 .
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Calculate the pH of a 500.0 mL solution that is 0.30 M NH3 and 0.50 M...
find pH when a 500.0 mL solution has 0.30 M NH3 and 0.50 M NH4Br. For NH3, Kb = 1.76 × 10-5 .
37. You have 500.0 mL of a buffer solution that is 0.30 M HF and 0.50 M KF. Ka for HF is 7.1 x 10-4 a) Calculate the pH of the buffer. b) Calculate the pH of the buffer after adding 0.020 moles of HCI. c) Calculate the pH of the buffer after adding 0.030 moles KOH. - -Loel.
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?
A 110.0 mL buffer solution is 0.100 M in NH3 and 0.125 M in NH4Br. (Kb of NH3 is 1.76×10−5.) question: If the same volume of the buffer were 0.250 M in NH3 and 0.395 M in NH4Br, what mass of HCl could be handled before the pH falls below 9.00? Help ASAP Please!!!!!
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?
A 120.0 ml. buffer solution 0.110 M NH3 and 0.135 M NH4Br. (Kb of NH3 is 1.76 x10^-5) Part B If the same volume of the butter were 0.265 M NH3 and 0.390 Min NH Br. What mass of HCl could be handled before the pH als below 9.00? Express the mass in grams to three significant
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.
Calculate the pH of a 0.401 M solution of NH4Br (Kb of NH3 = 1.8 x 10-5). Enter pH to 2 decimal places.
Given the solution 0.50 M NH3 (aq) with Kb = 1.75 * 10-5, calculate the pH using an I.C.E. table
Calculate the pH of a solution obtained by mixing 25.00 mL of 0.13 M NH3 with 25.00 mL of 5.0×10-2 M HCl. Kb for NH3 is 1.8×10-5.