J JimmyLewis Guest Jun 18, 2009 #1 what would be the pH of a solution made by mixing 0.1M NH3 and 0.1M NH4. the Kb of NH3 is 1.8x10 -5 ******NH4+ salt
what would be the pH of a solution made by mixing 0.1M NH3 and 0.1M NH4. the Kb of NH3 is 1.8x10 -5 ******NH4+ salt
T Tony P New member Jun 18, 2009 #2 well you can see that there is a conjugate acid and base pair. you know the value of Kb and the molarities are the same, so you can find the Ka value. The K value of water is 1.00 x 10-14 so just divide that by Kb to find Ka. Since the molarities of the two are equal pH=-logKa
well you can see that there is a conjugate acid and base pair. you know the value of Kb and the molarities are the same, so you can find the Ka value. The K value of water is 1.00 x 10-14 so just divide that by Kb to find Ka. Since the molarities of the two are equal pH=-logKa
T Tony P New member Jun 18, 2009 #3 well you can see that there is a conjugate acid and base pair. you know the value of Kb and the molarities are the same, so you can find the Ka value. The K value of water is 1.00 x 10-14 so just divide that by Kb to find Ka. Since the molarities of the two are equal pH=-logKa
well you can see that there is a conjugate acid and base pair. you know the value of Kb and the molarities are the same, so you can find the Ka value. The K value of water is 1.00 x 10-14 so just divide that by Kb to find Ka. Since the molarities of the two are equal pH=-logKa
