What is the pH of a 0.33 M solution of hydroxylammonium bromide (NH3OHBr)? Kb for hydroxylamine (NH2OH) is 6.6 × 10^-9
1. 2.911
2. 3.001
3. 3.281
4. 3.391
5. 18.33
6. 3.151
7. 9.669
8. 4.331
I got 9.669 but its not right.
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
What is the pH of a 0.33 M solution of hydroxylammonium bromide (NH3OHBr)? Kb for hydroxylamine...
BIU*. ** Efx as I What is the pH of a 0.12 M solution of hydroxylammonium bromide (NH3OHBr)? Kb for hydroxylamine (NH2OH) is 6.6 x 10-9. 1. 18.55 2.3.500 3.3.130 4.9.449 5.3370 6.3.610 7.3.220 8.4.551
hydroxylamine is a weak base with kb=7.96. determine the pH of 0.742 M hydroxylamine solution (to 2 decimals)
What is the pH of an aqueous 0.083 M hydroxylamine, HONH2, solution? Hydroxylamine is a basic substance when dissolved in water. Kb(HONH2)=1.1e-8.
Which 0.1 M solution of compounds below has the highest [H30*): formula Kb Name Hydroxylamine NH2OH 9.1x10-9 Isoquinoline C9H7N 2.5x10-9 Caffeine C8H10N402 4.1x10-4 Diethylamine (C2H5)2NH 6.9x10-4 Dimethylamine (CH3)2NH 5.9x10-4 O Diethylamine Hydroxylamine Isoquinoline Caffeine Dimethylamine
What is the pH of the solution from adding 25 mL of 0.33 M HCl to 25 mL of 0.58 M NH3? (Kb for NH3 is 1.8 x 10^-5)
3. A solution is prepared by treating 50 mL of 0.50 M HF (Ka = 6.6x10 ) with 10 mL of 1.15 M NaOH. Calculate the pH of the solution. 4. If enough NaOH is added to the solution in problem 3 to neutralize the HF, what will the pH be? 5. 42.16 mL of a solution of NaOH are required to neutralize 0.7878 g of potassium hydrogen phthalate (Mwt = 204.23 g/mol). Calculate the molar concentration of NaOH in...
Hey! Can you please help me with the following two questions I am highly confused and I don't really understand them at all. Thank you!! 16, Please help me with them, we have a test this thursday and problems that are similar are supposed to be on there. Thank you so much!!! 1.Calculate the pH of a 0.119 M aqueous solution of hydroxylamine (NH2OH, Kb = 9.1×10-9) and the equilibrium concentrations of the weak base and its conjugate acid. pH...
The Kb of hydroxylamine, NH2 OH, is 1.10 × 10^{-8}. A buffer solution is prepared by mixing 100 mL of a 0.37 M hydroxylamine solution with 60 mL of a 0.25 M HCl solution.Part AFind the pH of the resulting solution.
What is the pH of a .62 M [C5H5NH]NO3 solution? Kb(C5H5N) = 1.7 x 10-9 Kb(NH3) = 1.8 x 10-5
Calculate the pH of a 0.20 M solution of the weak base pyridine. (C5H5N; Kb = 1.7 x 10-9). What is the pH of a 0.20 M solution of NH4Cl? [Kb(NH3) = 1.8 ´ 10–5]