When comparing 1.0M solutions of bases, the base with the lowest [OH-] is the
A.) |
weakest base and it has the largest Kb value. |
B.) |
strongest base and it has the largest Kb value. |
C.) |
weakest base and it has the smallest Kb value. |
D.) |
strongest base and it has the smallest Kb value. |
When comparing 1.0M solutions of bases, the base with the lowest [OH-] is the A.) weakest...
List the following organic bases from strongest to weakest base. List the following organic bases from strongest to weakest base. A. B. H odio - 1. (Strongest) 2. - 3. . 5. . 6.(weakest)
List the following bases in order of strength, strongest to weakest. Pb(OH)2, Kb=9.6x10-4 H2NOH, Kb=1.2x10-8 NH4OH, Kb=1.8x10-3 NH3, Kb=1.8x10-5 CH3NH2, Kb=4.2x10-4
Exercise 1: Consider the following information for a series of solutions of weak acids, HA: Weak acid PK, К. If [HA], is... then [H3O+]E ... and pH HCOOH 3.74 1.8 x 10-4 0.100 M 4.2 x 10² M 2.38 HNO2 3.37 4.2 x 10-4 0.100 M 6.3 x 10-M 2.20 HCN 9.20 6.3 x 10-10 0.100 M 7.9 x 10ⓇM 5.10 4.23 0.100 M 5.9 10-M HOCI 7.46 3.5 x 10-8 0.200 M 8.3 x 10M 4.07 0.400 M 1.2...
Arrange the following three bases in order of increasing base strength. NH CH3OH ОСН; II I III a. (Weakest base) I < II < III (Strongest base) b. (Weakest base) I < III < II (Strongest base) c. (Weakest base) II < I < III (Strongest base) d. (Weakest base) II < III < I (Strongest base) e. (Weakest base) III < II <I (Strongest base) f. (Weakest base) III < I< II (Strongest base)
Solutions of each of the hypothetical bases in the following table are prepared with an initial concentration of 0.100 M. Which of the four solutions will have the lowest pH and be least basic? Base Kb A 1.8 x 10-3 B 2.3 x 10-1 C 4.6 x 10-4 D 5.3 x 10-6 All will have the same pH because the concentrations are the same.
HCN(aq) + SO *(aq) + Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.) Acid Base Strongest HC104 acids H2SO4 C104- HSO4- Weakest bases HI I HBr Br HCI Ci HNO3 NO3- H30+ H2O HSO4 SO42- H2SO3 HSO3- H3PO4 H2PO4- HNO2 NO2 HF F HC2H302 C2H2O2- Al(H20)63+ Al(H20); OH H2CO3 HCO3 HAS HS HCIO C10- HBrO Br0 NH4+ NH HCN CN HCN CN...
CHE 172 Acid-Base Equilibrium Worksheet 1. Identify the conjugate pairs in the following reaction: HC2H302(aq) + H2O + H20*24) + CH3O2 (aq) 2. Based on the Kb of the following weak bases, which is the strongest base? C6H5NH2 HONH2 H2NNH2 C2H5NH2 Kb = 4.3x10-10 Ko = 1.1x10-8 Kb = 1.3x106 Kb = 6.4x104 Which has the strongest conjugate acid? 3. Calculate the pH of the following solutions: a. 0.25M HBO b. 0.25M Ba(OH)2 C. 0.25M HCN (K. = 5.00x10-10) d....
1 ) Using the data in the table below, which conjugate acid is the weakest acid, given that all solutions (aq., 25 °C) are 0.200 M? Explain your choice! Base Kb CIO 3.3 x 10-7 CO3-2 1.8 x 10-4 HS- 1.8 x 10-7 NH2CH3 4.4 x 10-4 1b) Which of the following aqueous solutions has the lowest [OH-] (aq., 25 °C)? A) a solution with a pH of 3.0 B) a 1 x 10-4 M solution of HNO3 C) a...
3) Bases accept protons or hydronium ions in aqueous solutions. The equilibrium constant Kb describes the following reaction for a weak base, B, in aqueous solution: B +H20 В +н вн* BH* +OH с. a. BH +H20 B+H30* BH +02 d. B+OH b.
Acid H SO H.O2 HF HCIO CH OH Conjugate Base HSO HO F CIO C H 0 Ka 1.5x10-2 2.4x10-12 3.5x10-4 3.0x10 1.3x10-10 3. For the given table above, list the bases from weakest to strongest. (8pts) Show sample work.