For each solute, click the button under the better solvent. solute :0: || NH,−C. NH Br NH₂ HO · CH₂ CH₂-OH Which is the better solvent? H H H₂O :0: || CH₂-S- CH3 H CH3 CH₂CH₂OH :0: CH3 CH3-C - CH CH₂CH₂OH H H - CH3

The [OH-] of an aqueous solution is 3.5x10 -5. What is the [H+]

Calculate Ph

Each row of the table below describes an agueous solution at about 25 °C. [H,0 ]to Complete the table. That is, fill in any missing entries in the second and third columns. Round your entries for to 2 significant digits, and your entries for pH to 2 decimal places. [x,0] solution pH 5.6 x 10 -9 mol/L A O mol/L 7.15 B 0.049 mol/L

Calculate the pHpH of each solution. 1. [OH−]  = 9.9×10−7  M 2.[OH−] = 8.6×10−8 M 3.[OH−]  = 3.2×10−11  M 4.

3

Calculate either [H3O+] or [OH−] for each of the solutions at 25 °C. Solution A: [OH−]=2.73×10−7 M; [H3O+]= Solution B: [H3O+]=8.31×10−9 M; [OH−]= M Solution C: [H3O+]=6.79×10−4 M; [OH−]= M Which of these solutions are basic at 25 °C? Solution B: [H3O+]=8.31×10−9 M Solution C: [H3O+]=6.79×10−4 M Solution A: [OH−]=2.73×10−7 M

Choose the correct answer from among the alternatives; To make the sentence true: hydrocyanic acid HCN, the ionization constant Kaq = A) [Ka = [H3O +] / [H2O] [HCN B) [Ka = [H3O +] [CN-] / [HCN C)[Ka = [CN-] / [H2O] [HCN D) [Ka = [CN-] / [H2O

[OH-] = 5.6 × 10-4 M?

Circle the ions that would undergo hydrolysis when added to water