Indicate whether aqueous solutions of each of the following solutes contain only ions, only molecules, or mostly molecules and a few ions: NH4ClNH4Cl, a strong electrolyte                                CH3CH3OHCH3CH3OH, a nonelectrolyte                          HCNHCN, hydrocyanic acid, a weak electrolyte

Excluding H₂O, list all the species present in an aqueous solution of potassium fluoride (KF), and also give the correct comparison of [H3O*] to [OH-]. KF, [H3O+] = [OH-] K+, F˜, [H3O+] = [OH"] KF, K+, F¯, [H3O*] = [OH*] › K+, F¯, HF, [H3O*] > [OH-] OK+, F, HF, [H3O+] < [OH-]

Consider an aqueous solution of NaC2H3O2.  Which of the following statements is true? A)C2H3O2- is a weak base and NaC2H3O2 is a weak electrolyte. B)C2H3O2- is a strong base and NaC2H3O2 is a weak electrolyte. C)C2H3O2- is a  strong base and NaC2H3O2 is a strong electrolyte. D)C2H3O2- is a weak base and NaC2H3O2 is a strong electrolyte.

Each row of the table below describes an aqueous solution at about 25 °C. Complete the table. That is, fill in any missing entries in the second column. Be sure each entry you write includes the correct number of significant digits. [H₂O¹] solution A B с mol/L mol/L mol/L pH 11.49 0.090 7.92 0 10 X S

Which of the following (assuming the same concentration in water) would make a solution with the lowest hydrogen ion concentration? Group of answer choices H2S (Ka= 8.9×10−8) NH4+ (Ka= 5.6 × 10−10)   NH3 ( Kb= 1.8 × 10−5) HC2H3O2 (Ka= 1.8×10−5) HCl

f the pOH of a solution is 10.59, what is the H3O+ concentration in the solution?   Write the answer in scientific notation with 2 sig.dig.  For example if your answer is 3.49x10^3, write down 3.49e+3. The +/- signs are important!  Also, make sure there are no spaces between values, otherwise the answer will be considered incorrect!

Please don't provide handwriting solution

Each row of the table below describes an aqueous solution at about 25°C . Complete the table. That is, fill in any missing entries in the second and third columns. Be sure each entry you write includes the correct number of significant digits. solution H3O+ pH A 2.1x10-8 mol/L   B              mol/L  9.89 C 0.0030  mol/L

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

What type of compound cannot be dissolved in water? coordinate ionic O polar O nonpolar