H4CI) falls within what range? O O to 2 O 2 to 7 O 7 to 12 O 12 to 14

Estimate the pH that results when the following two solutions are mixed. a) 50 mL of 0.3 M CH3COOH and 50 mL of 0.4 M KOH b) 100 mL of 0.3 M CH3COOH and 50 mL of 0.4 M NaOH c) 150 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2 d) 200 mL of 0.3 M CH3COOH and 100 mL of 0.3 M Ba(OH)2

Which of the diagrams in Problem 10-135 represents the substance that is the weakest electrolyte?

What is the freezing point of vinegar, which is an aqueous solution of 5.00% acetic acid, HC2H3O2, by mass (d=1.006g/cm3)?

Composition diagrams, commonly known as alpha plots, are often used to visualize the species in a solution of an acid or base as the pH is varied. The diagram for 0.100 M acetic acid is shown here. The plot shows how the fraction [alpha ()] of acetic acid in solution, =[CH3CO2H][CH3CO2H]+[CH3CO2] changes as the pH increases (blue curve). (The red curve shows how the fraction of acetate ion, CH3CO2, changes as the pH increases.) Alpha plots are another way of viewing the relative concentrations of acetic acid and acetate ion as a strong base is added to a solution of acetic acid in the course of a titration. (a) Explain why the fraction of acetic acid declines and that of acetate ion increases as the pH increases. (b) Which species predominates at a pH of 4, acetic acid or acetate ion? What is the situation at a pH of 6? (c) Consider the point where the two lines cross. The fraction of acetic acid in the solution is 0.5, and so is that of acetate ion. That is, the solution is half acid and half conjugate base; their concentrations are equal. At this point, the graph shows the pH is 4.74. Explain why the pH at this point is 4 74.

What is the pOH for a solution at 25 °C that has a H3O+ concentration of 6.57 ×10-6 M?    A 34.1 % (NH4 )2SO4   (molar mass = 132.1 g mol−1) has a density of 1.15 g mL−1. What is the molarity of this solution?  (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3)     Determine the boiling point of a solution that contains 78.5 g of compound W (molar mass = 132.5 g mol–1) dissolved in 1088.6 g benzene (C6H6; molar mass = 84.156 g mol–1; Kb = 2.53 °C m–1; boiling point of pure benzene = 80.1 °C). (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3)   NEED HELP ASAP NO WORK NEEDED

5A

What is the concentration of hydroxide ion in a 0.54 M aqueous solution of hydroxylamine, NH2OH? (Assume the value of Kw is 1.0  10-14.)

The pH of dissolving 1.48 g of propanoic acid (CH3CH2COOH, Ka 1.3X105) in 200 mL H20 is 4.82 O3.71 O 2.94 O 1.22 O 5.25

chloride A solution is prepared at 25 °C that is initially 0.69M in dimethylamine ((CH3)2NH), a weak base with K = 5.4 × 10-4, and 2.4M in dimethylammonium ((CH3)2NH₂CI). Calculate the pH of the solution. Round your answer to 2 decimal places. pH =