After dissolving HCI in water, the final concentration of H3O* is 3.87x10-1. What is the pH of this solution? Give your answer to the 2nd decimal.

Chloroacetic acid, HC,H, C10,, has a greater acid strength than acetic acid because the electronegative chlorine atom pulls electrons away from the O-H bond and thus weakens it. Calculate the hydronium ion concentration and the pH of a 3.00 x 10-8 M solution of chloroacetic acid. K, is 1.3 x 10-. [HsO*]=| M pH =

1 being the lowest and 4 being the highest

Consider the following data on some weak acids and weak bases: name hydrocyanic acid acid nitrous acid 0.1 M NH4CI solution 0.1 M KBr 0.1 M CH3NH3Br 0.1 M KNO2 formula HCN Ka 4.9 × 10 HNO₂ 4.5 x 10 X - 10 -4 pH Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, '2' next to the solution that will have the next lowest pH, and so on. choose one 1 (lowest) choose one choose one name Ś base ammonia formula NH₂ Kb 1.8 × 10 -5 -4 methylamine CH3NH₂| 4.4 × 10

The K, of propanoic acid (C,H,COOH) is 1.34 × 10–5. Calculate the pH of the solution and the concentrations of C,H,COOH and C,H,CO0- in a 0.467 M propanoic acid solution at equilibrium. pH = [C,H,COOH] M [C,H,CO0] = M

A typical aspirin tablet contains 325 mg acetylsalicylic acid. Calculate the pH of a solution that is prepared by dissolving 2 aspirin tablets in enough water to make a 269 mL solution. Assume the aspirin tablets are pure acetylsalicylic acid, K₂ = 3.3 x 10-4. Acetylsalicylic acid has a molar mass of 180 g/mol. pH = Submit Question

A weak base has K, = 2.2 × 10-11. What is the value of K, for the conjugate acid? K.

What mass (in g) of potassium fluoride should be added to 0.50 Lof 0.255-M HF(aq) at 25 °C to give a solution with a pH of 3.85 given that the Ką of HF is 7.1x10-4? Molar mass of KF = 58.1 g/mol. Express your answer in decimal notation rounded to three significant figures.

Muscles produce lactic acid, CH₂CH(OH)COOH(aq), during exercise. Calculate the percent ionization (deprotonation), pH, and pOH of a 0.1120 M solution of lactic acid. The acid-dissociation (or ionization) constant, K₁, of this acid is 8.40 × 10-4. percent ionization = pH = pOH = %

Determine the pH of a solution that is 0.00482 M HCl0.00482 M HCl and 0.0304 M HClO2. The Ka of HClO2 is 1.1×10^−2.