To prepare 1-L buffer solution with pH = 5.05, how many moles of C6H5COONa (sodium benzoate) should be mixed with 0.86 mol C6H5COOH (benzoic acid) into a 1-L solution? Ka (C6H5COOH) = 6.3*10^-5. Your answer should have 2 significant figures.

What is the pH of a balsamic vinegar having an acetic acid (M.W. = 60.05g/mol; Ka = 1.8 x 10^-5) content of 5% (w/v)? w/v = weight of acetic acid/volume of vinegar.

Trimethylamine, (CH3)3N, is a gas with a fishy, ammonia–like odor. An aqueous solution that is 0.41 M trimethylamine has a pH of 11.71. What is Kb for trimethylamine? (Assume the value of Kw is 1.0  10-14.)

Calculate the pH when 1.77 g of C6H5COONa (FW = 144.1 g/mol) is added to 48 mL of 0.50 M benzoic acid, C6H5COOH (FW = 122.1 g/mol). Ignore any changes in volume.  The Ka value for C6H5COOH is 6.5 x 10^-5.

Calculate the pH of 0.606 M anilinium hydrochloride (C6H5NH3Cl) solution in water, given that Kb for aniline is 3.83 × 10-4. Show the ionization equation of the salt; the hydrolysis equation of the ion; the ICE table and your calculations.

Pls help Calculate the pH of a solution (aq., 25 oC) prepared by dissolving 23.632 g of solid methylammonium chloride (CH3NH3Cl) in 1.00 L of 1.10 M methylamine (CH3NH2). The Kb for methylamine is 4.40 × 10-4. Report to two decimal places. MM CH3NH3Cl = 67.518 g/mol

What is the pH of a solution prepared by adding 60.4 g ethylammonium chloride (C2H5NH3CI, 81.55 g/mol) to 1.00L of a 0.300 M aqueous solution of ethylamine (C2H5NH2, 45.08 g/mol, Kp = 4.3 x 104 at 25°C)? Enter your answer in decimal format with two decimal places (value + 0.02).

Propanoic acid (CH3CH2COOH) has a Ka of 1.3×10–5.FW(propanoic acid) = 74.08 g/mol; FW(calcium propanoate) = 186.22 g/mol a) At what pH will a solution of propanoic acid and sodium propanoate best resist changes to its pH? How do you know? b) 75 g calcium propanoate Ca(CH3CH2COO)2 is diluted to 150.0 mL with deionized water. 50.0 mL of a 3.0 M propanoic acid solution is added. Determine the equilibrium concentrations of each species and the pH of the resulting solution.

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. chloride pH = ☐

A solution is prepared at 25 °C that is initially 0.20M in chloroacetic acid (HCH₂CICO₂), a weak acid with K=1.3 x 10³, and 0.34 M in sodium chloroacetate (NaCH₂CICO₂). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = 0 Explanation 81°F Mostly sunny 3 F9 Check $ 4 X с с FS % 5 S 2 1 F6 6 Q Search. F7 & 7 LDL F8 * 8 F9 F10 ( 9 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessi F11 ) 0 *+ F12 JE PrtSc + Insert = Delete Backspace 4) J ►/11 Num