Calculate the pH when 1.35 g of C6H5COONa (FW = 144.1 g/mol) is added to 38 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.

Aspirin was discovered as a result of efforts to produce a derivative of salicylic acid that would not be irritating to the stomach lining. Aspirin is acetylsalicylic acid, CH3CO2C6H4CO2H The −CO2H functional group is still present but it’s acidity isreduced to Ka = 3.0 × 10^-4. What is the pH of a solution of acetylsalicylic acid with the concentration of 2.502?

A solution is prepared that is initially 0.45M in pyridine (CÂHÂN), a weak base, and 0.50M in pyridinium bromide (C5H₁NHBr). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in [où¯]. You can leave out the symbol for molarity. initial change final [C,H,N] [C₂H₂NH*] [OH-] 0 0 0 0 DO X Ar

A chemist titrates 220.0 mL of a 0.6204 M butanoic acid (HC₂H,CO₂) solution with 0.2746 M KOH solution at 25 °C. Calculate the pH at equivalence. The PK of butanoic acid is 4.82. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of KOH solution added. pH = 0 X Ś

HA is a weak acid. We mix 3.000 L of a 0.555 M solution of HA with1.000 L of a 0.444 M solution of NaOH. The pH of the solution produced (with atotal volume of 4.000 L) is 3.55. What is the value of the dissociation constant, Ka,for this weak acid HA? The temperature is 25.0◦C.

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).

Can you help me answer the PH=

Calculate the pH when 1.03 g of NaClO (FW = 74.44 g/mol) is added to 44.4 mL of 0.50 M HClO. Ignore any changes in volume. The Ka value for HClO is 3.0 x 10-8.

Calculate the pH of the solution that results when 15.0 mL of 0.1600 M lactic acid (Ka(CH3 CHOHCOOH) = 1.38 × 10 : 10-4) is a. diluted to 55.0 mL with distilled water. pH = b. mixed with 40.0 mL of 0.0600 M NaOH solution. pH = c. mixed with 40.0 mL of 0.120 M NaOH solution. pH = d. mixed with 40.0 mL of 0.120 M sodium lactate solution. pH =

An analytical chemist is titrating 243.8 mL of a 0.7000 M solution of butanoic acid (HC3H,CO2) with a 0.3800 M solution of NaOH. The pK of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 278.5 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. PH ☐ olo Ar