3. Calculate the pH of a 0.012 M acetic acid aqueous solution (pKa = 5.46). Report the pH to the hundredths place

Calculate the pH of a 0.0200M solution of ibuprofen (isobutylphenylpropionic acid, C,2H17COOH) solution at 25 °C given that it's conjugate base, isobutylphenylpropionate, has a Kp = 2.7 x 10-10 %3D 2.565 11.268 O6.130 O5.634 O 3.065

Calculate the pH for a 0.5 M nitrous acid (HNO2 ) aqueous solution. Ka= 7.1x10-4 I got 12.27. Just looking to see if I am correct or if I went one step to far.

Calculate the pH at 25 °C of a 0.20M solution of pyridinium chloride (C,H,NHC1). Note that pyridine (CHN) is a weak base with a pK, of 8.77. Round your answer to 1 decimal place. pH = ☐ G

At a particular temperature, the Ka of benzoic acid (C6H5COOH) is equal to 7.1 x 10-5. What is the pH of a solution prepared by combining 0.479 mol of a the acid with 0.143 mol of C6H5COONa (the sodium salt of the acid) in 4.0 L of water? Report your answer to the hundredths place and do not include units. Report your answer to the hundredths place and do not include units.

For a certain acid pK, = 7.13. Calculate the pH at which an aqueous solution of this acid would be 0.093% dissociated. Round your answer to 2 decimal places. pH=0 ?圖。民 2 F B

Calculate the pH of a 0.424 M aqueous solution of hydrocyanic acid (HCN, Ka = 4.0×10-10).

The pH of a 0.66 M solution of 4-chlorobutanoic acid (HC,H¸0,Cl) is measured to be 2.35. Calculate the acid dissociation constant K, of 4-chlorobutanoic acid. Round your answer to 2 significant digits. a K - O a x10

Include:  Balanced chemical equation for the base dissociation equilibrium.  Write the mathematical expression for Kb in terms of concentrations of substances involved in the equilibrium. Set up an ICE table below the balanced chemical equation.

A 0.035 M solution of a weak acid has a pH of 2.21. Calculate the acid ionization constant (Ka) of the acid.Express your answer to 2 significant figures.