(a)  Calculate the pH of a 0.20 M solution of benzoic acid at 25°C.(b)  How many moles of acetic acid must be dissolved per liter of water to            obtain the same pH as that from part (a)?

The acid dissociation constant K of trimethylacetic acid (HC(CH³)CO₂) is 9.33 × 10¯. Calculate the pH of a 1.2M solution of trimethylacetic acid. Round your answer to 1 decimal place. pH = 0

Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.62 M in this salt. The desired pH of the buffer should be equal to 4.5. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula Ammonia Methylamine Ethylamine Aniline NH3 CH;NH2 CH;NH2 CH;NH, C;H;N NH,+ CH;NH;* CH$NH;* CH;NH;* C;H;NH* 1.8 × 10-5 4.38 x 10-4 5.6 x 10-4 3.8 x 10-10 1.7 x 10-9 Pyridine 3. Compute the concentration of the weak base in Molarity. (Write your answer in 3 decimal places without the unit).

A 0.119 M solution of Covidenol, a weak acid, has a measured pH of 3.45.  Determine the pKa of Covidenol.

Draw the structures of the conjugate bases of the following acids:

Calculate the pH at 25°C of a 0.91 M solution of anilinium chloride (C6H5NH3Cl). Note that aniline (C6H5NH2) is a weak base with a pKb of 4.87.