What is the ratio of acetate ion to acetic acid (Ka = 1.76×10–5) in a solution containing these compounds at pH 3.52 ? Write your answer as a decimal and not as a fraction.

The Kb of carbonate is 1.8×10−4. Calculate the Ka of its conjugate acid.

The pH of a 0.54 M solution of 4-chlorobutanoic acid (HC,H,0,Cl) is measured to be 2.40. Calculate the acid dissociation constant K, of 4-chlorobutanoic acid. Be sure your answer has the correct number of significant digits. a K = |

The pH of a 0.78M solution of benzoic acid (HCH,CO₂) is measured to be 2.15. Calculate the acid dissociation constant K of benzoic acid. Be sure your answer has the correct number of significant digits. K-0 x G

How many moles of NaOH did it take to reach the equivalence point ? what is shown in the pictures is all I was given.

A solution was prepared at 25°C in which the ratio of methylamine (CH3NH2) to the salt methylammonium chloride (CH3NH3Cl) was two to one, and resulted in a pH = 11.00. Calculate Ka for the weak acid methylammonium (CH3NH3+) at 25°C.

Common aspirin is acetylsalicylic acid, which has the structure shown below and a pKa of 3.5. Calculate the pH of a solution in which one normal adult dose of aspirin ( 5.7×102mg ) is dissolved in 0.33 L of water. Express your answer to one decimal place.Common aspirin is acetylsalicylic acid, which has the structure shown below and a pKa of 3.5. Calculate the pH of a solution in which one normal adult dose of aspirin ( 5.7×102mg ) is dissolved in 0.33 L of water. Express your answer to one decimal place.

1. For equal concentrations of acids such as hydrofluoric acid, acetic acid, and benzoic acid, does the pH increase, decrease, or remain the same as the Ka value increases? Justify your answer.

What is the relationship between the value of pKa and the strength of a weak acid?

The acid-dissociation constant, Ka, for maleic acid, H2CAH4O5 , is 7.56x10-7. What is the base-dissociation constant, Kp for the maleate ion? Write your answer to 3 significant figures