What is the percent ionization of a monoprotic weak acid solution that is 0.165 M? The acid-dissociation (or ionization) constant, Ka, of this acid is 2.32×10−11

What is the percent ionization of a monoprotic weak acid solution that is 0.138 M? The acid-dissociation (or ionization) constant, Ka, of this acid is 4.92×10^-10.

The hydronium ion concentration in an aqueous solution at 25°C is 3.4×10 M. The hydroxide ion concentration is М. The pH of this solution is The pOH is

The pH of an aqueous solution at 25°C was found to be 7.00. The pOH of this solution is The hydronium ion concentration М. The hydroxide ion concentration is М.

Will 0.10 M aqueous solutions of the following salts be acidic, basic or neutral? (Assume a solution is neutral if its pH is 7.00±0.05). Equilibrium constants may be found in an appendix to your text. ammonium formate (NH4CHO₂) ammonium acetate (NH4C₂H302) sodium hydrogen arsenate (Na₂HASO4) sodium acetate (NaC₂H30₂) ammonium sulfide ((NH4)2S)

A 9.5×10−2 MM solution of a monoprotic acid has a percent dissociation of 0.56%. Determine the acid ionization constant (Ka)(Ka) for the acid. Express your answer using two significant figures.

Chemistry

A monoprotic base has a molar weight of 93 g/mol. The pH of a 100-mL solution containing 3.9 g of this base is 9.5. What is the base ionization constant, K?

A diprotic acid ( H2A ) has ?a1=4.38×10−7 and ?a2=5.81×10−11. What is the pH of a 0.348 M H2A solution?

A solution is prepared at 25 °C that is initially 0.41M in chlorous acid (HCIO,), a weak acid with K–1.1 × 10 , and 0.46M in sodium chlorite (NaCIO,). Calculate the pH of the solution. Round your answer to 2 decimal places. pH =