A monoprotic weak acid has a Ka of 1.44 x 10-4. What would be the pH if 1.03 moles of the acid is dissolved in 1 liter of water?
A monoprotic weak acid has a Ka of 1.44 x 10-4. What would be the pH...
1.) The Ka of a monoprotic weak acid is 7.93 x 10^-3. What is the percent ionization of a 0.170 M solution of this acid? 2.) Enough of a monoprotic acid is dissolved in water to produce a 0.0141 M solution. The pH of the resulting solution is 2.50. Calculate the Ka for the acid.
If the Ka of a monoprotic weak acid is 6.6 x 10-6, what is the pH of a 0.27 M solution of this acid? pH =
If the Ka of a monoprotic weak acid is 2.4 x 10-6, what is the pH of a 0.45 M solution of this acid? pH =
The Ka of a weak monoprotic acid is 1.55 x 10-5. What is the pH of a 0.0813 M solution of this acid? pH
If the Ka of a monoprotic weak acid is 6.4 × 10-6, what is the pH of a 0.39 M solution of this acid?
If the Ka of a monoprotic weak acid is 1.0 × 10-6, what is the pH of a 0.48 M solution of this acid?
If the Ka of a monoprotic weak acid is 4.7 × 10-6, what is the pH of a 0.46 M solution of this acid?
If the Ka of a monoprotic weak acid is 6.6*10^6, what is the pH of a 0.37 M solution of this acid?
If the Ka of a monoprotic weak acid is 3.0 × 10-6, what is the pH of a 0.45 M solution of this acid?
If the Ka of a monoprotic weak acid is 6.8 × 10−6, what is the pH of a 0.11 M solution of this acid?