stands for negative logarithm of concentration of hydrogen ion. The value increases with the decreasing concentration of hydrogen ion or with an increasing concentration of hydroxide ion.
Arrhenius Acid-Base Theory:
Acid:
It is a chemical substance which donates protons (hydrogen ion, ) when dissolved in water.
For example,
Base:
It is a chemical substance which donates hydroxyl ion, when dissolved in water.
For example,
Concentration:
Molar concentration of a solution is defined as the number of moles of solute dissolved in one liter of solution. It is expressed as mol/L or M.
Dissociation constant of water: (ion product constant)
Ans:
The pH of a 4.01 mg/L solution is 9.67.
Assuming complete dissociation, what is the pH of a 4.01 mg/L Ba(OH)2 solution?
Assuming complete dissociation, what is the pH of a 4.60 mg/L Ba(OH)2 solution?
Assuming complete dissociation, what is the pH of a 3.06 mg/L Ba(OH)2 solution?
Assuming complete dissociation, what is the pH of a 4.47 mg/L4.47 mg/L Ba(OH)2Ba(OH)2 solution? pH=
Assuming complete dissociation, what is the pH of a 3.77 mg/L Ba(OH), solution? pH =
Assuming complete dissociation, what is the pH of a 4.29 mg/L Ba(OH)_2 solution? pH =
What are the concentrations of OH− and H+ in a 0.00082 M solution of Ba(OH)2 at 25 °C? Assume complete dissociation. [OH−]= [H+]=
What is the pH of a 8.6 x 10-8 M solution of HCl(aq) at 25 °C? Report your answer to the hundredths place. pH = Assuming complete dissociation, what is the pH of a 3.98 mg/L Ba(OH), solution? pH = X10 Assuming equal concentrations, arrange these solutions by pH. Highest pH Lowest pH Answer Bank HCIO, (aq) Cabr,(aq) NaCN(aq) CH, NH, Br(aq) RbOH(aq)
Find the pH of a solution prepared from 1.0 L of a 0.05M solution of Ba(OH)2 and excess Zn(OH)2(s). The Ksp of Zn(OH)2 is 3
What are the concentrations of OH– and H in a 0.00086 M solution of Ba(OH)2 at 25 °C? Assume complete dissociation. [OH-]= [H+]=
What are the concentrations of OH− and H+ in a 0.00082 M solution of Ba(OH)2 at 25 °C? Assume complete dissociation.