Calculate the pH of the solution made by adding 0.50 mol of HObr in 0.30 mol of KOBr to 1.00 L of water. The value of Ka for HObr is 2.0 * 10^-9
The concept used to solve this problem is based on the chemical equilibrium.
The pH of solution is used to determine acidity and basicity of a solution.
The pH of solution can be determine by Henderson-Hasselbalch equation as follow.
Here is written as follow.
Here, is acid dissociation constant.
The of the solution can be calculated by formula as follow.
Substitute for .
Here, weak acid is and its conjugate base is . In the buffer mixture, is act as conjugate base.
The Henderson-Hasselbalch equation is as follow.
Thus, Substitute 8.7 for , for and for .
Ans:
The pH value of buffer solution is 8.5.
Calculate the pH of the solution made by adding 0.50 mol of HObr in 0.30 mol of KOBr to 1.00 L of water. The value of K...
Please explain the mechanism to me as well. Part A Calculate the pH of the solution made by adding 0.50 mol of HOBr and 0.30 mol of KOBr to 1.00 L of water. The value of Ka for HOBr is 2.0 x 10-9. Express your answer numerically using two decimal places. ► View Available Hint(s) O ADD A O O ? pH = Submit Request Answer
What is the pH of a solution made by adding 0.30 mol of acetic acid (Ka = 1.8 x 10-5) to enough water to make 1.0 L of solution?
Calculate the pH of a solution produced by adding 0.50 L of 1.00 M HCl to 0.50 L of 2.00 M NaClO. Ka(HClO) = 2.9x10-8 Calculate the pH of a solution produced by adding 0.50 L of 1.00 M NaOH to 0.50 L of 2.00 M HClO. Ka(HClO) = 2.9x10-8 It is desired to have a buffer with a pH = 5.000 using acetic acid. If [HAc] + [Ac─ ] = 0.500 M, what is the required [HAc] and [Ac─...
Calculate the pH and % dissociation of a 4.68 M solution of KOBr in water (ka=2.8*10^-9 for HOBr)
Calculate the pH of a solution produced by mixing 0.50 mol of HCN and 0.20 mol of NaOH in a total of 1.00 L of solution. Ka = 4.9 × 10-10 for HCN
2. Calculate the pH, pOH, [H3O+], and [OH-] of a 0.30 M solution of the weak acid, hypobromous acid, HOBr. The Ka value for HOBr is 2.8 x 10-9.
A 1.00 L buffer solution with pH = 4.74 is composed of 0.30 mol acetic acid and 0.30 mol sodium acetate. A) Determine the pKa of acetic acid B) If 0.030 mol of NaOH is added, determine the pH of the solution
A solution is prepared by adding 1.0 mol of lithium nitrate. LINO3 to 1.00 L of water. Which of the following statement about the solution is correct? The solution is neutral. The solution is basic. The solution is strongly acidic. The solution is weakly acidic. The values of Ka and Kb for the species in the solution must be known in order to make a prediction.
A buffer solution is made by adding 20.0 mL of a 0.50 M Na2CO3 solution to 10.0 mL of a 0.50 M NaHCO3 solution in a test tube. The pH of this buffer was found to be 10.20. After 2.0 mL of 1.0 M HCl solution is added to this buffer solution, the pH is measured to be 9.95. What is the buffering capacity with respect to a strong acid, βa, of this buffer solution, in units of mol/L per pH unit?...
Calculate the pH of a solution that is 0.27M in naOBr. Ka (HOBr) = 2.0x10^-9, include a balanced equation for the ion effecting the PH of this solution in water. detailed explaination please.