For a weak acid
pH = pKa + log c
where c = concentration of acid.
So pH= 3.244+ log 0.122 = 2.33
w Solve the quadratie egn. 2) An Acid HA , 0.122m, Ka= 5.78104 at a certain...
Calculate the equilibrium constant, Ka for the acid, HA if, at equilibrium, the pH of a 1.85 M solution of HA is 3.13? I know that: Use pH = -log [H+] first and solve for [H+]. Then use Ka = [H+][A-]/[HA] to solve for Ka. [A-] = [H+] [HA] is given in the problem. I keep getting it wrong, any ideas??
A certain weak acid HA, has Ka value of 9.8*10^-7 Calculate the percent ionization of HA in a 0.10M Solution
A certain weak acid, HA, with a Ka value of 5.61×10−6, is titrated with NaOH.A.A solution is made by titrating 8.00 mmol (millimoles) of HA and 2.00 mmol of the strong base. What is the resulting pH?Express the pH numerically to two decimal places.B.More strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 43.0 mL?Express the pH numerically to two decimal places.
A certain weak acid, HA , has a Ka value of 2.7×10−7 1.)Calculate the percent ionization of HA in a 0.10 M solution 2.)Calculate the percent ionization of HA in a 0.010 M solution
A certain weak acid, HA, with a Ka value of 5.61×10−6, is titrated with NaOH. A solution is made by titrating 46.19 mmol (millimoles) of HA and 2.24 mmol of the strong base. Then, more strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 85.1 mL ?
A certain weak acid, HA, with a Ka value of 5.61×10−6, is titrated with NaOH. A solution is made by titrating 9.91 mmol (millimoles) of HA and 2.66 mmol of the strong base. Then, more strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 58.2 mL ?
A certain weak acid, HA, has a Ka value of 1.3×10−7. Calculate the percent ionization of HA in a 0.010 M solution.
A certain weak acid, HA, has a Ka value of 5.3×10−7 Calculate the percent ionization of HA in a 0.10 M solution.
Titration of Weak Acid with Strong Base A certain weak acid, HA, with a Ka Value of 5.61 *10^-6, is titrated with NaOH. PART A A solution is made by mixing 8.00 mmol(millimoles) of HA and 1.00 mmol of the strong base. What is the resulting pH? express the pH numerically to two decimal places. pH = ? PART B More strong base is added until the equicalence point is reached. What is the pH of this solution at the...
A certain weak acid, HA, has a Ka value of 9.1×10−7. Part A Calculate the percent dissociation of HA in a 0.10 M solution.