Calculations with Equilibrium Constants. I\'m having trouble with how these work

Question

Calculations with Equilibrium Constants. I'm having trouble with how these work. Please explain.

Calculations with Equilibrium Constants Calculating the Equilibrium Constant K from the Inital Concentration and Measured pH sn Reid base reactien cart be determined from the initial concentration of the acad or tase n solution and trom the measured pH of the A 0.056 Maqueous solution of butanoic add. CHrcooH, hak a pH at 272 at 25C, What is the vaue Ka for butanoic acid? Calculating Equilibrium concentrations and pH from Ka Problem 2: What are the equlbrium Doncentrations of acutie acid, ita conjugate base acetate ion, sed Hao" for a 0.10 M soution of acetic acid (K. 1.Bx 10 What is the pH of the solution Calculating the pH of a Solution of a Conjugate Base of a Problem 3: sodium hypochlorite, Nacio. is vsed ss a disimlectsrt pools and water treatment plants. What are the concentrations of HCIO and OH Ion and the pHof a 0.015 M soluton of NaCO at 25 C (K of CIO 2.3 x 10 T) Calculating the pH After the Reaction of a weak Base with an Acid Problem 4: What is the pH cf the solution that resubs trom mixing 25 m NHa and 25 ml of 0 01e MHCl

Explanation / Answer

Q1.

M = 0.056 M of a Benzoic Acid

formula --> C7H5OOH

in equilibirum:

C7H5OOH(aq) <-> C7H5OO-(aq) + H+(aq)

Ka = [C7H5OO-][H+]/[C7H5OOH]

if we know pH, then

[H+] = 10^-pH = 10^-2.72 = 0.001905

so..

benzoate ion = h+ = 0.001905 M

then, in equilibrium

Benzoic acid = 0.056 - 0.001905 = 0.054095 (Account for dissociated acid)

therefore

Ka = (0.001905 )(0.001905) / (0.054095)

Ka = 6.7086*10^-5

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