I am having problems with my chemistry lab homework Title De

I am having problems with my chemistry lab homework. Title: Determining the dissociation of a weak acid using pH Measurements

Data:

Molarity of unknown acid1.0 M

NaOH solution: 0.500 M

Volume of Unknown acid, mL: 20.0 mL

Final Buret Reading, mL: (#1) 37.2 mL & (#2) 20.00 mL

Initial Buret Reading, mL: (#1) 18.76 mL & (#2) 0.00 mL

Volume of NaOH solution, mL: (#1) 18.44 mL & (#2) 20.00 mL

Total Volume of solution, mL: .100 mL & .100 mL

pH reading: 4.64 & 4.82

I need to find the following for both numbers #1,#2 from the data sheet : Calculating Ka of unknown acid

Initial number of moles for HAn(aq) & OH- (aq)

Number of moles at equilibrium: HAn(aq) & An-

Equilibrium concentration, mol L^-: HAn, An- & H3O^+

Ka ?

Slope of the line ?

Ka Determined slope

Please help

Plz show work so I can understand it

Solution

Determination of the First Dissociation Constant of Weak Acids SCHA-266 Experiment 1 Apparatus: pH meter with electrode sodium hydroxide solution, about 0.1 M (standardized) unknown solution of a weak acid (100mL of approx. solution) 25-mL pipet buret, buret clamp, and ring stand 150-mL beaker 250-mL beakers (3) standard buffer solutions, pH 4, 7 and 10 General Theory According to the Br