What change in pH should be observed if 10.0 mL of 0.100 M NaOH is added to 100 mL of a buffer that is 0.100 M in CH3COOH and 0.100 M in NaCH3CO2? Ka for acetic acid is 1.8 x 10-5.
Step -1
Apply Handerson's equation to find out pH value of buffer Solution
pH = pKa + log { [ salt ] / [ Acid ] }
= - log Ka + log { [ Salt ] / [ Acid ] }
= - (1.8 x 10-5 ) + log { ( 0.1 ) / ( 0.1 ) }
= - ( -4.7447 )
= 4.7447
Hence [ H+ ] = antilog of ( - 4.7447 )
= 5.55 x 10-5
Now when 10.0 ml of NaOH is added to 100ml of buffer solution , it will increase the [ OH- ] and decrease
[ H+ ] by equivalent concentration. , so Find out the concentration of OH- in100ml of buffer solution using
relation N 1 V 1 = N 2 V 2
N 1 x 100 = 0.100 x 10.0
N 1 = 0.01M
Thus the concentratin of hydroxyl ion in buffer solution would increase by 0.01 M , and accordingly the concentration of hydrogen ion would decrease by 0.01M
Therefore new [ H+ ] in buffer solution = ( 5.55 x 10-5 ) - 0.01
= 0.009944M
& changed pH ( apply Handerson's equation again )
pH = pKa + log (0.10 ) / (.009944)
= 4.7447 + 1.0021
= 5.7468
hence, Change in pH = 5.7468 - 4.7447
= 1.0021
What change in pH should be observed if 10.0 mL of 0.100 M NaOH is added...
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