Which solution is more acidic and why? 1M HCl or 2M HCl aqueous solution.
Ka for HCl= 1*10^-3
HCl-> H+ + Cl-
1-x
x x
1*10^-3 = x2/1-x
x2 +1*10^-3x -1*10^-3 =0
x= 0.0311 M
1M HCl -> pH =-log[H+] = -log0.0311 =1.507
HCl-> H+ + Cl-
2-x
x x
1*10^-3 = x2/2-x
x2 +1*10^-3x -2*10^-3 =0
x= 0.0442 M
2M HCl -> pH =-log[H+] = -log0.0442 =1.354
hence, more acidic will be 2M HCl as it has lower pH than 1M HCl and lower the pH more acidic the solution
Which solution is more acidic and why? 1M HCl or 2M HCl aqueous solution.
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