The pH of the final solution is 9.25.
In chemistry the pH scale is used to define the acidity or basicity of an aqueous solution. Historically, pH stood for "potential of hydrogen." The pH values of acidic solutions are typically lower than those of basic or alkaline solutions.
Moles = Molarity * Volume(L)
n(NH3) = 1.5 * 0.5 = 0.75 mol
n(HCl) = 0.5 * 0.5 = 0.25 mol
HCl will react with NH3 to form Nh4Cl which is conjugate acid of NH3, so, they will form buffer solution.
HCl + NH3 --> NH4Cl
n(HCl) = n(NH4Cl)
remaining NH3 = 0.75 - 0.25 = 0.50 mol
Whenever the moles of weak base and its conjugate acid is same in buffer, the pOH is equal to its pkb.
pkb = -log(Kb) = - log (1.8 * 10∧ -5) = 4.745
pkb = pOH = 4.745
pH = 14 - 4.745 = 9.25
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