Answer :
The ph of the solution after the addition of 100. 0 ml of HNO3 is 5.6. In a 100. 0 ml sample of 0. 10 m NH3 is titrated with 0. 10 m HNO3.
Define anion and cation.
Ions with a positive charge are called cations. Ions with negative charge are called anions. Ionic molecules or atoms are charged. A balanced atom will become a positively charged cation if it loses one or more electrons. An anion is a negatively charged atom that develops when a balanced atom acquires one or more electrons.
Reaction: HNO₃(aq) + NH₃(aq) → NH₄NO₃(aq) +H₂O(l)
NH₄⁺ (aq) + NO₃⁻(aq)
NH₄⁺(aq) + H₂O (aq) ⇆ H₃O⁺(aq) + NH₃(aq)
Mol NH₃ = 0.10 mol/L × 100 mL × 1 L/1000 mL = 0.01 mol
Mol HNO₃ = 0.10 mol/L × 100 mL × 1 L/1000mL = 0.01 mol
Mol NH₄NO₃ produced = 0.01 mol NH₄NO₃
Mol HNO₃ left = 0.01 - 0.01 = 0 mol
Hydrolyzing NH₄⁺ and applying ICE approach
NH₄⁺ --> H⁺ + NO₃⁻
I 0.01 0 0
C -x +x +x
E 0.01-x x x
Kh = Kw/Kb = [H⁺][NO₃⁻]/[NH₄⁺]
10⁻¹⁴/1.8×10⁻⁵ = [x][x]/[0.01-x]
Solving for x,
x = [H⁺] = 2.357×10⁻⁶ mol
The formula for pH is
pH = -log [H⁺]
Aside from 2.357×10⁻⁶ mol, let's add the H⁺ from the remaining HNO₃ which is 0.
Therefore,
pH = -log[2.357×10⁻⁶ mol + 0 mol]
pH = 5.6
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