Predict whether or not a precipitate will form upon mixing 175.0 ml of a 0.0055 mkcl solution with 145.0 ml of a 0.0015 m agno3 solution. identify the precipitate, if any. express your answer as a chemical formula. enter noreaction if no precipitate is formed.

"" precipitate will form. A further explanation is below.

According to the question,

We can say the,

AgCl is a precipitate.

Ksp of AgCl,

then,

→

By substituting the values, we get

→        

→        

Thus the above answer is appropriate.

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AgCl

Step-by-step explanation:

The equation for a possible reaction is

KCl(aq) + AgNO₃(aq) ⟶ KNO₃ + AgCl

The possible precipitate is silver chloride.

Moles KCl = 0.1750 × 0.0055/1

Moles KCl = 9.62 × 10⁻⁴ mol

Moles AgNO₃ = 0.1450 × 0.0015

Moles AgNO₃ = 2.18 × 10⁻⁴  mol

Total volume = 175.0 + 145.0

Total volume = 320.0 mL

[KCl] = 9.62 × 10⁻⁴/0.3200

[KCl] = 3.01 × 10⁻³ mol·L⁻¹

[AgNO₃] = 2.18 × 10⁻⁴/0.3200

[AgNO₃] = 6.80 × 10⁻⁴ mol·L⁻¹

The equation for the equilibrium is

                AgCl ⇌        Ag⁺       +      Cl⁻

I/mol·L⁻¹:                  6.80 × 10⁻⁴   3.01 × 10⁻³

Q_sp = [Ag⁺][Cl⁻]

Q_sp = 6.80 × 10⁻⁴ × 3.01 × 10⁻³

Q_sp = 2.04 × 10⁻⁶

K_sp = 1.8 × 10⁻¹⁰

Q_sp > K_sp, so a precipitate will form.

explanation:

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