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ruddymorales1123
27.06.2019 •
Chemistry
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.
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Ответ:
"
" precipitate will form. A further explanation is below.
According to the question,
We can say the,
AgCl is a precipitate.
Ksp of AgCl,
then,
→![Qsp = [Ag^+][Cl^-]](/tpl/images/0022/4288/07ba1.png)
By substituting the values, we get
→![= 0.0015\times 0.0055](/tpl/images/0022/4288/1f244.png)
→![= 8.25\times 10^{-6}](/tpl/images/0022/4288/4a5f8.png)
Thus the above answer is appropriate.
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Ответ:
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.
Ответ: