A solid dissolves in a liquid when it mixes completely with the liquid. ... Things which dissolve are called solutes and the liquid in which they dissolve is called a solvent to form a solution
sodium chloride
and lead (II) acetate
potassium sulfate and strontium iodide
chromium (III) nitrate and sodium phosphate
1.
2NaCl + Pb(CH3COO)2 → 2NaCH3COO + PbCl2
2.
K2SO4 + SrI2 → KI + SrSO4
3.
Cr(NO3)3 + Na3PO4 →CrPO4 + NaNO3
Answer:
Q = 1.08x10⁻¹⁰
Yes, precipitate is formed.
Explanation:
The reaction of CoF₂ with NaOH is:
CoF₂(aq) + 2 NaOH(aq) ⇄ Co(OH)₂(s) + 2 NaF(aq).
The solubility product of the precipitate produced, Co(OH)₂, is:
Co(OH)₂(s) ⇄ Co²⁺(aq) + 2OH⁻(aq)
And Ksp is:
Ksp = 3x10⁻¹⁶= [Co²⁺][OH⁻]²
Molar concentration of both ions is:
[Co²⁺] = 0.018Lₓ (8.43x10⁻⁴mol / L) / (0.018 + 0.022)L = <em>3.79x10⁻⁴M</em>
[OH⁻] = 0.022Lₓ (9.72x10⁻⁴mol / L) / (0.018 + 0.022)L = <em>5.35x10⁻⁴M</em>
Reaction quotient under these concentrations is:
Q = [3.79x10⁻⁴M] [5.35x10⁻⁴M]²
<em>Q = 1.08x10⁻¹⁰</em>
As Q > Ksp, <em>the equilibrium will shift to the left producing Co(OH)₂(s) </em>the precipitate
I hope this will help you
Calcium chloride dehydrate (CaCl₂ · 2 H₂O) have a molar mass equal to 147 g/mol.
Explanation:
To calculate the molar mass of calcium chloride dehydrate (CaCl₂ · 2 H₂O) we use the following formula:
molar mass of CaCl₂ · 2 H₂O = atomic weight of Ca × 1 + atomic weight of Cl × 2 + atomic weight of H × 4 + atomic weight of O × 2
molar mass of CaCl₂ · 2 H₂O = 40 × 1 + 35.5 × 2 + 1 × 4 + 16 × 2
molar mass of CaCl₂ · 2 H₂O = 147 g/mol
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molar mass
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