Answer:
The vinegar is not enough to neutralize the pool.
Explanation:
The [OH⁻] in the pool is 1.0x10⁻¹mol / L. To know how many moles of OH⁻ are in the solution, you must calculate volume of the pool thus:
V(pool) = πr²h
<em>Where r, radius is d/2 = 12m/2 = 6m and h is deep of the pool = 10m
</em>
V(pool) = π(6m)²*10
V(pool) = 1131m³
As 1m³ = 1000L:
1131m³ × (1000L / 1m³) = 1131000L in the pool.
And moles of OH⁻ are:
1.0x10⁻¹mol / L ₓ 1131000L = 131100 moles of OH⁻ are in the pool
The neutralization of OH⁻ with H⁺ is:
OH⁻ + H⁺ → H₂O
<em>That means to neutralize the pool you must add 131100 moles of H⁺.
</em>
The H⁺ concentration in a vinegar pH = 2 is:
pH = -log [H⁺]
2 = -log [H⁺]
1x10⁻²M = [H⁺]
4L are just 4x10⁻² moles of [H⁺]. As you need 131100 moles of H⁺:
<h3>The vinegar is not enough to neutralize the pool.</h3>
Answer:
0.0222 mole of NaOH is needed to react with NH4F
Explanation:
NH4F + NaOH --> NaF + NH3 + H2O
Data given
Mass of NH4F =0.821g, Concentration of NaOH= 1M, volume of NaoH =25ml
But mole = (CV)/1000
given mole of NaoH = (1 * 25)/1000 = 0.025moles of NaOH used
Molar mass of NH4F = 37g/mol
mole of NH4F used 0.821 / 37 = 0.0222 mole NH4F
Determine the excess and limiting reactant,
NaOH is in excess
0.025 - 0.0222 = 0.0028 mole NaOH excess
0.0222 mole of NaOH is required to react with NH4F
Rutherford, Geiger and Marsden's experiment proved that every atom has a nucleus and that this nucleus is of positive charge and contains the most of the mass of the atom. 0.005% of the volume occupied by the electrons is the volume of the nucleus.
Given :
The student looks up the value of the appendix of his textbook but cannot find a value for NaCl.
To Find :
Why the Ksp of NaCl is not present .
Solution :
Ksp values are given for those compounds which are partially soluble or insoluble in water .
But , we know NaCl is strong electrolyte and it completely dissociated in water .
So , the reaction go forward and their is no need to calculate Ksp .
Therefore , the Ksp of NaCl is not present .
Hence , this is the required solution .
Homogeneous Mixture:
<span>It may be mistaken for a pure substance.
</span><span>It can be separated using distillation
</span>
Heterogeneous Mixture:
<span>Its components are visible
</span><span>It can be separated using distillation.
Concrete is an example of this kind of mixture.
</span>
Hope this helps!
