HCl = H⁺ + Cl⁻
c(HCl)=9.8*10⁻⁵ mol/l
pH=-lg[H⁺]
[H⁺]=c(HCl)
pH=-lg{c(HCl)}
pH=-lg{9.8*10⁻⁵}=4.009
pH=4.009
A because b is for photosynthesis
The weight of aluminum are required to produce 8.70 moles of aluminum chloride is 234.9 g
<h3>
What is the use of aluminium chloride ?</h3>
Aluminum chloride is useful for the treatment of palmar, plantar, and axillary hyperhidrosis.
Aluminum chloride has also been reported to be useful in facial and scalp hyperhidrosis
The balanced chemical equation represents the mole ratio in which the chemicals combine.
In this case, illustrates that 2 mol Al produces 2 mol Al Cl₃, hence these 2 chemicals are in a 1:1 ratio.
Thus, to produce 8.70 mol aluminium chloride, it will require 8.70 mol aluminium.
But this quantity of Al has a mass in grams of
m = n × Mr
= 8.70 mol × 27g/mol
= 234.9 g
Hence, The weight of aluminum are required to produce 8.70 moles of aluminum chloride is 234.9 g
Learn more about mole concept here ;
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