How many grams of MgCl2 (molar mass = 95.20 g/mol) will be formed from 25.6 mL of a 0.100 M HCL solution reacting with excess ma
2 answers:
Answer:
0.1219 g
Explanation:
mole = mass/molar mass = molarity x volume
From the balanced equation of reaction:
1 mole of MgCl2 is formed from 2 moles of HCl
x mole of MgCl2 is formed from 0.1 x 0.0256 moles HCl
x mole of MgCl2 = 1 x 0.1 x 0.0256/2
= 0.00128
0.00128 moles of MgCl2 is formed from 0.00256 moles HCl
Hence,
mass of MgCl2 = moles x molar mass
= 0.00128 x 95.20
= 0.1219 g
<em>Therefore, 0.1219 g of MgCl2 will be formed from 25.6 mL of a 0.100 M HCL solution reacting with excess magnesium metal. </em>
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Answer:
a) [H₃O⁺] = 1.8x10⁻⁵ M
b) pH = 4.75
c) % rxn = 3.5x10⁻³ %
Explanation:
a) The dissociation reaction of HCN is:
HCN(aq) + H₂O(l) ⇄ H₃O⁺(aq) + CN⁻(aq)
0.5 M - x x x
The dissociation constant from the above reactions is given by:
By solving the above quadratic equation we have:
x = 1.75x10⁻⁵ M = 1.8x10⁻⁵ M = [H₃O⁺] = [CN⁻]
Hence, the [H₃O⁺] is 1.8x10⁻⁵ M.
b) The pH is equal to:
Then, the pH of the HCN solution is 4.75.
c) The % reaction is the % ionization:
Therefore, the % reaction or % ionization is 3.5x10⁻³ %.
I hope it helps you!
Explanation:
The reaction equation will be as follows.
Hence, the expression for is as follows.
Let us assume that the concentration of both and
is x.
x = 0.01118034
This means that the concentration of is 0.01118034.
Since, we know that the relation between pH and concentration of hydrogen ions is as follows.
pH =
=
= 1.958
Thus, we can conclude that the pH of a 0.500 M solution of arsenic acid is 1.958.