1. Two students below described a type of Earth's outermost layer:
2 answers:
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Statement D is the correct option as the solution will have pH of 3. It has an H3O+ ion concentration of 1 × mol/L and is acidic.
Explanation:
It is given in question that solution must have pH of 3. The value if being less than 7 shows that solution is acidic. The pH value of 3 indicates that given solution is highly acidic and has strong acid. Strong acid gets fully dissociated into ions.
pH of the solution is calculated as:
pH = -log10[]
the concentration or molarity of the hydronium ion is given as moles/litre
concentration of hydronium ion in the solution is 1 X moles/litre
putting the values in the equation:
pH = - log10( 1 X )
pH = 3 (acidic)
Thus it can be concluded that D option is the right answer.
Answer:
0.182 moles of acetic acid are needed, this means 10.93 g.
0.318 moles of sodium acetate are needed, this means 26.08 g.
Explanation:
The Henderson–Hasselbalch (<em>H-H</em>) equation tells us the relationship between the concentration of an acid, its conjugate base, and the pH of a buffer:
pH = pka +
In this case, [A⁻] is the concentration of sodium acetate, and [HA] is the concentration of acetic acid. The pka is a value that can be looked up in literature: 4.76.
From the problem we know that
[A⁻] + [HA] = 250 mM = 0.250 M eq. 1
We use the <em>H-H</em> equation, using the data we know, to describe [A⁻] in terms of [HA]:
5.0 = 4.76 +
eq.2
Now we replace the value of [A⁻] in eq. 1, to calculate [HA]:
1.74 [HA] + [HA] = 0.250 M
[HA] = 0.091 M
Then we calculate [A⁻]:
[A⁻] + 0.091 M = 0.250 M
[A⁻] = 0.159 M
Using the volume, we can calculate the moles of each substance:
- moles of acetic acid = 0.091 M * 2 L = 0.182 moles
- moles of sodium acetate = 0.159 M * 2 L = 0.318 moles
Using the molecular weight, we can calculate the grams of each substance:
- grams of acetic acid = 0.182 mol * 60.05 g/mol = 10.93 g
- grams of sodium acetate = 0.318 mol * 82.03 g/mol = 26.08 g