<h3>
Answer:</h3>
The molecular weight of unknown acid is 33.33 g
<h3>
Explanation:</h3>
- The reaction between an acid and a base such as NaOH is called a neutralization reaction.
- Neutralization titration may be used to standardize a solution or determine the concentration of solution whose molarity is unknown.
- The balanced equation for reaction between an acid and Sodium hydroxide is
HX(aq)+ NaOH(aq) → NaX(aq)+ H₂O(l)
We need to determine the molecular weight of the acid;
<h3>Step 1: Moles of Sodium hydroxide </h3>
Number of moles is given by multiplying molarity and volume of the solution.
Number of moles = Molarity × Volume
= 0.103 M × 0.04365 L
= 0.0045 Moles NaOH
<h3>Step 2: Moles of the acid </h3>
The mole ratio of the acid to NaOH is 1:1
Therefore; the moles of the acid will be 0.0045 moles
<h3>Step 3: Molecular weight of the acid </h3>
Moles of the acid that reacted are 0.0045 moles
Mass of the acid in 0.0045 moles is 0.1500 g
Therefore;
Molecular weight = mass ÷ moles
= 0.1500 g ÷ 0.0045 moles
= 33.33 g/mol
Therefore, the molecular weight of the acid in grams is 33.33 g
It should be (electrons are evenly distributed in the water molecule) .
Let me know if you need more help!
The parent isotope percent will change from 100% to 50% to 25% to 12.5% and to 6.25%. So the sample go through four times of half-life. So the sample is 58*4=232 years old.
the correct answer is choice D
M₁ x V₁ = M₂ x V₂
2.5 x V₁ = 0.50 x 100.0
2.5 x V₁= 50
V₁ = 50 / 2.5
V₁= 20 mL
hope this helps!