In 250 mL of volumetric flask add 0.975875 grams of and dissolve it in the 250 mL of water.
Given:
The solid of calcium fluoride.
To prepare:
The 250 mL solution of 0.100 M of fluoride ions from solid calcium fluoride.
Method:
Molarity of the fluoride ion solution needed = M = 0.100 M
The volume of the fluoride ion solution needed = V = 250 mL
The moles of fluoride ion needed = n
According to the definition of molarity:
Moles of fluoride ion = 0.025 mol
We know that solid calcium fluoride dissolves in water to give calcium ions and fluoride ions.
According to reaction, 2 moles of fluoride ions are obtained from 1 mole of calcium fluoride, then 0.025 moles of fluoride ions will be obtained from:
Moles of calcium fluoride = 0.0125 mol
Mass of calcium fluoride needed to prepare the solution :
Preparation:
- Weight 0.975875 grams of calcium fluoride
- Add weighed calcium fluoride to a volumetric flask of the labeled volume of 250 mL.
- Now add a small amount of water to dissolve the calcium fluoride completely.
- After this add more water up to the mark of the volumetric flask of volume 250 mL.
Learn more about molarity of solution ere:
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Please see the answer here
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Answer:325 mL of acid
Explanation:250 mL + 75 mL = 325 mL
Answer : The correct option is, (1) Gains an electron and its radius increases.
Explanation :
The given element is chlorine.
Atomic number of chlorine = '17'
The electronic configuration of chlorine is,
Number of electrons = 17
Number of protons = 17
The electronic configuration of chloride ion is,
Number of electrons = 18
Number of protons = 17
When the chlorine atom gains an electron to acquire a stable electronic configuration. As the electrons add in the valence shell of the chlorine, the number of electrons increases but the number of protons remains the same. So, the protons will not be able to bind the extra electron and it will remain far from the nucleus.