Answer:- density of the liquid is 0.21 gram per mL.
Solution:- ![density=\frac{mass}{volume}](https://tex.z-dn.net/?f=density%3D%5Cfrac%7Bmass%7D%7Bvolume%7D)
From given data, mass of cylinder = 10.4 g
mass of cylinder along with liquid = 11.7 g
So, mass of liquid = 11.7 g - 10.4 g = 1.3 g
Volume of liquid = 6.2 mL
Let's divide the mass by the volume to get the density of the liquid:
![density=\frac{1.3g}{6.2mL}](https://tex.z-dn.net/?f=density%3D%5Cfrac%7B1.3g%7D%7B6.2mL%7D)
density = ![0.21\frac{g}{mL}](https://tex.z-dn.net/?f=0.21%5Cfrac%7Bg%7D%7BmL%7D)
So, the density of the liquid is 0.21 gram per mL.
<span>The correct answer is D.how wind and temperature affect your body in winter. Basically, it's how you perceive the cold weather on your skin regardless of what the temperature actually is. It's usually lower and that's why you have forecasts say that it will be for example 0, but it will feel like -5 degrees Celsius.</span><span />
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
![1 mL = 0.001L\\V=250 mL=250\times 0.001 L=0.250 L](https://tex.z-dn.net/?f=1%20mL%20%3D%200.001L%5C%5CV%3D250%20mL%3D250%5Ctimes%200.001%20L%3D0.250%20L)
The moles of fluoride ion needed = n
According to the definition of molarity:
![M=\frac{n}{V}\\0.100M=\frac{n}{0.250 L}\\n=0.100M\times 0.250 L=0.025 mol](https://tex.z-dn.net/?f=M%3D%5Cfrac%7Bn%7D%7BV%7D%5C%5C0.100M%3D%5Cfrac%7Bn%7D%7B0.250%20L%7D%5C%5Cn%3D0.100M%5Ctimes%200.250%20L%3D0.025%20mol)
Moles of fluoride ion = 0.025 mol
We know that solid calcium fluoride dissolves in water to give calcium ions and fluoride ions.
![CaF_2(s)\rightarrow Ca^{2+}(aq)+2F^-(aq)](https://tex.z-dn.net/?f=CaF_2%28s%29%5Crightarrow%20Ca%5E%7B2%2B%7D%28aq%29%2B2F%5E-%28aq%29)
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:
![=\frac{1}{2}\times 0.025 mol=0.0125 \text{mol of } CaF_2](https://tex.z-dn.net/?f=%3D%5Cfrac%7B1%7D%7B2%7D%5Ctimes%200.025%20mol%3D0.0125%20%5Ctext%7Bmol%20of%20%7D%20CaF_2)
Moles of calcium fluoride = 0.0125 mol
Mass of calcium fluoride needed to prepare the solution :
![=0.0125 mol\times 78.07 g/mol=0.975875 g](https://tex.z-dn.net/?f=%3D0.0125%20mol%5Ctimes%2078.07%20g%2Fmol%3D0.975875%20g)
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:
brainly.com/question/10053901?referrer=searchResults
brainly.com/question/10270173?referrer=searchResults
C, hope it was correct. Pls give brainest answer if it was correct
I think b because it talks more about the question