C.354
1L/1000cm^3
0.354L/ycm^3 *1L/1000cm^3
Cross multiply 0.354 by 1000and then divide by one to get 354.
Answer:
≈194.7
Explanation:
(547cm^3/590K) / (V2/210K)
V2 = 194.69 or 194.7
:D
Not 100% sure, but I think it’s Water, hope this helps
Answer:
Total concentration of ions present in the final solution is 0.0726 M.
Explanation:
Mass of silver nitrate = 54.0 g
Moles of silver nitrate = ![\frac{54.0 g}{170 g/mol}=0.318 mol](https://tex.z-dn.net/?f=%5Cfrac%7B54.0%20g%7D%7B170%20g%2Fmol%7D%3D0.318%20mol)
Volume of the solution made = V = 350.0 mL = 0.350 L
![Molarity=\frac{Moles}{Volume(L)}](https://tex.z-dn.net/?f=Molarity%3D%5Cfrac%7BMoles%7D%7BVolume%28L%29%7D)
![M=\frac{0.318 mol}{0.35 L} =0.9086 M](https://tex.z-dn.net/?f=M%3D%5Cfrac%7B0.318%20mol%7D%7B0.35%20L%7D%20%3D0.9086%20M)
After dilution of 10.00 mL 0.9227 M solution.
![M_1=0.9086 M](https://tex.z-dn.net/?f=M_1%3D0.9086%20M)
![V_1=10.00 mL](https://tex.z-dn.net/?f=V_1%3D10.00%20mL)
![M_2=?](https://tex.z-dn.net/?f=M_2%3D%3F)
![V_2=250.0 mL](https://tex.z-dn.net/?f=V_2%3D250.0%20mL)
![M_1V_1=M_2V_2](https://tex.z-dn.net/?f=M_1V_1%3DM_2V_2)
![M_2=\frac{M_1V_1}{V_2}=\frac{0.9086 M\times 10.00 mL}{250.0 mL}](https://tex.z-dn.net/?f=M_2%3D%5Cfrac%7BM_1V_1%7D%7BV_2%7D%3D%5Cfrac%7B0.9086%20M%5Ctimes%2010.00%20mL%7D%7B250.0%20mL%7D)
![M_2=0.0363 M](https://tex.z-dn.net/?f=M_2%3D0.0363%20M)
Concentration of silver nitrate after dilution = 0.0363 M
![AgNO_3\rightarrow Ag^++NO_3^{-}](https://tex.z-dn.net/?f=AgNO_3%5Crightarrow%20Ag%5E%2B%2BNO_3%5E%7B-%7D)
![[AgNO_3]=[Ag^+]=[NO_3^{-}]=0.0363 M](https://tex.z-dn.net/?f=%5BAgNO_3%5D%3D%5BAg%5E%2B%5D%3D%5BNO_3%5E%7B-%7D%5D%3D0.0363%20M)
Total concentration of ions present in the final solution:
![[Ag^+]+[NO_3^{-}]=0.0363 M+0.0363 M=0.0726 M](https://tex.z-dn.net/?f=%5BAg%5E%2B%5D%2B%5BNO_3%5E%7B-%7D%5D%3D0.0363%20M%2B0.0363%20M%3D0.0726%20M)
<span>[Ne] 3s2 3p5
Hope this helps!</span>