Earth because it has so much water come on b
Explanation:
Let us assume that the given data is as follows.
mass of barium acetate = 2.19 g
volume = 150 ml = 0.150 L (as 1 L = 1000 ml)
concentration of the aqueous solution = 0.10 M
Therefore, the reaction equation will be as follows.
![Ba(C_{2}H_{3}O_{2})_{2} \rightarrow Ba^{2+} + 2C_{2}H_{3}O^{-}_{2}](https://tex.z-dn.net/?f=Ba%28C_%7B2%7DH_%7B3%7DO_%7B2%7D%29_%7B2%7D%20%5Crightarrow%20Ba%5E%7B2%2B%7D%20%2B%202C_%7B2%7DH_%7B3%7DO%5E%7B-%7D_%7B2%7D)
Hence, moles of
=
.......... (1)
As, No. of moles =
Hence, moles of
will be calculated as follows.
No. of moles =
=
(molar mass of
is 255.415 g/mol)
= ![8.57 \times 10^{-3}](https://tex.z-dn.net/?f=8.57%20%5Ctimes%2010%5E%7B-3%7D)
Moles of
= ![2 \times 8.57 \times 10^{-3}](https://tex.z-dn.net/?f=2%20%5Ctimes%208.57%20%5Ctimes%2010%5E%7B-3%7D)
= 0.01715 mol
Hence, final molarity will be as follows.
Molarity = ![\frac{\text{no. of moles}}{volume}](https://tex.z-dn.net/?f=%5Cfrac%7B%5Ctext%7Bno.%20of%20moles%7D%7D%7Bvolume%7D)
= ![\frac{0.01715 mol}{0.150 L}](https://tex.z-dn.net/?f=%5Cfrac%7B0.01715%20mol%7D%7B0.150%20L%7D)
= 0.114 M
Thus, we can conclude that final molarity of barium cation in the solution is 0.114 M.
Answer:
The volume of the water after it freezes (at 0°C) is 354.4 mL.
Explanation:
We need to use this additional information, the densities of liquid water and ice at 0 °C are 1.000 g/mL and 0.917 g/mL, respectively.
Step 1. Find the mass of water before it freezes.
![325 \:mL \cdot 1.000 \:{\frac{g}{mL} }=325 \:g](https://tex.z-dn.net/?f=325%20%5C%3AmL%20%5Ccdot%201.000%20%5C%3A%7B%5Cfrac%7Bg%7D%7BmL%7D%20%7D%3D325%20%5C%3Ag)
Step 2. The mass does not change when the temperature does. So, you take the grams of water and divide it by the density of the ice to obtain the volume it occupies.
![325 \:g\cdot \frac{1}{0.917 \:{\frac{g}{mL} }} =354.4 \:mL](https://tex.z-dn.net/?f=325%20%5C%3Ag%5Ccdot%20%5Cfrac%7B1%7D%7B0.917%20%5C%3A%7B%5Cfrac%7Bg%7D%7BmL%7D%20%7D%7D%20%3D354.4%20%5C%3AmL)