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Chemistry

1 answer:

Vlad [161]3 years ago

7 0

Answer:

yum yummy

Explanation:

Mis-ka, Mou-ska

Mickey Mouse!

M-I-C-K-E-Y

M-O-U-S-E (that's me!)

M-I-C-K-E-Y

M-O-U-S-E

It's the Mickey Mouse Clubhouse

Come inside, it's fun inside

It's the Mickey Mouse Clubhouse (roll call!)

Donald (present!)

Daisy (here!)

Goofy (hyuck, here!)

Pluto (woof! woof!)

Minnie (hi, here!)

Mickey (right here!)

It's the Mickey Mouse Clubhouse

Come inside, it's fun inside

M-I-C-K-E-Y

M-O-U-S-E

You might be interested in

In the background information, it was stated that CaF2 has solubility, at room temperature, of 0.00160 g per 100 g of water. How

____ [38]

Answer:

2.05*10⁻⁵ moles of CF₂ can dissolve in 100 g of water.

12.82 moles of CaF₂ will dissolve in exactly 1.00 L of solution

Explanation:

First, by definition of solubility, in 100 g of water there are 0.0016 g of CaF₂. So, to know how many moles are 0.0016 g, you must know the molar mass of the compound. For that you know:

Ca: 40 g/mole
F: 19 g/mole

So the molar mass of CaF₂ is:

CaF₂= 40 g/mole + 2*19 g/mole= 78 g/mole

Now you can apply the following rule of three: if there are 78 grams of CaF₂ in 1 mole, in 0.0016 grams of the compound how many moles are there?

$moles=\frac{0.0016 grams*1 mole}{78 grams}$

moles=2.05*10⁻⁵

2.05*10⁻⁵ moles of CF₂ can dissolve in 100 g of water.

Now, to answer the following question, you can apply the following rule of three: if by definition of density in 1 mL there is 1 g of CaF₂, in 1000 mL (where 1L = 1000mL) how much mass of the compound is there?

$mass of CaF_{2}=\frac{1000 mL*1g}{1mL}$