Molarity : Molarity is defined as the moles of solute present in one liter of the solution. Or it is defined as the concentration of solute present in one liter of solution.

The unit of molarity is, (M) i.e, mole/liter. It is also known as molar concentration.

Molarity of 0.01 M means, 0.01 concentration of the acid present in the solution.

Therefore, the 0.01 M refer to the concentration of the acid.

5 0

4 years ago

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A certain ore is 24.3% nickel by mass. how many kilograms of this ore would you need to dig up to have 55.0 g of nickel?

zysi [14]

Let x be the mass of the ore in grams such that the equation that would allow us to answer this item would be,

55 = (x)(0.243)

The value of x is calculated as,

x = 55/0.243
x = 226.337 grams

Then, solve for amount in kilograms by dividing the calculated value by 1000. This methodology will give us an answer of 0.226337. Hence, the answer is 0.226.

4 0

3 years ago

What mass of sucrose (C12H22O11) should be combined with 546 g of water to make a solution with an osmotic pressure of 8.80 atm

lesya [120]

<u>Answer:</u> The mass of sucrose required is 69.08 g

<u>Explanation:</u>

To calculate the concentration of solute, we use the equation for osmotic pressure, which is:

$\pi=iMRT$

Or,

$\pi=i\times \frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}\times RT$

where,

$\pi$ = osmotic pressure of the solution = 8.80 atm

i = Van't hoff factor = 1 (for non-electrolytes)

Mass of solute (sucrose) = ?

Molar mass of sucrose = 342.3 g/mol

Volume of solution = 564 mL (Density of water = 1 g/mL)

R = Gas constant = $0.0821\text{ L.atm }mol^{-1}K^{-1}$

T = Temperature of the solution = 290 K

Putting values in above equation, we get:

$8.80atm=1\times \frac{\text{Mass of sucrose}\times 1000}{342.3\times 546}\times 0.0821\text{ L.atm }mol^{-1}K^{-1}\times 290K\\\\\text{Mass of sucrose}=\frac{8.80\times 342.3\times 546}{1\times 1000\times 0.0821\times 290}=69.08g$

Hence, the mass of sucrose required is 69.08 g

5 0

3 years ago