Question

what is the mloarity of a solution prepared by dissolving 50g of NaOH in 100ml of water​

Answer 1

Answer:

The correct answer of this question is the actual solution volume of solute is additive to the 100 mL of water then the Molarity is equal to 1.25 mol/0.1235 L or 10.12 M.

Explanation:

Given - The mloarity of a solution prepared by dissolving 50g of NaOH in 100ml of water​ .

To Find - Write what is the mloarity of a solution prepared by dissolving 50g of NaOH in 100ml of water​ .

The density of the NaOH volume is 2.13 g/mL, the volume is 50 g /(2.13 g/mL) = 23.474 mL or 0.0235 L. The actual solute solution volume is additive to the 100 mL of water, the molarity is 1.25 mol/0.1235 L, or 10.12 M.

The NaOH volume is not additive, the solution's molarity is 1.25 mol/0.100 L, or 12.5 M.

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Answer 2

Step 1: Given data

Amount of $NaOH=50g$

Volume of water$=100mL$

Molarity of solution$=?$

Step 2: Using the formula

$M=\frac{n}{V}$, $n$ is number of moles, $V$ is the volume of solution in litres and $M$ is the molarity of solution.

Step 3: Calculating the molarity of the solution

Firstly, we have to convert $50g\ NaOH$ into moles by finding molar mass of $NaOH$.

We know that,

• $Na=\ 22.99\ g/mol$,  $1$ atom
• $O=\ 16.00\ g/mol$,  $1$ atom
•  $H=\ 1.01\ g/mol$,  $1$ atom

Molar mass of $NaOH$ is: 

$22.99\times 1+16.00\times 1+1.01\times 1=22.99+16.00+1.01=40.00g/mol$

The molar mass of $NaOH$ is $40\ g/mol$.

So $50g\ NaOH$ will have-

$50g\ NaOH=50g\ NaOH\times \frac{1\ mol\ NaOH}{40g\ NaOH}=\frac{50\ mol\ NaOH}{40} } =1.25\ mol\ NaOH$

Therefore, the moles of solute is $1.25\ mol$, which means $n=1.25$

Now,

$100mL=\frac{100}{1000}=0.1L$

So,

$M=\frac{1.25}{0.1}=12.5\ mol/L$

Hence, the molarity of solution is $12.5\ mol/L$.

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