Question

What volume of water should be added to 50ml of HNO3 having density 1.5g/ml and 63% by weight to have one molar solution

Answer 1

Mass of HNO3 solution = 50 mL * 1.5 g/mL 

Mass of HNO3 = mass of HNO3 solution * 0.63 

Convert mass of HNO3 to moles. 

for molarity, concentration = moles / volume. 

concentration is 1 mole/L per the problem. You just worked out the moles of HNO3. Calculate the volume of the solution. 

Volume of water = volume of solution from above - 50 mL

Answer 2

Answer: Volume of water to be added to 50ml of HNO3 having density 1.5g/ml and 63% by weight to have one molar solution is 700 ml.

Explanation:-  Given: $HNO_3$ is labelled as 63% by weight means 63 gram of $HNO_3$ is dissolved in 100 g of solution.

To calculate the moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\textMolar mass}}=\frac{63g}{63g/mol}=1mole$

Density of solution= 1.5 g/ml

Now we have to calculate the volume of solution.

$Density=\frac{Mass}{Volume}$

$Volume=\frac{mass}{Density}=\frac{100g}{1.5g/ml}=66.7ml$

Molarity : It is defined as the number of moles of solute present per liter of the solution.

Formula used :

$Molarity=\frac{n\times 1000}{V_s}$

where,

n= moles of solute

$V_s$ = volume of solution in ml

$Molarity=\frac{1\times 1000}{66.7ml}=15M$

According to the neutralization law,According to the neutralization law,  

$M_1V_1=M_2V_2$

$15\times 50ml=1\times V_2$     (1L=1000ml)

$V_2=750ml$

Thus water added is 750-50 = 700 ml.