How many grams of concentrated nitric acid solution should be used to prepare 250ml of 2.0 (M) HNO3 (the concentrated acid is 70% HNO3) a. 54g b. 45g c. 90g d. 70g. please explain it friends?

Question

Answer

Calculation of Concentrated Nitric Acid Solution

To prepare 250ml of 2.0 (M) HNO3, we need to calculate the amount of concentrated nitric acid solution required.

Step 1: Calculate the number of moles of HNO3 required

Molarity = Number of moles/Volume (in L)

2.0 (M) = Number of moles/0.25 L

Number of moles = 0.5 mol

Step 2: Calculate the mass of HNO3 required

Mass of HNO3 = Number of moles x Molar mass of HNO3

= 0.5 mol x 63 g/mol

= 31.5 g

Step 3: Calculate the volume of concentrated nitric acid solution required

The concentrated nitric acid is 70% HNO3, which means that 100 g of the solution contains 70 g of HNO3.

Let x be the volume of concentrated nitric acid solution required.

Mass of HNO3 in x ml of concentrated nitric acid solution = (70/100) x

Mass of HNO3 required = 31.5 g

(70/100) x = 31.5 g

x = (31.5 g x 100)/70

x = 45 g

Therefore, the amount of concentrated nitric acid solution required to prepare 250ml of 2.0 (M) HNO3 is 45g.

Answer: (b) 45g

Answer

Shayak ans is (b)45gm....2=(70*x*1000)/(100*250*63)where, x=required wt of HNO3...by solving x , we get x=45gm.....

Answer

(b)

Answer

Ans is 45gm.....??????

Answer

Thank you friends :-)..ans is 45 gm

Answer

B) 45 first find mass of nitric acid needed by molarity formula and then divide it by 0.7 because acid is 70% concentrated

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