NaCl Solution Preparation

The necessary mass of NaCl can be calculated using the formula: $mass = molarity \times volume \times molar\ mass$. Substituting the given values, we get: $mass = 0.01 \times 250 \times 58.44 = 146.5 \text{ grams}$.

The necessary mass of NaCl can be calculated using the formula: $mass = molarity \times volume \times molar\ mass$. Substituting the given values, we get: $mass = 0.2 \times 250 \times 58.44 = 2930 \text{ grams}$.

The necessary mass of NaCl can be calculated using the formula: $mass = molarity \times volume \times molar\ mass$. Substituting the given values, we get: $mass = 0.1 \times 250 \times 58.44 = 1465 \text{ grams}$.

<p>The necessary mass of NaCl for the preparation of 250 ml of 0.2M solution is calculated using the formula: $mass = \text{volume} \times \text{molarity} \times \text{molar mass}$. Thus, $mass = 0.25 , \text{L} \times 0.2 , \text{mol/L} \times 58.44 , \text{g/mol} = 2.92 , \text{g}$.</p> Signup and view all the answers

<p>The necessary mass of NaCl for the preparation of 250 ml of 0.1M solution is calculated using the formula: $mass = \text{volume} \times \text{molarity} \times \text{molar mass}$. Thus, $mass = 0.25 , \text{L} \times 0.1 , \text{mol/L} \times 58.44 , \text{g/mol} = 1.46 , \text{g}$.</p> Signup and view all the answers

<p>The necessary mass of NaCl for the preparation of 250 ml of 0.01M solution is calculated using the formula: $mass = \text{volume} \times \text{molarity} \times \text{molar mass}$. Thus, $mass = 0.25 , \text{L} \times 0.01 , \text{mol/L} \times 58.44 , \text{g/mol} = 0.146 , \text{g}$.</p> Signup and view all the answers