Biochemistry Lab Solution Preparation Quiz

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Questions and Answers

What is the molecular weight of NaCl?

35.45 g/mol

58.44 g/mol (correct)

22.99 g/mol

45.44 g/mol

How many moles of NaCl are needed to prepare 100 ml of 0.1 N solution?

0.5844 moles

1 mole

0.1 moles

0.05844 moles (correct)

What is the definition of normality (N) in this context?

Concentration in moles per liter of solution

Molar mass per liter of solution

Number of molecules per liter of solution

Number of equivalents of a solute per liter of solution (correct)

If a 0.2 N solution of NaCl is needed, what volume of solution would contain 1 mole of NaCl?

100 ml Signup and view all the answers

If the molar mass of a compound is 40 g/mol, how many grams are needed to prepare 500 ml of 0.2 N solution?

16 g Signup and view all the answers

What is the molecular weight of NaCl?

The molecular weight of NaCl is calculated by adding the molar masses of sodium (Na) and chlorine (Cl): $22.99 , \text{g/mol} (Na) + 35.45 , \text{g/mol} (Cl) = 58.44 , \text{g/mol}$. Signup and view all the answers

How many moles of NaCl are needed to prepare 100 ml of 0.1 N solution?

To calculate the moles of NaCl needed, we can use the formula: Moles = Normality $\times$ Volume (in liters). So, for a 0.1 N solution and 100 ml (0.1 L) volume, the moles of NaCl needed would be: Moles = 0.1 N $\times$ 0.1 L = 0.01 moles. Signup and view all the answers

What is the definition of normality (N) in this context?

In this context, normality (N) is defined as the number of equivalents of a solute per liter of solution. Signup and view all the answers

If you need to prepare a 0.1 N solution of NaCl, what mass of NaCl would be required to make 500 ml of the solution?

To calculate the mass of NaCl required, we can use the formula: Mass = Moles $\times$ Molecular weight. Using the previously calculated moles (0.01) and the molecular weight of NaCl (58.44 g/mol), the mass of NaCl required would be: Mass = 0.01 moles $\times$ 58.44 g/mol = 0.5844 grams. Signup and view all the answers

How many equivalents of NaCl are present in 100 ml of 0.1 N solution?

To calculate the equivalents of NaCl, we can use the formula: Equivalents = Normality $\times$ Volume (in liters). For a 0.1 N solution and 100 ml (0.1 L) volume, the equivalents of NaCl present would be: Equivalents = 0.1 N $\times$ 0.1 L = 0.01 equivalents. Signup and view all the answers

What is the molecular weight of NaCl?

The molecular weight of NaCl is calculated by adding the molar masses of sodium (Na) and chlorine (Cl): [ \text{Molecular weight of NaCl} = 22.99 , \text{g/mol (Na)} + 35.45 , \text{g/mol (Cl)} = 58.44 , \text{g/mol} ] Signup and view all the answers

If 0.1 N NaCl solution is to be prepared, how many moles of NaCl are needed to prepare 100 ml of the solution?

To prepare a 0.1 N solution of NaCl, the number of moles needed can be calculated using the formula: [ \text{Number of moles} = \text{Normality} \times \text{Volume (in liters)} = 0.1 \times 0.1 = 0.01 , \text{moles} ] Signup and view all the answers

Define the normality (N) in the context of this solution preparation.

In this context, normality (N) is defined as the number of equivalents of a solute per liter of solution. For NaCl, as it is a simple ionic compound, 1 mole of NaCl is equivalent to 1 mole of Na+ ions and 1 mole of Cl- ions. Signup and view all the answers

If a 0.2 N solution of NaCl is needed, what volume of solution would contain 1 mole of NaCl?

The volume of solution containing 1 mole of NaCl for a 0.2 N solution can be calculated using the formula: [ \text{Volume (in liters)} = \frac{\text{Number of moles}},{\text{Normality}} = \frac{1},{0.2} = 5 , \text{liters} ] Signup and view all the answers

If the molar mass of a compound is 40 g/mol, how many grams are needed to prepare 500 ml of 0.2 N solution?

The grams needed to prepare a 0.2 N solution can be calculated using the formula: [ \text{Grams} = \text{Number of moles} \times \text{Molar mass} = 0.1 \times 40 = 4 , \text{grams} ] Signup and view all the answers

Study Notes

Preparation of 0.1N 100mL Solution of NaCl

To prepare a 0.1N 100mL solution of NaCl, the molecular weight of NaCl is required, which is calculated by summing the molar masses of Na and Cl.
The molar mass of Na is approximately 22.99 g/mol.
The molar mass of Cl is approximately 35.45 g/mol.
The molecular weight of NaCl is 58.44 g/mol (22.99 g/mol + 35.45 g/mol).

Calculating the Number of Moles of NaCl

Normality (N) is defined as the number of equivalents of a solute per liter of solution.
For NaCl, 1 mole is equivalent to 1 mole of Na+ ions and 1 mole of Cl- ions.
To prepare 0.1N NaCl, the number of moles of NaCl needed is calculated based on the normality and volume of the solution.

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Description

Test your knowledge on solution preparation and pH adjustment in the biochemistry lab. This quiz covers the preparation of different buffers, pH adjustment, and the calculation of molecular weight for creating solutions. Ideal for students and professionals in the field of biochemistry.