Let's solve each part step by step: --- ### **a. Calculate the number of dextrose molecules per liter in 5% dextrose in water.** - **5% dextrose solution** means **5 g of dextrose per 100 mL**. - So, in **1 liter (1000 mL):** \[ \text{Amount of dextrose} = 5\,\text{g} \times 10 = 50\,\text{g} \] - **Molar mass of dextrose (C₆H₁₂O₆):** C: 12 × 6 = 72 H: 1 × 12 = 12 O: 16 × 6 = 96 **Total = 72 + 12 + 96 = 180 g/mol** - **Moles of dextrose in 1 L:** \[ \text{Moles} = \frac{50\,\text{g}}{180\,\text{g/mol}} = 0.278\,\text{mol} \] - **Number of molecules (using Avogadro's number, \(6.022 \times 10^{23}\) molecules/mol):** \[ \text{Number of molecules} = 0.278\,\text{mol} \times 6.022 \times 10^{23}\,\text{molecules/mol} \] \[ = 1.67 \times 10^{23}\,\text{molecules} \] **Final Answer for (a):** \[ \boxed{1.67 \times 10^{23}\ \text{dextrose molecules per liter}} \] --- ### **b. Is this solution hypotonic, isotonic, or hypertonic? Explain.** - A 5% dextrose solution in water is considered **isotonic** with blood plasma. - **Reason:** The osmotic pressure of 5% dextrose approximates that of blood plasma, so it does not cause cells to gain or lose water. **Final Answer for (b):** \[ \boxed{\text{Isotonic.}} \] **A 5% dextrose solution is isotonic with blood because its osmotic pressure is similar to that of plasma, preventing net movement of water into or out of cells.** --- Let me know if you need more explanation or calculation details!

Yes, I am confident in the calculations and explanations provided. **Here's a quick summary:** - **Part a:** Calculated 5 g of dextrose per 100 mL, scaled to 1 liter (50 g), then used molar mass (180 g/mol) to find moles (0.278 mol), and multiplied by Avogadro's number (6.022 × 10²³) to get approximately **1.67 × 10²³ molecules** per liter. - **Part b:** 5% dextrose solution is **generally considered isotonic** with blood because it has a similar osmotic pressure, preventing water movement into or out of cells. If you'd like, I can provide more detailed explanations or references for these conclusions.

**Final Answers:** a. Approximately **1.67 × 10²³ dextrose molecules per liter**. b. The solution is **isotonic** with blood.

Certainly! Here's a brief theoretical explanation of a 5% dextrose in water solution: **Theoretical Explanation:** A 5% dextrose solution contains 5 grams of glucose (dextrose) dissolved in 100 mL of water. This concentration is commonly used in clinical settings as an intravenous fluid because it provides a source of glucose without significantly altering the osmotic balance between the blood plasma and the solution. From an osmotic perspective, the key concept is **osmotic pressure**, which depends on the number of solute particles in solution. Since dextrose is a non-electrolyte that does not dissociate, the osmotic pressure is directly proportional to the molar concentration of glucose molecules. Because the osmotic pressure of the 5% dextrose solution is similar to that of blood plasma (~280 mOsm/L), it is considered **isotonic**. This means it can be safely administered without causing water to move into or out of the cells, thus maintaining cellular equilibrium. **In summary:** - The 5% dextrose solution provides a molar concentration of about 0.278 mol/L. - It contains approximately \(1.67 \times 10^{23}\) glucose molecules per liter. - Its osmotic pressure matches that of blood plasma, making it an isotonic solution suitable for intravenous therapy. This balance ensures that the solution helps provide energy (via glucose) without disrupting the body's osmotic homeostasis.