A 2.0% (w/v) solution of sodium hydrogen citrate, Na₂C₆H₆O₇, which also contains 2.5% (w/v) of dextrose, C₆H₁₂O₆, is used as an anticoagulant for blood which is to be used for transfusions. What is the molarity of the sodium hydrogen citrate in the solution? A)0.085 M B)0.19 M C)0.53 M D)1.2 M E)1.3 M

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To find the molarity, we need to calculate the moles of sodium hydrogen citrate in 1 liter of solution. A 2.0% (w/v) solution means 2.0 grams of sodium hydrogen citrate per 100 mL of solution. Therefore, in 1 liter (1000 mL), there are 20 grams of sodium hydrogen citrate. The molar mass of Na₂C₆H₆O₇ is approximately 236.1 g/mol. Moles = mass/molar mass = 20 g / 236.1 g/mol ≈ 0.085 mol. Thus, the molarity is approximately 0.085 M.

A 20% (W/v) Solution of Sodium Hydrogen Citrate, Na2C6H6O7, Which Also

A 20% (W/v) Solution of Sodium Hydrogen Citrate, Na₂C₆H₆O₇, Which Also