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What is the osmotic pressure of an aqueous solution of 1.64 $\mathrm{g}$ of $\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}$ in water at $25^{\circ} \mathrm{C} ?$ The volume ofthe solution is 275 $\mathrm{mL}$ .(a) Outline the steps necessary to answer the following question.(b) Answer the question.

2.67 $\mathrm{atm}$

02:16

Aadit S.

Chemistry 102

Chapter 11

Solutions and Colloids

Solutions

Carleton College

Rice University

University of Maryland - University College

Brown University

Lectures

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to determine the osmotic pressure of the solution That contains 1.64 g of calcium nitrate In 275 million liters of water. We will use the osmotic pressure equation First we will calculate the polarity of the calcium nitrate solution. Then we will recognize the I. Value. The Vonta factor will be three because we will produce one cat iron and to an ions. Then using the I. Value the value and the temperature. With the osmotic pressure equation, we can calculate osmotic pressure. To calculate polarity. It will take the mass of calcium nitrate divided by the molar mass of calcium nitrate to get most calcium nitrate and then divide that whole thing by the volume of the solution. In leaders it was 275 ml which equates to .275 leaders and we get a polarity a .20363 molar in i. value of three. Now we'll use the top equation with our I. value our polarity, the r. value and the temperature 25°C or to 98.15 Kelvin. And we'll get 2.67 atmospheres

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