A water desalination plant is set up near a salt marsh containing water that is 0.10 M NaCl. Calculate the minimum pressure that must be applied at $20 ^\circ$ to purify the water by reverse osmosis. Assume that NaCl is completely dissociated.

If the human eye has an osmotic pressure of 8.00 atm at $25 ^ { \circ } \mathrm { C } ,$ what concentration of solute particles in water will provide an isotonic eyedrop solution (a solution with equal osmotic pressure)?

Calculate the freezing point and the boiling point of each of the following solutions. (Assume complete dissociation.) $2.0\ \mathrm{g}\ \mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}$ in $15\ \mathrm{g}\ \mathrm{H}_{2} \mathrm{O}$

Compute f'(x) using the limit definition.

$$f ( x ) = x - \sqrt { x }$$

An unknown compound contains only carbon, hydrogen, and oxygen. Combustion analysis of the compound gives mass percents of 31.57% C and 5.30% H. The molar mass is determined by measuring the freezingpoint depression of an aqueous solution. A freezing point of $- 5.20 ^ { \circ } \mathrm { C }$ is recorded for a solution made by dissolving 10.56 g of the compound in 25.0 g of water. Determine the empirical formula, molar mass, and molecular formula of the compound. Assume that the compound is a nonelectrolyte.

From the following:

$$\begin{array} { l } { \text { pure water } } \\ { \text { solution of } \mathrm { C } _ { 6 } \mathrm { H } _ { 12 } \mathrm { O } _ { 6 } ( \chi = 0.01 ) \text { in water } } \\ { \text { solution of } \mathrm { NaCl } ( \chi = 0.01 ) \text { in water } } \\ { \text { solution of } \mathrm { CaCl } _ { 2 } ( \chi = 0.01 ) \text { in water } } \end{array}$$

choose the one with the following: lowest freezing point

From the following: pure water

$$\begin{array} { l } { \text { solution of } \mathrm { C } _ { 6 } \mathrm { H } _ { 12 } \mathrm { O } _ { 6 } ( \chi = 0.01 ) \text { in water } } \\ { \text { solution of } \mathrm { NaCl } ( \chi = 0.01 ) \text { in water } } \\ { \text { solution of } \mathrm { CaCl } _ { 2 } ( \chi = 0.01 ) \text { in water } } \end{array}$$

choose the one with the following: lowest boiling point

From the following: pure water

$$\begin{array} { l } { \text { solution of } \mathrm { C } _ { 6 } \mathrm { H } _ { 12 } \mathrm { O } _ { 6 } ( \chi = 0.01 ) \text { in water } } \\ { \text { solution of } \mathrm { NaCl } ( \chi = 0.01 ) \text { in water } } \\ { \text { solution of } \mathrm { CaCl } _ { 2 } ( \chi = 0.01 ) \text { in water } } \end{array}$$

choose the one with the following: highest boiling point

From the following:

$$\begin{array} { l } { \text { pure water } } \\ { \text { solution of } \mathrm { C } _ { 6 } \mathrm { H } _ { 12 } \mathrm { O } _ { 6 } ( \chi = 0.01 ) \text { in water } } \\ { \text { solution of } \mathrm { NaCl } ( \chi = 0.01 ) \text { in water } } \\ { \text { solution of } \mathrm { CaCl } _ { 2 } ( \chi = 0.01 ) \text { in water } } \end{array}$$

choose the one with the following: highest freezing point

The equilibrium constant for a certain reaction increases by a factor of 6.67 when the temperature is increased from 300.0 K to 350.0 K. Calculate the standard change in enthalpy $\left( \Delta H ^ { \circ } \right)$ for this reaction (assuming $\Delta H ^ { \circ }$ is temperature-independent).

From the following: pure water

$$\begin{array} { l } { \text { solution of } \mathrm { C } _ { 6 } \mathrm { H } _ { 12 } \mathrm { O } _ { 6 } ( \chi = 0.01 ) \text { in water } } \\ { \text { solution of } \mathrm { NaCl } ( \chi = 0.01 ) \text { in water } } \\ { \text { solution of } \mathrm { CaCl } _ { 2 } ( \chi = 0.01 ) \text { in water } } \end{array}$$

choose the one with the following: highest osmotic pressure

What mass of glycerin $\left( \mathrm { C } _ { 3 } \mathrm { H } _ { 8 } \mathrm { O } _ { 3 } \right) ,$ a nonelectrolyte, must be dissolved in 200.0 g of water to give a solution with a freezing point of $- 1.50 ^ { \circ } \mathrm { C }?$

The term proof is defined as twice the percent by volume of pure ethanol in solution. Thus a solution that is 95% (by volume) ethanol is 190 proof. What is the molarity of ethanol in a 92 -proof ethanolwater solution? Assume the density of ethanol $\left( \mathrm { C } _ { 2 } \mathrm { H } _ { 5 } \mathrm { OH } \right)$ is $0.79\ \mathrm { g } / \mathrm { cm } ^ { 3 }$ and the density of water is $1.0\ \mathrm { g } / \mathrm { cm } ^ { 3 }.$

The equilibrium constant for a certain reaction increases by a factor of 6.67 when the temperature is increased from 300.0 K to 350.0 K. Calculate the standard change in enthalpy $\left(\Delta H^{\circ}\right)$ for this reaction (assuming $\Delta H^{\circ}$ is temperature-independent).