Solutions

If the solid $NaCl$ in a saturated solution of $NaCl$ continues to dissolve, why is there no change in the concentration of the $NaCl$ solution? $(9.3)$

Identify the solute and the solvent in each solution composed of the following:

a. $10.0 g$ of $NaCl$ and $100.0 g$ of$H_{2}O$

b. $50.0 mL$ of ethanol, $C_2{H}_{6}O$, and $10.0 mL$ of $H_{2}O$

c. $0.20 L$ of $O_2$ and $0.80 L$ of $N_2$

Identify the solute and the solvent in each solution composed of the following:

a. $10.0 mL$ of acetic acid and $200 mL$ of water

b. $100.0 mL$ of water and $5.0 g$ of sugar

c. $1.0 g$ of $B{r}_2$ and $50.0 mL$ of methylene chloride $\left(l\right)$

Describe the formation of an aqueous $KI$ solution, when solid $KI$ dissolves in water.

Describe the formation of an aqueous $LiBr$ solution, when solid $LiBr$ dissolves in water.

Water is a polar solvent and carbon tetrachloride $\left(CC{l}_4\right)$ is a nonpolar solvent. In which solvent is each of the following, which is found or used in the body, more likely to be soluble?

a. $CaC{O}_3$ (calcium supplement), ionic

b. retinol (vitamin A), nonpolar

c. sucrose (table sugar), polar

d. cholesterol (lipid), nonpolar

Water is a polar solvent and hexane $C_6{H}_{14}$ is a nonpolar solvent. In which solvent is each of the following, which is found or used in the body, more likely to be soluble?

a. vegetable oil, nonpolar

b. oleic acid (lipid), nonpolar

c. niacin (vitamin $B_3$), polar

d. $FeS{O}_4$ (iron supplement), ionic

$KF$ is a strong electrolyte, and $HF$ is a weak electrolyte. How is the solution of $KF$ different from that of $HF$?

$NaOH$ is a strong electrolyte, and $C{H}_{3}OH$ is a nonelectrolyte. How is the solution of $NaOH$ different from that of $C{H}_{3}OH$ ?

Write a balanced equation for the dissociation of each of the following strong electrolytes in water:

a.  $KCl$

b. $CaC{l}_2$

c. $K_{3}P{O}_4$

d. $Fe{\left(N{O}_3\right)}_3$

Write a balanced equation for the dissociation of each of the following strong electrolytes in water:

a. $LiBr$

b. $NaN{O}_3$

c. $CuC{l}_2$

d. $K_{2}C{O}_3$

Indicate whether aqueous solutions of each of the following solutes contain only ions, only molecules, or mostly molecules and a few ions:

a. Acetic acid, $H{C}_2{H}_3{O}_2$, a weak electrolyte.

b. $NaBr$, a strong electrolyte.

c. fructose, $C_6{H}_{12}{O}_6$, a nonelectrolyte.

Indicate whether aqueous solutions of each of the following solutes contain only ions, only molecules, or mostly molecules and a few ions:

a. $N{H}_{4}Cl$, a strong electrolyte.

b. ethanol, $C_2{H}_{6}O$, a nonelectrolyte.

c. $HCN$, hydrocyanic acid, a weak electrolyte.

Classify the solute represented in each of the following equations as a strong, weak, or nonelectrolyte:

a. ${\mathrm{K}}_2{\mathrm{SO}}_4\left(s\right)\stackrel{{\mathrm{H}}_2\mathrm{O}}{⟶}2{ \mathrm{K}}^{+}\left(aq\right)+{\mathrm{SO}}_4^{2-}\left(aq\right)$

b. ${\mathrm{NH}}_3\left(g\right)+{\mathrm{H}}_2\mathrm{O}\left(l\right)\rightleftarrows {\mathrm{NH}}_4^{+}\left(aq\right)+{\mathrm{OH}}^{-}\left(aq\right)$

c. ${\mathrm{C}}_6{\mathrm{H}}_{12}{\mathrm{O}}_6\left(s\right)\stackrel{{\mathrm{H}}_2\mathrm{O}}{⟶}{\mathrm{C}}_6{\mathrm{H}}_{12}{\mathrm{O}}_6\left(aq\right)$

Classify the solute represented in each of the following equations as a strong, weak, or nonelectrolyte:

a. ${\mathrm{CH}}_4\mathrm{O}\left(l\right)\stackrel{{\mathrm{H}}_2\mathrm{O}}{⟶} {\mathrm{CH}}_4\mathrm{O}\left(aq\right)$

b. ${\mathrm{MgCl}}_2\left(s\right)\stackrel{{\mathrm{H}}_2\mathrm{O}}{⟶}{\mathrm{Mg}}^{2+}\left(aq\right)+2{\mathrm{Cl}}^{-}\left(aq\right)$

c. $\mathrm{HClO}\left(aq\right)\stackrel{{\mathrm{H}}_2\mathrm{O}}{\rightleftarrows }{\mathrm{H}}^{+}\left(aq\right)+{\mathrm{ClO}}^{-}\left(aq\right)$

Calculate the number of equivalents in each of the following: 

a. $1\text{ mole of }{\mathrm{K}}^{+}$

b. ${\text{2 moles of OH}}^{-}$

c. $1{\text{ mole of Ca}}^{2+}$

d. ${{\text{3 moles of CO}}_3}^{2-}$

Calculate the number of equivalents in each of the following:

a. $1{\text{ mole of Mg}}^{2+}$

b. ${\text{0.5 mole of H}}^{+}$

c. ${\text{4 moles of Cl}}^{-}$

d. ${\text{2 moles of Fe}}^{3+}$

An intravenous saline solution contains $154 mEq/L$ each of $N{a}^{+}$and $C{l}^{-}$. How many moles each of $N{a}^{+}$and $C{l}^{-}$ are in $1.00 L$ of the saline solution?

An intravenous solution to replace potassium loss contains $40 mEq/L$ each of $K^{+}$ and $C{l}^{-}$. How many moles each of $K^{+}$ and $C{l}^{-}$ are in $1.5 L$ of the solution?

An intravenous solution contains $40mEq/L$ of $C{l}^{-}$and $15 mEq/ L$ of $HP{O_4}^{2-}$. If $N{a}^{+}$ is the only cation in the solution, what is the $N{a}^{+}$concentration, in milliequivalents per liter?

A Ringer's solution contains the following concentrations $(mEq/L)$ of cations: $N{a}^{+ }147, K^{+} 4, and C{a}^{2+} 4.$ If $C{l}^{-}$is the only anion in the solution, what is the $C{l}^{-}$ concentration, in milliequivalents per liter?

When Michelle's blood was tested, the chloride level was $0.45 g/dL.$

a. What is this value in milliequivalents per liter?

b. According to Table $9.6$, is this value above, below, or within the normal range?

After dialysis, the level of magnesium in Michelle's blood was $0.0026g/dL.$

a. What is this value in milliequivalents per liter?

b. According to Table $9.6$, is this value above, below, or within the normal range?

State whether each of the following refers to a saturated or an unsaturated solution:

a. A crystal added to a solution does not change in size.

b. A sugar cube completely dissolves when added to a cup of coffee.

c. A uric acid concentration of $4.6 mg/100 mL$ in the kidney does not cause gout.

State whether each of the following refers to a saturated or an unsaturated solution:

a. A spoonful of salt added to boiling water dissolves.

b. A layer of sugar forms on the bottom of a glass of tea as ice is added.

c. A kidney stone of calcium phosphate forms in the kidneys when urine becomes concentrated.

Determine whether each of the following solutions will be saturated or unsaturated at ${20}^{\circ }C$ :

a. adding $25 g$ of $KCl$ to $100 g$ of $H_{2}O$ 

b. adding $11 g$ of $NaN{O}_3$ to $25 g$ of $H_{2}O$

c. adding $400 g$ of sugar to $125 g$ of $H_{2}O$

Determine whether each of the following solutions will be saturated or unsaturated at ${50}^{\circ }C$ :

a. adding $25 g$ of $KCl$ to $50 g of H_{2}O$

b. adding $150 g of NaN{O}_3$ to $75 g of H_{2}O$

c. adding $80 g$ of sugar to $25 g of H_{2}O$

A solution containing $80 g of KCl$ in $200 g of H_{2}O$ at ${50}^{\circ }C$ is cooled to ${20}^{\circ }C$

a. How many grams of $KCl$ remain in solution at ${20}^{\circ }C$ ?

b. How many grams of solid $KCl$ crystallized after cooling?

Explain the following observations:

a. More sugar dissolves in hot tea than in iced tea.

b. Champagne in a warm room goes flat.

c. A warm can of soda has more spray when opened than a cold one.

Explain the following observations:

a. An open can of soda loses its "fizz" faster at room temperature than in the refrigerator.

b. Chlorine gas in tap water escapes as the sample warms to room temperature.

c. Less sugar dissolves in iced coffee than in hot coffee.

Predict whether each of the following ionic compounds is soluble in water:

a. $LiCl$

b. $PbS$

c. $BaC{O}_3$

d. $K_{2}O$

e. $Fe{\left(N{O}_3\right)}_3$

Predict whether each of the following ionic compounds is soluble in water:

a. $AgCl$

b. $KI$

c. $N{a}_{2}S$

d. $A{g}_{2}O$

e. $CaS{O}_4$

A solution containing $80 g of NaN{O}_3$ in $75 g of H_{2}O$ at ${50}^{\circ }C$ is cooled to ${20}^{\circ }C$ 

a. How many grams of $NaN{O}_3$ remain in solution at ${20}^{\circ }C$?

b. How many grams of solid $NaN{O}_3$ crystallized after cooling?

Calculate the mass percent $(m/m)$ for the solute in each of the following:

a. $25 g of KCl$ and $125 g of H_{2}O$

b. $12 g$ of sucrose and $225 g$ of tea solution.

c. $8.0 g of CaC{l}_2$ and $80.0 g of CaC{O}_2$ solution.

A mouthwash contains $22.5\% (v/v)$ alcohol. If the bottle of mouthwash contains $335 mL$, what is the volume, in milliliters, of alcohol?

What is the difference between a $5.00\% (m/m)$ glucose solution and a $5.00\% (m/v)$ glucose solution?

What is the difference between a $10.0\% (v/v)$ methanol $\left(C{H}_{4}O\right)$ solution and a $10.0\% (m/m)$ methanol solution?

Calculate the mass/volume percent $(m/v)$ for the solute in each of the following:

a. $75 g of N{a}_{2}S{O}_4$ in $250 mL$of $N{a}_{2}S{O}_4$ solution.

b. $39 g$ of sucrose in $335 mL$ of a carbonated drink.

Calculate the mass/volume percent $(m/v)$ for the solute in each of the following:

a. $2.50\mathrm{g}\text{ of }\mathrm{LiCl}$ in $40 mL of \mathrm{LiCl}$ solution.

b. $7.5 \mathrm{g}$ of casein in $20 mL$of low-fat milk.

Calculate the grams or milliliters of solute needed to prepare the following:

a.$\text{ 50 }\mathrm{g}\text{ of a }5.0\% ( \mathrm{m}/\mathrm{m}) \mathrm{KCl}$ solution.

b. $1250 \mathrm{mL}\text{ of a }4.0\% ( \mathrm{m}/\mathrm{v} ){\mathrm{NH}}_4\mathrm{Cl}$ solution.

c. $\text{ 250 }\mathrm{mL}\text{ of a }10.0\% (\mathrm{v}/\mathrm{v})$ acetic acid solution.

Calculate the grams or milliliters of solute needed to prepare the following:

a.$\text{ 150 }\mathrm{g}\text{ of a }40.0\mathrm{\%} (\mathrm{m}/\mathrm{m}) {\mathrm{LiNO}}_3$ solution.

b. $450 \mathrm{mL}\text{ of a }2.0\mathrm{\%} (\mathrm{m}/\mathrm{v}) \mathrm{KOH}$ solution.

c. $225 \mathrm{mL}\text{ of a }15\mathrm{\%} (\mathrm{v}/\mathrm{v})$ isopropyl alcohol solution.

A bottle of champagne is $11\% (v/v)$ alcohol. If there are $750 mL$ of champagne in the bottle, what is the volume, in milliliters, of alcohol?

For each of the following solutions, calculate the:

a. grams of $25\% (m/m) LiN{O}_3$ solution that contains $5.0 g of LiN{O}_3.$

b. milliliters of $10.0\% (m/v) KOH$ solution that contains $40.0 g of KOH.$

c. milliliters of $10.0\% (v/v)$ formic acid solution that contains $20.0 mL$ of formic acid.

For each of the following solutions, calculate the:

a. grams of $2.0\% (m/m) NaCl$ that contains $7.50 g of NaCl.$

b. milliliters of $25\% (m/v) NaF$ solution that contains $4.0 g of NaF.$

c. milliliters of $8.0\% (v/v)$ ethanol solution that contains $20.0 mL$ of ethanol.

Calculate the molarity of each of the following:

a. $2.00$ moles of glucose in $4.00 L$ of a glucose solution.

b. $4.00 g of KOH$ in $2.00 L of a KOH$ solution.

c. $5.85 g of NaCl$ in $400 mL of a NaCl$ solution.

Calculate the molarity of each of the following:

a. $0.500$ mole of glucose in a $0.200 L$ of a glucose solution.

b. $73.0 g of HCl$ in a $2.00 L of HCl$ solution.

c. $30.0 g of NaOH$ in $350 mL of NaOH$ solution.

A patient receives $100 mL of 20\% (m/v)$ mannitol solution every hour.

a. How many grams of mannitol are given in $1 h$?

b. How many grams of mannitol does the patient receive in ?

A patient receives $250 mL of a 4.0\% (m/v)$ amino acid solution twice a day.

a. How many grams of amino acids are in $250 mL$ of solution?

b. How many grams of amino acids does the patient receive in $1$ day?

A patient needs $100 g$ of glucose in the next $12 h$. How many liters of a $5\% (m/v)$ glucose solution must be given?

A patient received $2.0 g of NaCl$ in $8 h$. How many milliliters of a $0.90\% (m/v)$$NaCl$ (saline) solution were delivered?