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

a. 10.0 g of NaCl and 100.0 g of H₂O

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

Water is a polar solvent and carbon tetrachloride (CCl₄) 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?

d. cholesterol (lipid), nonpolar

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

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

d. Fe(NO₃)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, HC₂H₃O₂, a weak electrolyte

Indicate whether aqueous solutions of each of the following solutes contain only ions, only molecules, or mostly molecules and a few ions: c. fructose, C₆H₁₂O₆, a nonelectrolyte

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

b. NaBr, a strong electrolyte

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

a. $K_{2}S{O}_4\left(aq\right)\stackrel{H_{2}O}{\to }2K^{+}\left(aq\right)+S{O}_4^{2-}\left(aq\right)$

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

b. NH₃(g) + H₂O(l) ⇌ NH₄⁺(aq) + OH^–(aq)

Calculate the number of equivalents in each of the following:

d. 3 moles of CO₃^2–

Calculate the number of equivalents in each of the following:

d. 2 moles of Fe³⁺

An intravenous saline solution contains 154 mEq/L each of Na⁺ and Cl^–. How many moles each of Na⁺ and Cl^– are in 1.00 L of the saline solution?

An intravenous solution contains 40. mEq/L of Cl^– and 15 mEq/L of HPO₄^2–. If Na⁺ is the only cation in the solution, what is the Na⁺ concentration, in milliequivalents per liter?

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

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.

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

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

A solution containing 80. g of KCl in 200. g of H₂O at 50 °C is cooled to 20 °C. a. How many grams of KCl remain in solution at 20 °C?

Explain the following observations:

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

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

c. BaCO₃

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

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

b. Kl

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 (CH₄O) 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 Na₂SO₄ in 250 mL of Na₂SO₄ solution

A mouthwash contains 22.5% (v/v) alcohol. If the bottle of mouthwash contains 355 mL, what is the volume, in milliliters, of alcohol?

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

c. 250. mL of a 10.0% (v/v) acetic acid solution

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

b. How many grams of mannitol does the patient receive in 12 h?

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?

Determine the final volume, in milliliters, of each of the following:

b. a 2.0% (m/v) LiCl solution prepared from 50.0 mL of a 10.0% (m/v) LiCl solution