Q: Which of the following is the correct formula for calculating the molarity of a solution?

$\text{Molarity} = \frac{\text{moles of solute}}{\text{liters of solution}}$

Question 1

Which of the following statements best explains why ionic compounds are generally more soluble in water than in hexane?

Accepted Answer

Water is a polar solvent and can stabilize ions through ion-dipole interactions, while hexane is nonpolar and cannot.

Question 2

A student mixes 0.10 mol of acetic acid ($CH_3COOH$) with 0.10 mol of sodium acetate ($CH_3COONa$) in 1.0 L of water. What type of solution is formed?

Accepted Answer

A buffer solution

Question 3

Which equation correctly relates the equilibrium constant $K$ to the Gibbs free energy change $\Delta G^\circ$ at standard conditions?

Accepted Answer

$\Delta G^\circ = -RT \ln K$

Question 4

A reaction has an activation energy of 50 kJ/mol. If the temperature is increased, what will happen to the rate constant $k$ according to the Arrhenius equation?

Accepted Answer

The rate constant $k$ will increase.

Question 5

Which of the following best describes the effect of adding a catalyst to a chemical reaction?

Accepted Answer

It lowers the activation energy, increasing the reaction rate without being consumed.

Question 6

A solution is prepared by dissolving 0.5 mol of NaCl in 1.0 L of water. What is the van 't Hoff factor $i$ for NaCl in this solution?

Accepted Answer

$i = 2$

Question 7

Which of the following is the correct expression for the equilibrium constant $K_{sp}$ for the dissolution of $Ag_2CO_3$?

Accepted Answer

$K_{sp} = [Ag^+]^2[CO_3^{2-}]$

Question 8

A buffer solution is made by mixing equal concentrations of a weak acid and its conjugate base. What will happen to the pH if a small amount of strong acid is added?

Accepted Answer

The pH will decrease slightly, but the buffer will resist large changes.

Question 9

Which of the following is true about the entropy change $\Delta S$ for the melting of ice at 0°C?

Accepted Answer

$\Delta S$ is positive because the system becomes more disordered.

Question 10

Which of the following best describes the effect of increasing the concentration of reactants on the rate of a chemical reaction?

Accepted Answer

The reaction rate increases because more collisions occur per unit time.

Question 11

A student titrates 25.0 mL of 0.100 M $HCl$ with 0.100 M $NaOH$. What is the pH at the equivalence point?

Accepted Answer

pH = 7

Question 12

Which of the following is the correct formula for calculating the cell potential $E_{cell}$ under non-standard conditions using the Nernst equation?

Accepted Answer

$E_{cell} = E_{cell}^\circ - \frac{0.0592}{n} \log Q$

Question 13

Which statement best describes the difference between nuclear fission and nuclear fusion?

Accepted Answer

Fission splits heavy nuclei into smaller fragments, while fusion combines light nuclei to form heavier nuclei.

Question 14

Which of the following is the correct expression for the rate law of a reaction that is first order in $A$ and second order in $B$?

Accepted Answer

$	ext{rate} = k[A][B]^2$

Question 15

Which of the following is a colligative property?

Accepted Answer

Boiling point elevation

Question 16

A voltaic (Galvanic) cell is constructed using $Zn$ and $Cu$ electrodes. Which half-cell undergoes oxidation?

Accepted Answer

The $Zn$ electrode

Question 17

Which of the following best describes the coordination number of a metal ion in a complex?

Accepted Answer

The number of ligand atoms directly bonded to the metal ion

Question 18

Which of the following is the correct formula for calculating the molarity of a solution?

Accepted Answer

$	ext{Molarity} = \frac{	ext{moles of solute}}{	ext{liters of solution}}$

Question 19

Which of the following is true about the standard reduction potential ($E^\circ$) of a half-cell?

Accepted Answer

It is measured relative to the standard hydrogen electrode, which is assigned a potential of 0 V.

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