Aqueous Stoichiometry and Solution Concentrations

Vocabulary flashcards covering solution concentration, acid-base titrations, redox stoichiometry, and mass percentage problems from Examples 4.13, 4.14, 4.77, 4.92, and 4.159.

Neutralization Reaction of Sulfuric Acid and Sodium Hydroxide

The balanced chemical equation represented by $H_2SO_4(aq) + 2NaOH(aq) \rightarrow 2H_2O(l) + Na_2SO_4(aq)$.

Equivalence Volume of $NaOH$ (Example 4.13)

$49.0\,\text{mL}$, which is the volume of $0.250\,\text{M}\ NaOH$ required to completely neutralize $35.0\,\text{mL}$ of $0.175\,\text{M}\ H_2SO_4$.

Neutralization Reaction of Hydrochloric Acid and Sodium Hydroxide

The titration reaction represented by $HCl(aq) + NaOH(aq) \rightarrow H_2O(l) + NaCl(aq)$, exhibiting a $1:1$ mole ratio.

Molar Mass of $HCl$

$36.5\,\text{g/mol}$, the molar mass used to determine the mass of hydrochloric acid from titration data.

Mass of $HCl$ (Example 4.14)

$0.0338\,\text{g}$, the mass of hydrochloric acid calculated from the titration with $4.47\,\text{mL}$ of $0.207\,\text{M}\ NaOH$.

Molar Mass of $Na_2Cr_2O_7$

$261.97\,\text{g/mol}$, the molar mass of sodium dichromate used in preparing aqueous solutions.

Mass of $Na_2Cr_2O_7$ (Example 4.77)

$0.86\,\text{g}$, the mass of sodium dichromate needed in a $100.0\text{-mL}$ volumetric flask to prepare a $0.033\,\text{M}\ Na_2Cr_2O_7$ solution.

Redox Reaction of $FeSO_4$ and $KMnO_4$

The balanced equation $10FeSO_4(aq) + 2KMnO_4(aq) + 8H_2SO_4(aq) \rightarrow 5Fe_2(SO_4)_3(aq) + 2MnSO_4(aq) + K_2SO_4(aq) + H_2O(l)$.

Molar Mass of $FeSO_4$

$151.91\,\text{g/mol}$, the molar mass of iron(II) sulfate used to convert grams to moles in redox calculations.

Stoichiometric Ratio of $FeSO_4$ to $KMnO_4$

$10\,\text{mol}\ FeSO_4$ to $2\,\text{mol}\ KMnO_4$ (a $5:1$ molar ratio).

Volume of $0.250\,\text{M}\ KMnO_4$ (Example 4.92)

$18.7\,\text{mL}$, the volume needed to react completely with $3.55\,\text{g}$ of $FeSO_4$.

Aluminum Sulfate Synthesis Reaction

The chemical equation represented by $2Al(s) + 3H_2SO_4(aq) \rightarrow Al_2(SO_4)_3(aq) + 3H_2(g)$, used to produce $37.4\,\text{g}$ of aluminum sulfate.

Sulfuric Acid Solution Specifications (Example 4.159)

A solution defined by a density of $1.104\,\text{g/mL}$ and containing $15.0\%\ H_2SO_4$ by mass.