EConcentrated hydrochloric acid solution is 37.0 % HC and has a density of 1.19 g / mL. A dilut

step 1 So in this problem, first of all, this original solution is a density of 1 .19 grams for 1 milli

EConcentrated hydrochloric acid solution is 37.0 % HC and...

EConcentrated hydrochloric acid solution is $37.0 \% \mathrm{HC}$ and has a density of $1.19 \mathrm{~g} / \mathrm{mL}$. A dilute solution of $\mathrm{HCl}$ is prepared by diluting $4.50 \mathrm{~mL}$ of this concentrated $\mathrm{HCl}$ solution to $100.00 \mathrm{~mL}$ with water. Then $10.0 \mathrm{~mL}$ of this dilute $\mathrm{HCl}$ solution reacts with an $\mathrm{AgNO}_{3}$ solution according to the following reaction: $$ \mathrm{HCl}(\mathrm{aq})+\mathrm{AgNO}_{3}(\mathrm{aq}) \longrightarrow \mathrm{HNO}_{3}(\mathrm{aq})+\mathrm{AgCl}(\mathrm{s}) $$ How many milliliters of $0.1105 \mathrm{M} \mathrm{AgNO}_{3}$ solution is reauired to precipitate all of the chloride as $\mathrm{AgCl}(\mathrm{s})$ ?

EConcentrated hydrochloric acid solution is $37.0 \% \mathrm{HC}$ and has a density of $1.19 \mathrm{~g} / \mathrm{mL}$. A dilute solution of $\mathrm{HCl}$ is prepared by diluting $4.50 \mathrm{~mL}$ of this concentrated $\mathrm{HCl}$ solution to $100.00 \mathrm{~mL}$ with water. Then $10.0 \mathrm{~mL}$ of this dilute $\mathrm{HCl}$ solution reacts with an $\mathrm{AgNO}_{3}$ solution according to the following reaction:
$$
\mathrm{HCl}(\mathrm{aq})+\mathrm{AgNO}_{3}(\mathrm{aq}) \longrightarrow \mathrm{HNO}_{3}(\mathrm{aq})+\mathrm{AgCl}(\mathrm{s})
$$
How many milliliters of $0.1105 \mathrm{M} \mathrm{AgNO}_{3}$ solution is reauired to precipitate all of the chloride as $\mathrm{AgCl}(\mathrm{s})$ ?

Key Concepts

Dilution

Dilution is the process of reducing the concentration of a solute in a solution, usually by adding more solvent. The key point in dilutions is that the number of moles of solute remains unchanged, even though the total volume increases. Understanding dilution allows one to calculate the new concentration of the solution after the volume change.

Reaction Stoichiometry

Reaction stoichiometry involves using the coefficients from a balanced chemical equation to determine the quantitative relationships between reactants and products. It is essential for calculating the amounts of reagents needed or produced in a reaction. In the context of precipitations or titrations, stoichiometry is used to determine the volume or concentration of a titrant required to react completely with a given amount of analyte.

Molarity

Molarity is a concentration unit defined as the number of moles of solute per liter of solution. It provides a simple and practical way to quantify the concentration of a solution and is directly used to relate the amount of reactant in a chemical reaction according to balanced chemical equations.

Unit Conversion

Unit conversion involves translating a quantity from one unit system to another, such as converting milliliters to grams or grams to moles using molar mass. This skill is fundamental in chemistry for ensuring that quantities are calculated with consistent units, especially when densities, volumes, and masses are all involved.

Density

Density is the mass per unit volume of a substance and is essential for converting between the volume of a solution and its mass. In the context of solution chemistry, knowing the density of a concentrated solution allows you to determine the total mass of solution contained in a given volume, which can then be used in conjunction with the mass percent to compute the mass (and ultimately the moles) of a solute.

Mass Percent Concentration

Mass percent concentration describes the percentage by mass of a solute present in a solution. It tells you how many grams of the solute are contained in 100 grams of the solution. This concept is crucial for converting percentages to actual masses when dealing with concentrated solutions and is widely used in preparing solutions of a desired composition.

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