You can purchase nitric acid in a concentrated form that is 70.3% HNO$_3$ by mass and has a density of 1.41 g/ mL. Describe exactly how you would prepare 1.15 L of 0.100 M HNO$_3$ from the concentrated solution

A sample of concentrated nitric acid has a density of 1.41 g/mL and contains 70.0% $HNO_3$ by mass. What mass (g) of $HNO_3$ is present per liter of solution?

A solution contains naphthalene ($C_{10}H_8$) dissolved in hexane ($C_6H_{14}$) at a concentration of 12.35% naphthalene by mass. Calculate the vapor pressure at 25$^{\circ} C$ of hexane above the solution. The vapor pressure of pure hexane at 25$^{\circ} C$ is 151 torr.

How did the rise of the counterculture lead to a generation gap?

Nitric acid is usually purchased in concentrated form with a $70.3 \% \mathrm{HNO}_3$ concentration by mass and a density of $1.41 \mathrm{~g} / \mathrm{mL}$. How much of the concentrated stock solution in milliliters should you use to make $2.5 \mathrm{~L}$ of $0.500 \mathrm{M} \mathrm{HNO}_3$ ?

Suppose a certain insect species lives only in a specific species of tree. It feeds off the sap of the tree and produces a chemical that protects the tree from certain fungi. What kind of relationship is this?

What are the common units for expressing solution concentration?

Silver nitrate solutions are often used to plate silver onto other metals. What is the maximum amount of silver (in grams) that can be plated out of 4.8 L of an $AgNO_3$ so luti on containing 3.4% Ag by mass? Assume that the density of the solution is 1.01 g/mL.

An aq ueo us NaCl so lution is made usin g 112 g of NaCl diluted to a total soluti on volume of 1.00 L. Calculate the molarity, rnolality, and mass percent of the solution. (Assume a density of 1.08 g/ mL for the solution .)

Events $E_1$ and $E_2$ are mutually exclusive if $E_1\cap E_2=\varnothing$.

To what volume should you dilute 50.0 mL of a 5.00 M KI solution so that 25.0 mL of the diluted solution contains 3.05 g of KI?

An aqueous solution containing 17.5 g of an unknown molecular (nonelectrolyte) compound in 100.0 g of water has a freezing point of - 1.8$^{\circ} \mathrm{C}$. Calculate the molar mass of the unknown compound.

How much of 5.0M nitric acid $(HNO_3)$, in milliliters, is needed to make 225 mL of 1.0M $HNO_3$?

Describe how to prepare each solution from the dry solute and the solvent. a. $1.00 \times 10^{2}$ mL of 0.500 M KCl b. $1.00 \times 10^{2}$ g of 0.500 m KCl c. $1.00 \times 10^{2}$ g of 5.0% KCl solution by mass