Calculate the molarity of a solution prepared by dissolving $5$ grams of NaCl $($molecular weight $=58\mathrm{.}44$ g$/$mol$)$ in $250$ mL of water.

Determine the number of moles of CO$$ produced when $2$ moles of C$$H$$ are completely combusted in excess oxygen.

Calculate the pH of a $0\mathrm{.}01$ M HCl solution.

Determine the empirical formula of a compound that contains $40\%$ carbon, $6\mathrm{.}7\%$ hydrogen, and $53\mathrm{.}3\%$ oxygen by mass.

Calculate the enthalpy change for the reaction: N$($g$)+3$H$($g$)2$NH$($g$),$ given the bond enthalpies: N$$N $=945$ kJ$/$mol$,$ H$-$H $=436$ kJ$/$mol$,$ and N$-$H $=391$ kJ$/$mol$.$

Determine the concentration of OH$$ ions in a solution with a pH of $3\mathrm{.}5.$

Calculate the volume of $0\mathrm{.}1$ M H$$SO$$ required to neutralize $50$ mL of $0\mathrm{.}2$ M NaOH.

Determine the percent yield if $5\mathrm{.}0$ grams of product is obtained from a reaction that has a theoretical yield of $6\mathrm{.}5$ grams.

Calculate the freezing point depression of a solution containing $1$ mole of NaCl in $1$ kg of water $($Kf for water $=1\mathrm{.}86$C kg$/$mol$).$

Determine the equilibrium constant, Kc$,$ for the reaction: H$($g$)+$ I$($g$)2$HI$($g$),$ given the equilibrium concentrations: $[$H$]=0\mathrm{.}2$ M$,[$I$]=0\mathrm{.}1$ M$,$ and $[$HI$]=0\mathrm{.}8$ M$.$

Calculate the wavelength of light emitted when an electron in a hydrogen atom transitions from the n $=4$ level to the n $=2$ level $($Rydberg constant, R $=1\mathrm{.}097$ x $10$ m$).$

Determine the mass of CaCO$$ that will react with $25$ mL of $1$ M HCl solution.

Calculate the standard Gibbs free energy change $($G$)$ for the reaction: $2$SO$($g$)+$ O$($g$)2$SO$($g$),$ given $$H$=-198$ kJ and $$S$=-188$ J$/$K at $298$ K$.$

Determine the concentration of Ag$$ ions in a saturated solution of AgCl, given Ksp $=1\mathrm{.}8$ x $10.$

Calculate the energy required to vaporize $100$ grams of water at $100$C $($latent heat of vaporization for water $=2260$ J$/$g$).$

Determine the number of electrons transferred in the redox reaction: MnO$+8$H$+5$Fe$^2$ Mn$^2+5$Fe$^3+4$H$$O$.$

Calculate the osmotic pressure of a $0\mathrm{.}5$ M glucose solution at $25$C $($R $=0\mathrm{.}0821$ L$$atm$/$mol$$K$).$

Determine the oxidation state of sulfur in H$$SO$.$

Calculate the enthalpy change for the reaction: CH$($g$)+2$O$($g$)$ CO$($g$)+2$H$$O$($g$),$ given the enthalpies of formation: $$Hf$($CH$)=-74\mathrm{.}8$ kJ$/$mol$,$Hf$($CO$)=-393\mathrm{.}5$ kJ$/$mol$,$ and $$Hf$($H$$O$)=-241\mathrm{.}8$ kJ$/$mol$.$

Determine the mass of KCl required to prepare $250$ mL of a $0\mathrm{.}5$ M solution.

Calculate the ionization energy of an atom if the energy required to remove an electron is $1\mathrm{.}96$ x $10$ J$.$

Determine the molality of a solution prepared by dissolving $10$ grams of NaOH in $500$ grams of water.

Calculate the standard cell potential $($E$$cell$)$ for the galvanic cell: Zn$($s$)|$ Zn$^2($aq$)||$ Cu$^2($aq$)|$ Cu$($s$),$ given E$($Zn$^2/$Zn$)=-0\mathrm{.}76$ V and E$($Cu$^2/$Cu$)=0\mathrm{.}34$ V$.$

Determine the rate constant for a first$-$order reaction with a half$-$life of $15$ minutes.

Calculate the mass percent of oxygen in K$$Cr$$O$($molecular weight $=294\mathrm{.}18$ g$/$mol$).$

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