Chapter 7
Chemical Principles in the Laboratory · 2 exercises
Problem 1
A sample containing \(0.221 \mathrm{g} \mathrm{Cl}^{-}\) is dissolved in \(50.0 \mathrm{mL}\) water. a. How many moles of \(\mathrm{Cl}^{-}\) ion are in the solution? b. What is the molarity of the \(\mathrm{Cl}^{-}\) ion in the solution? \(\left(M_{\mathrm{Cl}^{-}}=n_{\mathrm{Cl}^{-}} / V_{\text {soln }}\right)\)
4 step solution
Problem 2
A solid chloride sample weighing 0.3147 g required \(43.75 \mathrm{mL}\) of \(0.05273 \mathrm{M}\) AgNO, to reach the \(\mathrm{Ag}_{2} \mathrm{CrO}_{4}\) end point. a. How many moles \(\mathrm{Cl}^{-}\) ion were present in the sample? (Use Eqs. 2 and \(3 .\) ) b. How many grams Cl- ion were present? (Use Eq. 4.) c. What was the mass percent \(\mathrm{Cl}^{-}\) ion in the sample? (Use Eq. 5.)
3 step solution