An aqueous solution contains 1.2 mM of total ions. (a) If the solution is NaCl(aq), what is the concentration of chloride ion?

An aqueous solution contains 1.2 mM of total ions. (b) If the solution is FeCl3(aq), what is the concentration of chloride ion?

Which data set, of the two graphed here, would you expect to observe from a titration like that shown in Figure 4.18?

You are titrating an acidic solution with a basic one, and just realized you forgot to add the indicator that tells you when the equivalence point is reached. In this titration, the indicator turns blue at the equivalence point from an initially colorless solution. You quickly grab a bottle of indicator and add some to your titration beaker, and the whole solution turns dark blue. What do you do now?

State whether each of the following statements is true or false. Justify your answer in each case. (a) Electrolyte solutions conduct electricity because electrons are moving through the solution.

State whether each of the following statements is true or false. Justify your answer in each case. (b) If you add a nonelectrolyte to an aqueous solution that already contains an electrolyte, the electrical conductivity will not change.

(a) Do colloids made only of gases exist? Why or why not?

(b) In the 1850s, Michael Faraday prepared ruby-red

colloids of gold nanoparticles in water that are still stable

today. These brightly colored colloids look like solutions.

What experiment(s) could you do to determine whether a

given colored preparation is a solution or colloid?

Choose the best answer: A colloidal dispersion of one liquid

in another is called (a) a gel, (b) an emulsion, (c) a foam,

(d) an aerosol

We have learned in this chapter that many ionic solids dissolve in water as strong electrolytes; that is, as separated ions in solution. Which statement is most correct about this process? (a) Water is a strong acid and therefore is good at dissolving ionic solids. (b) Water is good at solvating ions because the hydrogen and oxygen atoms in water molecules bear partial charges. (c) The hydrogen and oxygen bonds of water are easily broken by ionic solids.

Would you expect that an anion would be physically closer to the oxygen or to the hydrogens of water molecules that surround it in solution?

Ignoring protolysis reactions (i.e. proton transfer reaction), specify what ions are present in a solution upon dissolving each of the following substances in water: (a)Li₂CO₃

Ignoring protolysis reactions (i.e. proton transfer reaction), specify what ions are present in a solution upon dissolving each of the following substances in water: (b)(NH₄)₃PO₄ (c) Na₂Cr₂O₇ (d) NaPF₆.

Specify what ions are present upon dissolving each of the following substances in water: (a) MgI₂

Specify what ions are present upon dissolving each of the following substances in water: (b) K₂CO₃

Specify what ions are present upon dissolving each of the following substances in water: (c) HClO₄

Specify what ions are present upon dissolving each of the following substances in water: (d) NaCH₃COO

Formic acid, HCOOH, is a weak electrolyte. What solutes are present in an aqueous solution of this compound?

Formic acid, HCOOH, is a weak electrolyte. Write the chemical equation for the ionization of HCOOH.

Acetone, CH₃COCH₃, is a nonelectrolyte; hypochlorous acid, HClO, is a weak electrolyte; and ammonium chloride, NH₄Cl, is a strong electrolyte. (a) What are the solutes present in aqueous solutions of each compound? What solute particles are present in an aqueous solution of CH₃COCH₃?

Acetone, CH3COCH3, is a nonelectrolyte; hypochlorous acid, HClO, is a weak electrolyte; and ammonium chloride, NH4Cl, is a strong electrolyte. (a) What are the solutes present in aqueous solutions of each compound? What solute particles are present in an aqueous solution of HClO?

Acetone, CH3COCH3, is a nonelectrolyte; hypochlorous acid, HClO, is a weak electrolyte; and ammonium chloride, NH4Cl, is a strong electrolyte. (a) What are the solutes present in aqueous solutions of each compound? What solute particles are present in an aqueous solution of NH4Cl?

Acetone, CH₃COCH₃, is a nonelectrolyte; hypochlorous acid, HClO, is a weak electrolyte; and ammonium chloride, NH₄Cl, is a strong electrolyte. (b) If 0.1 mol of each compound is dissolved in solution, which one contains 0.2 mol of solute particles, which contains 0.1 mol of solute particles, and which contains somewhere between 0.1 and 0.2 mol of solute particles?

Using solubility guidelines, predict whether each of the following compounds is soluble or insoluble in water: (a) MgBr₂ (b) NH₄OH (c) Ni(CH₃COO)₂ (d) AgNO₃ (e) FeCO₃.

Predict whether each of the following compounds is soluble in water: (a) MgS (b) Cr(OH)₃ (c) ZnCl₂ (d) Pb₃(PO₄)₂ (e) Sr(CH₃COO)₂.

Will precipitation occur when the following solutions are mixed? If so, write a balanced chemical equation for the reaction. (a) Ca(CH₃COO)₂ and NaOH (b) K₂CO₃ and NH₄NO₃, (c) Na₂S and FeCl₃.

Identify the precipitate (if any) that forms when the following solutions are mixed, and write a balanced equation for each reaction. (a) NH₄I and CuCl₂ (b) LiOH and MnCl₂ (c) K₃PO₄ and CoSO₄

Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed? (a) potassium carbonate and magnesium sulfate