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Chapter 4: Problem 16

Specify what ions are present upon dissolving each of the following substances in water: (a) \(\mathrm{MgI}_{2}\), (b) \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3},\) (c) \(\mathrm{HClO}_{4}\), (d) \(\mathrm{NaCH}_{3} \mathrm{COO}\)

Short Answer

Expert verified
Upon dissolving the given substances in water, the following ions are present: (a) \(\mathrm{MgI}_{2}\): Magnesium ions (\(\mathrm{Mg}^{2+}\)) and iodide ions (I⁻) (b) \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\): Aluminum ions (\(\mathrm{Al}^{3+}\)) and nitrate ions (NO₃⁻) (c) \(\mathrm{HClO}_{4}\): Hydrogen ions (\(\mathrm{H}^{+}\)) and perchlorate ions (ClO₄⁻) (d) \(\mathrm{NaCH}_{3} \mathrm{COO}\): Sodium ions (\(\mathrm{Na}^{+}\)) and acetate ions (CH₃COO⁻)

Step by step solution

01

(a) Dissociating MgI₂

When magnesium iodide (\(\mathrm{MgI}_{2}\)) is dissolved in water, it dissociates into one magnesium ion (Mg²⁺) and two iodide ions (I⁻): \[\mathrm{MgI}_{2} \rightarrow \mathrm{Mg}^{2+} + 2\mathrm{I}^{-}\]
02

Ions Present in MgI₂ Solution

In the case of a \(\mathrm{MgI}_{2}\) solution, we have magnesium ions (\(\mathrm{Mg}^{2+}\)) and iodide ions (I⁻). -----
03

(b) Dissociating Al(NO₃)₃

When aluminum nitrate (\(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\)) is dissolved in water, it dissociates into one aluminum ion (Al³⁺) and three nitrate ions (NO₃⁻): \[\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3} \rightarrow \mathrm{Al}^{3+} + 3\mathrm{NO}_{3}^{-}\]
04

Ions Present in Al(NO₃)₃ Solution

In the case of an \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) solution, we have aluminum ions (\(\mathrm{Al}^{3+}\)) and nitrate ions (NO₃⁻). -----
05

(c) Dissociating HClO₄

When perchloric acid (\(\mathrm{HClO}_{4}\)) is dissolved in water, it dissociates into one hydrogen ion (H⁺) and one perchlorate ion (ClO₄⁻): \[\mathrm{HClO}_{4} \rightarrow \mathrm{H}^{+} + \mathrm{ClO}_{4}^{-}\]
06

Ions Present in HClO₄ Solution

In the case of an \(\mathrm{HClO}_{4}\) solution, we have hydrogen ions (\(\mathrm{H}^{+}\)) and perchlorate ions (ClO₄⁻). -----
07

(d) Dissociating NaCH₃COO

When sodium acetate (\(\mathrm{NaCH}_{3} \mathrm{COO}\)) is dissolved in water, it dissociates into one sodium ion (Na⁺) and one acetate ion (CH₃COO⁻): \[\mathrm{NaCH}_{3} \mathrm{COO} \rightarrow \mathrm{Na}^{+} + \mathrm{CH}_{3}\mathrm{COO}^{-}\]
08

Ions Present in NaCH₃COO Solution

In the case of a \(\mathrm{NaCH}_{3} \mathrm{COO}\) solution, we have sodium ions (\(\mathrm{Na}^{+}\)) and acetate ions (CH₃COO⁻).

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Most popular questions from this chapter

(a) How many grams of solute are present in \(15.0 \mathrm{~mL}\) of \(0.736 \mathrm{M} \mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7} ?\) (b) If \(14.00 \mathrm{~g}\) of \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\) is dissolved in enough water to form \(250 \mathrm{~mL}\) of solution, what is the molarity of the solution? (c) How many milliliters of \(0.0455 \mathrm{M} \mathrm{CuSO}_{4}\) contain \(3.65 \mathrm{~g}\) of solute?

If you want to double the concentration of a solution, how could you do it? [Section 4.5\(]\)

(a) How would you prepare \(175.0 \mathrm{~mL}\) of \(0.150 \mathrm{M} \mathrm{AgNO}_{3}\) solution starting with pure \(\mathrm{AgNO}_{3} ?\) (b) An experiment calls for you to use \(100 \mathrm{~mL}\) of \(0.50 \mathrm{M} \mathrm{HNO}_{3}\) solution. All you have available is a bottle of \(3.6 \mathrm{M} \mathrm{HNO}_{3} .\) How would you prepare the desired solution?

A \(0.5895-\mathrm{g}\) sample of impure magnesium hydroxide is dissolved in \(100.0 \mathrm{~mL}\) of \(0.2050 \mathrm{M} \mathrm{HCl}\) solution. The excess acid then needs \(19.85 \mathrm{~mL}\) of \(0.1020 \mathrm{M} \mathrm{NaOH}\) for neutralization. Calculate the percent by mass of magnesium hydroxide in the sample, assuming that it is the only substance reacting with the HCl solution.

The distinctive odor of vinegar is due to acetic acid, \(\mathrm{CH}_{3} \mathrm{COOH},\) which reacts with sodium hydroxide in the following fashion: $$\mathrm{CH}_{3} \mathrm{COOH}(a q)+\mathrm{NaOH}(a q) \longrightarrow$$ If \(3.45 \mathrm{~mL}\) of vinegar needs \(42.5 \mathrm{~mL}\) of \(0.115 \mathrm{M} \mathrm{NaOH}\) to reach the equivalence point in a titration, how many grams of acetic acid are in a \(1.00-\) qt sample of this vinegar?
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