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Chapter 17: Problem 64

For each of the following slightly soluble salts, write the net ionic equation, if any, for reaction with a strong acid: (a) MnS, (b) \(P \mathrm{bF}_{2}\) (c) \(\mathrm{AuCl}_{3}\) (d) \(\mathrm{Hg}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\) (e) CuBr.

Short Answer

Expert verified
Net ionic equations: (a) \(\text{S}^{2-} + 2\text{H}^{+} \rightarrow \text{H}_2\text{S}\), (b) \(2\text{F}^{-} + 2\text{H}^{+} \rightarrow 2\text{HF}\), (c) No reaction, (d) \(\text{C}_2\text{O}_4^{2-} + 2\text{H}^{+} \rightarrow \text{H}_2\text{O} + \text{CO}_2\), (e) No reaction.

Step by step solution

01

Understand the reaction with a strong acid

For a slightly soluble salt to react with a strong acid, the salt must be able to produce ions that can react with the hydrogen ions from the acid, resulting in soluble products or gases. This usually involves the anion of the salt reacting with the hydrogen ion to form a soluble compound or release a gas.
02

Analyze MnS with a strong acid

MnS reacts with a strong acid to form Mn虏鈦� and H鈧係 gas, as the sulfide ions react with hydrogen ions: \[ \text{MnS(s) + 2H鈦�(aq) } \rightarrow \text{ Mn}^{2+}\text{(aq) + H鈧係(g)} \]. The net ionic equation is: \[ \text{S}^{2-}\text{(s) + 2H}^{+}\text{(aq) } \rightarrow \text{H}_2\text{S(g)} \].
03

Analyze PbF鈧� with a strong acid

For PbF鈧�, the reaction with a strong acid will lead to the formation of soluble Pb虏鈦� ions and HF gas if the product is less soluble or gaseous. The net ionic equation is: \[ \text{2F}^{-}\text{(s) + 2H}^{+}\text{(aq) } \rightarrow \text{2HF(g)} \].
04

Analyze AuCl鈧� with a strong acid

AuCl鈧� does not react with strong acids in a typical acid-base manner, as the chloride ions do not react with hydrogen ions to form gaseous or otherwise very insoluble products. Hence, no net ionic equation is applicable.
05

Analyze Hg鈧侰鈧侽鈧� with a strong acid

Hg鈧侰鈧侽鈧� reacts with strong acids, and the oxalate ion can react with hydrogen ions, producing soluble Hg ions and carbon dioxide gas. The net ionic equation is: \[ \text{C}_2\text{O}_4^{2-}\text{(s) + 2H}^{+}\text{(aq) } \rightarrow \text{H}_2\text{O(l) + CO}_2\text{(g)} \].
06

Analyze CuBr with a strong acid

CuBr does not react with strong acids in a way that would form a gas or a significantly more soluble product with the anion; therefore, no net ionic equation is applicable for this combination.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Slightly Soluble Salts
Slightly soluble salts are salts that do not dissolve well in water. They form a solid in the solution because only a small amount of the salt can dissolve to produce ions in the mix. When such salts do dissolve, even a little, they form ions that are part of the ionic lattice breaking into the solution.
These salts often play a role in chemical reactions, particularly when interacting with acids.
  • Common slightly soluble salts include MgCO鈧� (magnesium carbonate) and CaSO鈧� (calcium sulfate).
  • The extent of solubility for these salts is governed by the solubility product constant ( K_{sp} ), a measure of the solubility of a compound.
Understanding these aspects helps predict products when slightly soluble salts are mixed with other compounds like acids.
Acid-Base Reactions
Acid-base reactions involve the transfer of hydrogen ions ( H^{+} ) between reactants. When a slightly soluble salt interacts with a strong acid, a reaction can sometimes occur where the acid donates H^{+} ions to the anion from the salt.
This often leads to the formation of a more soluble product or gas, driving the reaction forward.
  • In these reactions, the anion from the salt often pairs with hydrogen ions to form gaseous compounds like CO_2 (carbon dioxide) in the case of oxalates.
  • This interaction can result in effervescence due to gas production.
  • Not all acid-salt combinations will result in a reaction as some do not form significantly more soluble or gaseous products.
Grasping the behavior of different ions in acid-base reactions helps in writing balanced net ionic equations.
Ionic Compounds
Ionic compounds consist of charged particles known as ions. They are generally formed when a metal reacts with a non-metal, leading to an ionic bond. These compounds often dissolve in water, dispersing the ions into the solution.
However, the extent of their solubility varies depending on the compound.
  • Ions such as Na^{+} and Cl^{-} separate and move freely in the solution when a salt like NaCl is dissolved.
  • Ionic bonds are strong electrostatic forces of attraction between positively charged cations (like Na^{+} ) and negatively charged anions (like Cl^{-} ).
Understanding ionic compounds is vital in chemistry, especially when predicting the outcomes of chemical reactions.
Solubility Rules
Solubility rules are a set of guidelines that help predict whether a salt will dissolve in water. These rules are crucial for determining the outcome of chemical reactions, especially involving ionic compounds and acids.
  • Most nitrate ( NO_3^{-} ) and acetate ( CH_3COO^{-} ) salts are soluble.
  • Sulfates ( SO_4^{2-} ) are generally soluble, except for those paired with barium, lead, mercury, and calcium.
  • Chlorides ( Cl^{-} ), bromides ( Br^{-} ), and iodides ( I^{-} ) are also mostly soluble, except when with silver, lead, and mercury.
Understanding these rules helps anticipate which salts are likely to dissolve, which are essential for mixing solutions and predicting reaction products effectively.

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Most popular questions from this chapter

(a) A \(0.1044-g\) sample of an unknown monoprotic acid requires \(22.10 \mathrm{~mL}\) of \(0.0500 \mathrm{M} \mathrm{NaOH}\) to reach the end point. What is the molar mass of the unknown? (b) As the acid is titrated, the \(\mathrm{pH}\) of the solution after the addition of \(11.05 \mathrm{~mL}\) of the base is \(4.89 .\) What is the \(K_{a}\) for the acid? (c) Using Appendix D, suggest the identity of the acid.

Consider a beaker containing a saturated solution of CaF \(_{2}\) in equilibrium with undissolved \(\mathrm{CaF}_{2}(s)\). Solid \(\mathrm{CaCl}_{2}\) is then added to the solution. (a) Will the amount of solid \(\mathrm{CaF}_{2}\) at the bottom of the beaker increase, decrease, or remain the same? (b) Will the concentration of \(\mathrm{Ca}^{2+}\) ions in solution increase or decrease? (c) Will the concentration of F ions in solution increase or decrease?

A sample of \(7.5 \mathrm{~L}\) of \(\mathrm{NH}_{3}\) gas at \(22^{\circ} \mathrm{C}\) and 735 torr is bubbled into a \(0.50-\mathrm{L}\) solution of \(0.40 \mathrm{M} \mathrm{HCl}\). Assuming that all the \(\mathrm{NH}_{3}\) dissolves and that the volume of the solution remains \(0.50 \mathrm{~L},\) calculate the \(\mathrm{pH}\) of the resulting solution.

The acid-base indicator bromcresol green is a weak acid. The yellow acid and blue base forms of the indicator are present in equal concentrations in a solution when the pH is \(4.68 .\) What is the \(p K_{a}\) for bromcresol green?

A sample of \(0.2140 \mathrm{~g}\) of an unknown monoprotic acid was dissolved in \(25.0 \mathrm{~mL}\) of water and titrated with \(0.0950 \mathrm{M}\) \(\mathrm{NaOH}\). The acid required \(30.0 \mathrm{~mL}\). of base to reach the equivalence point. (a) What is the molar mass of the acid? (b) After \(15.0 \mathrm{~mL}\) of base had been added in the titration, the \(\mathrm{pH}\) was found to be \(6.50 .\) What is the \(K_{a}\) for the unknown acid?
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