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Chapter 19: Problem 80

Which compound in each pair is more soluble in water? (a) Strontium sulfate or barium chromate (b) Calcium carbonate or copper(II) carbonate (c) Barium iodate or silver chromate

Short Answer

Expert verified
Strontium sulfate, calcium carbonate, and barium iodate are more soluble in water in their respective pairs.

Step by step solution

01

Understand Solubility Rules

To determine which compound is more soluble in water, you need to apply solubility rules. Generally, compounds of Group 1 elements and ammonium are soluble, as well as nitrates, acetates, and most sulfates. On the other hand, carbonates, chromates, and phosphates are generally insoluble except when paired with Group 1 elements or ammonium.
02

Compare Strontium Sulfate and Barium Chromate

Strontium sulfate (SrSO₄) and barium chromate (BaCrO₄) both involve ions with sulfate and chromate. According to solubility rules, sulfates are generally soluble except for those of barium, calcium, and lead. Chromates are generally insoluble except for those of Group 1 elements and ammonium. Therefore, strontium sulfate is more soluble in water than barium chromate.
03

Compare Calcium Carbonate and Copper(II) Carbonate

Calcium carbonate (CaCO₃) and copper(II) carbonate (CuCO₃) are both carbonates. According to solubility rules, carbonates are generally insoluble except for those of Group 1 elements and ammonium. Neither calcium nor copper are Group 1 elements, so both compounds are generally insoluble. However, calcium carbonate is slightly more soluble in water compared to copper(II) carbonate.
04

Compare Barium Iodate and Silver Chromate

Barium iodate (Ba(IO₃)₂) and silver chromate (Ag₂CrO₄) involve iodate and chromate ions respectively. Iodates are generally soluble except for a few exceptions. Chromates are generally insoluble except for those involving Group 1 elements and ammonium. Based on the solubility rules, barium iodate is more soluble in water than silver chromate.

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Key Concepts

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

strontium sulfate
Strontium sulfate (SrSO₄) is a sulfate compound of strontium and sulfate ions. Generally, compounds containing sulfate ions are soluble in water. However, there are exceptions to this rule, namely with sulfate compounds of barium, calcium, and lead, which are less soluble. Strontium sulfate is more soluble compared to barium sulfate but less soluble than the sulfates of Group 1 elements. When comparing with other compounds in our exercise, considering solubility rules plays an essential role.
barium chromate
Barium chromate (BaCrO₄) is a compound consisting of barium and chromate ions. According to solubility rules, chromates are generally insoluble in water except when paired with Group 1 elements or ammonium. Barium belongs to Group 2, rendering barium chromate less soluble in water. This helps us understand why strontium sulfate is more soluble in water compared to barium chromate.
calcium carbonate
Calcium carbonate (CaCO₃) is comprised of calcium and carbonate ions. Carbonates are generally insoluble in water except for those containing Group 1 elements or ammonium. Neither calcium nor carbonate fits these categories, making calcium carbonate sparingly soluble in water. It is slightly more soluble than some other carbonates, such as copper(II) carbonate, due to its chemical properties.
copper(II) carbonate
Copper(II) carbonate (CuCO₃) consists of copper and carbonate ions. Similar to calcium carbonate, carbonates are typically insoluble unless paired with Group 1 elements or ammonium. Copper does not fall into these categories, resulting in copper(II) carbonate being mostly insoluble in water. This compound has even lower solubility compared to calcium carbonate.
barium iodate
Barium iodate (Ba(IO₃)₂) contains barium and iodate ions. Iodates are generally soluble, with a few exceptions. In this case, barium iodate is more soluble in water compared to compounds like silver chromate because of the general solubility tendency of iodates. Understanding solubility rules again helps explain this characteristic.
silver chromate
Silver chromate (Ag₂CrO₄) is a compound made up of silver and chromate ions. Chromates, according to solubility rules, are mostly insoluble except when associated with Group 1 elements or ammonium. Since silver does not belong to these categories, silver chromate is usually insoluble in water. This makes the compound less soluble compared to barium iodate.

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Most popular questions from this chapter

Write the ion-product expressions for (a) lead(II) iodide; (b) strontium sulfate; (c) chromium(III) hydroxide.

A 500.-mL solution consists of \(0.050 \mathrm{~mol}\) of solid \(\mathrm{NaOH}\) and \(0.13 \mathrm{~mol}\) of hypochlorous acid \(\left(\mathrm{HClO} ; K_{\mathrm{a}}=3.0 \times 10^{-8}\right)\) dissolved in water. (a) Aside from water, what is the concentration of each species that is present? (b) What is the \(\mathrm{pH}\) of the solution? (c) What is the pH after adding \(0.0050 \mathrm{~mol}\) of \(\mathrm{HCl}\) to the flask?

Gout is caused by an error in metabolism that leads to a buildup of uric acid in body fluids, which is deposited as slightly soluble sodium urate \(\left(\mathrm{C}_{5} \mathrm{H}_{3} \mathrm{~N}_{4} \mathrm{O}_{3} \mathrm{Na}\right)\) in the joints. If the extracellular \(\left[\mathrm{Na}^{+}\right]\) is \(0.15 \mathrm{M}\) and the solubility of sodium urate is \(0.085 \mathrm{~g} / 100 . \mathrm{mL}\) what is the minimum urate ion concentration (abbreviated [Ur-]) that will cause a deposit of sodium urate?

The normal \(\mathrm{pH}\) of blood is \(7.40 \pm 0.05\) and is controlled in part by the \(\mathrm{H}_{2} \mathrm{CO}_{3} / \mathrm{HCO}_{3}^{-}\) buffer system. (a) Assuming that the \(K_{\mathrm{a}}\) value for carbonic acid at \(25^{\circ} \mathrm{C}\) applies to blood, what is the \(\left[\mathrm{H}_{2} \mathrm{CO}_{3}\right] /\left[\mathrm{HCO}_{3}^{-}\right]\) ratio in normal blood? (b) In a condition called acidosis, the blood is too acidic. What is the \(\left[\mathrm{H}_{2} \mathrm{CO}_{3}\right] /\left[\mathrm{HCO}_{3}^{-}\right]\) ratio in a patient whose blood \(\mathrm{pH}\) is \(7.20 ?\)

EDTA binds metal ions to form complex ions (see Problem 19.142 ) , so it is used to determine the concentrations of metal ions in solution: $$ \mathrm{M}^{n+}(a q)+\mathrm{EDTA}^{4-}(a q) \longrightarrow \mathrm{MEDTA}^{n-4}(a q) $$ A \(50.0-\mathrm{mL}\) sample of \(0.048 M \mathrm{Co}^{2+}\) is titrated with \(0.050 M\) EDTA \(^{4-}\). Find \(\left[\mathrm{Co}^{2+}\right]\) and \(\left[\mathrm{EDTA}^{4-}\right]\) after addition of (a) \(25.0 \mathrm{~mL}\) and \((b) 75.0 m L\) of \(E D T A^{4-}\left(\log K_{f}\right.\) of \(\left.C o E D T A^{2-}=16.31\right)\)
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