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Chapter 15: Q113E (page 879)

What is the effect on the amount of\(CaHP{O_4}\) that dissolves and the concentrations of \(C{a^{2 + }}\;and\;HPO_4^ - \)when each of the following are added to a mixture of solid \(CaHP{O_4}\)and water at equilibrium?

\(\;(a)\;CaC{l_2}\)

\(\;(b)\;HCl\)

\(\;(c)\;KCl{O_4}\)

\(\;(d)\;NaOH\)

\(\;(e)\;CaHP{O_4}\)

Short Answer

Expert verified

The amount of \({\rm{CaHP}}{{\rm{O}}_4}\)and concentration of \({\rm{C}}{{\rm{a}}^{2 + }}\) increases, and the concentration of \({\rm{HP}}{{\rm{O}}_4}^{2 - }\) decreases

Step by step solution

01

Define CaCl2

Calcium chloride is an inorganic compound, a salt with the chemical formula\({\rm{CaC}}{{\rm{l}}_2}\). It is a white crystalline solid at room temperature, and it is highly soluble in water. It can be created by neutralizing hydrochloric acid with calcium hydroxide.

02

Concentration of increases and decreases

Since\({\rm{C}}{{\rm{a}}^{2 + }}\)is added, equilibrium will shift to the left, hence, the amount of\({\rm{CaHP}}{{\rm{O}}_4}\)and concentration of\({\rm{C}}{{\rm{a}}^{2 + }}\)increases, and the concentration of\({\rm{HP}}{{\rm{O}}_4}^{2 - }\)decreases.

\(\;(b)\;HCl\)

Answer:

The amount of \({\rm{CaHP}}{{\rm{O}}_4}\)and concentration of \({\rm{HP}}{{\rm{O}}_4}^{2 - }\)decreases, and the concentration of \({\rm{C}}{{\rm{a}}^{2 + }}\)increases

03

Define HCl

Hydrochloric acid \(\left[ {{{\rm{H}}^ + }{\rm{C}}{{\rm{l}}^ - }{\rm{or\;}}{{\rm{H}}_3}{{\rm{O}}^ + }{\rm{C}}{{\rm{l}}^ - }} \right]\)also known as muriatic acid, is an aqueous solution of hydrogen chloride. It is a colorless solution with a distinctive pungent smell. It is classified as a strong acid. It is a component of the gastric acid in the digestive systems of most animal species, including humans

04

Ions reacts

\({{\rm{H}}^ + }\)ions react with\({\rm{H}}{{\rm{P}}^2}{{\rm{O}}_4}^2\)ions, to produce\({{\rm{H}}_3}{\rm{P}}{{\rm{O}}_4}\).

Hence, the concentration of\({\rm{HP}}{{\rm{O}}_4}^{2 - }\)decreases. That causes the equilibrium to shift to the right, and the concentration of\({\rm{C}}{{\rm{a}}^{2 + }}\)increases, and the amount of\({\rm{CaHP}}{{\rm{O}}_4}\)decreases.

\(\;(c)\;KCl{O_4}\)

Answer:

No change in amount of \({\rm{CaHP}}{{\rm{O}}_4}\), and concentrations of\({\rm{C}}{{\rm{a}}^{2 + }}\), and \({\rm{HP}}{{\rm{O}}_4}^{2 - }\)

05

Define KCIO4

Potassium perchlorate is an inorganic salt with the chemical formula KClO4. It is a strong oxidizer with the lowest solubility of the alkali metal perchlorates. Potassium is most commonly used in flares and automobile airbags.

06

This salt does not contain common ions

Since this salt does not contain common ions, there will be no change in amount of\({\rm{CaHP}}{{\rm{O}}_4}\), and concentrations of\({\rm{C}}{{\rm{a}}^{2 + }}\), and\({\rm{HP}}{{\rm{O}}_4}^{2 - }\).

\(\;(d)\;NaOH\)

Answer:

The amount of \({\rm{CaHP}}{{\rm{O}}_4}\)and concentration of \({\rm{C}}{{\rm{a}}^{2 + }}\)decreases, and the concentration of \({\rm{HP}}{{\rm{O}}_4}^{2 - }\) increases

07

Define NaOH

Sodium hydroxide, also known as lye and caustic soda, is an inorganic compound with the formula NaOH. It is a white solid ionic compound consisting of sodium cations Na鈦� and hydroxide anions OH鈦�.

08

That causes the equilibrium to shift to the right

Here, we have addition of\({\rm{O}}{{\rm{H}}^ - }\)ions.\({\rm{O}}{{\rm{H}}^ - }\)ions reacts with\({\rm{C}}{{\rm{a}}^{2 + }}\)ions, to produce\(Ca{(OH)_2}\).

\(\;(e)\;CaHP{O_4}\)

Answer:

The concentration of\({\rm{C}}{{\rm{a}}^{2 + }}\), and \({\rm{HPO}}_4^{2 - }\)remain the same, but the amount of \({\rm{CaHP}}{{\rm{O}}_4}\) increases

09

Define CaHPO4

Dicalcium phosphate is the calcium phosphate with the formula \({\rm{CaHP}}{{\rm{O}}_4}\) and its dihydrate. The "di" prefix in the common name arises because the formation of the HPO鈧�2鈥� anion involves the removal of two protons from phosphoric acid, H鈧働O鈧�. It is also known as dibasic calcium phosphate or calcium monohydrogen phosphate.

10

The amount of increases.

When \({\rm{CaHP}}{{\rm{O}}_4}\)is added, the concentration of\({\rm{C}}{{\rm{a}}^{2 + }}\), and \({\rm{HPO}}_4^{2 - }\)remain the same, but the amount of \({\rm{CaHP}}{{\rm{O}}_4}\)increases.

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Most popular questions from this chapter

Question: 29. The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate \({K_{sp}}\) for each of the slightly soluble solids indicated:

(a) TlCl:\(\left( {T{l^ + }} \right) = 1.21 \times 1{0^{ - 2}}M,\left( {C{l^ - }} \right) = 1.2 \times 1{0^{ - 2}}M\)

(b)\(Ce{\left( {I{O_3}} \right)_4}:\left( {C{e^{4 + }}} \right) = 1.8 \times 1{0^{ - 4}}M,\left( {I{O_3}^ - } \right) = 2.6 \times 1{0^{ - 13}}M\)

(c)\(G{d_2}{\left( {S{O_4}} \right)_3}:\left( {G{d^{3 + }}} \right) = 0.132M,\left( {SO_4^{2 - }} \right) = 0.198M\)

(d)\(A{g_2}S{O_4}:\left( {A{g^ + }} \right) = 2.40 \times 1{0^{ - 2}}M,\left( {SO_4^{2 - }} \right) = 2.05 \times 1{0^{ - 2}}M\)

(e) \(BaS{O_4}:\left( {B{a^{2 + }}} \right) = 0.500M,\left( {SO_4^{2 - }} \right) = 2.16 \times 1{0^{ - 10}}M\)

Question: We have seen an introductory definition of an acid: An acid is a compound that reacts with water and increases the amount of hydronium ion present. In the chapter on acids and bases, we saw two more definitions of acids: a compound that donates a proton (a hydrogen ion, \({H^ + }\)) to another compound is called a Br酶nsted-Lowry acid, and a Lewis acid is any species that can accept a pair of electrons. Explain why the introductory definition is a macroscopic definition, while the Br酶nsted-Lowry definition and the Lewis definition are microscopic definitions.

Calculate the molar solubility of Sn (OH)2 in a buffer solution containing equal concentrations of NH3and NH4+.

Question:A saturated solution of a slightly soluble electrolyte in contact with some of the solid electrolyte is said to be a system in equilibrium. Explain. Why is such a system calling a heterogeneous equilibrium?

Question: In dilute aqueous solution HF acts as a weak acid. However, pure liquid HF (boiling point = 19.5 掳C) is a strong acid. In liquid HF, HNO3 acts like a base and accepts protons. The acidity of liquid HF can be increased by adding one of several inorganic fluorides that are Lewis acids and accept F鈥�ion (for example, BF3 or SbF5). Write balanced chemical equations for the reaction of pure HNO3 with pure HF and of pure HF with BF3.
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