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Chapter 14: Problem 136

Will the following oxides give acidic, basic, or neutral solutions when dissolved in water? Write reactions to justify your answers. a. \(\mathrm{Li}_{2} \mathrm{O}\) b. \(\mathrm{CO}_{2}\) c. \(\mathrm{SrO}\)

Short Answer

Expert verified
a. Li2O forms a basic solution when dissolved in water. Equation: \(Li_2O + H_2O \rightarrow 2 LiOH\) b. CO2 forms an acidic solution when dissolved in water. Equation: \(CO_2 + H_2O \rightarrow H_2CO_3\) c. SrO forms a basic solution when dissolved in water. Equation: \(SrO + H_2O \rightarrow Sr(OH)_2\)

Step by step solution

01

Classification of Oxides

Oxides can typically be divided into three categories: acidic, basic, and amphoteric. Acidic oxides are non-metallic oxides that react with water to form acidic solutions. Basic oxides are metallic oxides that react with water to form basic solutions. Amphoteric oxides can behave as both acidic and basic oxides depending on the conditions.
02

Li2O+Evaluating

Lithium oxide (Li2O) is a metallic oxide. When metallic oxides dissolve in water, they typically form a basic solution. We will write the chemical equation to observe this process. Li2O + H2O -> 2 LiOH The presence of the hydroxide ions (OH-) in the solution indicates that Li2O forms a basic solution when dissolved in water.
03

CO2 - Evaluating

Carbon dioxide (CO2) is a non-metallic oxide. When non-metallic oxides dissolve in water, they typically form acidic solutions. We will write the chemical equation to observe this process. CO2 + H2O -> H2CO3 The formation of carbonic acid (H2CO3) indicates that CO2 forms an acidic solution when dissolved in water.
04

SrO - Evaluating

Strontium oxide (SrO) is a metallic oxide. When metallic oxides dissolve in water, they typically form a basic solution. We will write the chemical equation to observe this process. SrO + H2O -> Sr(OH)2 The presence of the hydroxide ions (OH-) in the solution indicates that SrO forms a basic solution when dissolved in water.
05

Final Answers

Based on our analysis, we can conclude the following: a. Li2O forms a basic solution when dissolved in water. Equation: Li2O + H2O -> 2 LiOH b. CO2 forms an acidic solution when dissolved in water. Equation: CO2 + H2O -> H2CO3 c. SrO forms a basic solution when dissolved in water. Equation: SrO + H2O -> Sr(OH)2

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Most popular questions from this chapter

Calculate the concentration of an aqueous \(\mathrm{Sr}(\mathrm{OH})_{2}\) that has \(\mathrm{pH}=10.50\) .

A solution is made by adding 50.0 \(\mathrm{mL}\) of 0.200\(M\) acetic acid \(\left(K_{\mathrm{a}}=1.8 \times 10^{-5}\right)\) to 50.0 \(\mathrm{mL}\) of \(1.00 \times 10^{-3} \mathrm{M} \mathrm{HCl}\) a. Calculate the pH of the solution. b. Calculate the acetate ion concentration.

For solutions of the same concentration, as acid strength increases, indicate what happens to each of the following (increases, decreases, or doesn't change). $$ \begin{array}{ll}{\text { a. }\left[\mathrm{H}^{+}\right]} & {\text { d. pOH }} \\ {\text { b. pH }} & {\text { e. } K_{\mathrm{a}}} \\ {\text { c. }\left[\mathrm{OH}^{-}\right]}\end{array} $$

An acid \(\mathrm{HX}\) is 25\(\%\) dissociated in water. If the equilibrium concentration of \(\mathrm{HX}\) is \(0.30 \mathrm{M},\) calculate the \(K_{\mathrm{a}}\) value for \(\mathrm{HX}\) .

a. The principal equilibrium in a solution of \(\mathrm{NaHCO}_{3}\) is $$ \mathrm{HCO}_{3}^{-}(a q)+\mathrm{HCO}_{3}^{-}(a q) \rightleftharpoons \mathrm{H}_{2} \mathrm{CO}_{3}(a q)+\mathrm{CO}_{3}^{2-}(a q) $$ Calculate the value of the equilibrium constant for this reaction. b. At equilibrium, what is the relationship between $\left[\mathrm{H}_{2} \mathrm{CO}_{3}\right]\( and \)\left[\mathrm{CO}_{3}^{2-}\right] ?$ c. Using the equilibrium $$ \mathrm{H}_{2} \mathrm{CO}_{3}(a q) \rightleftharpoons 2 \mathrm{H}^{+}(a q)+\mathrm{CO}_{3}^{2-}(a q) $$ derive an expression for the pH of the solution in terms of \(K_{\mathrm{a}_{1}}\) and \(K_{\mathrm{a}_{2}}\) using the result from part b. d. What is the pH of a solution of \(\mathrm{NaHCO}_{3} ?\)
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