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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

Classify each of the following as a strong acid, weak acid, strong base, or weak base in aqueous solution. a. \(\mathrm{HNO}_{2}\) b. HNO \(_{3}\) c. \(\mathrm{CH}_{3} \mathrm{NH}_{2}\) d. \(\mathrm{NaOH}\) e. \(\mathrm{NH}_{3}\) f. \(\mathrm{HF}\) g. \(\mathrm{HC}-\mathrm{OH}\) h. \(\mathrm{Ca}(\mathrm{OH})_{2}\) i. \(\mathrm{H}_{2} \mathrm{SO}_{4}\)

A typical aspirin tablet contains 325 mg acetylsalicylic acid \(\left(\mathrm{HC}_{9} \mathrm{H}_{7} \mathrm{O}_{4}\right) .\) Calculate the \(\mathrm{pH}\) of a solution that is prepared by dissolving two aspirin tablets in enough water to make one \(\operatorname{cup}(237 \mathrm{mL})\) of solution. Assume the aspirin tablets are pure acetylsalicylic acid, \(K_{\mathrm{a}}=3.3 \times 10^{-4}\) .

When determining the pH of a weak acid solution, sometimes the 5\(\%\) rule can be applied to simplify the math. At what \(K_{\mathrm{a}}\) values will a \(1.0-M\) solution of a weak acid follow the 5\(\%\) rule?

Calculate the mass of \(\mathrm{HONH}_{2}\) required to dissolve in enough water to make 250.0 \(\mathrm{mL}\) of solution having a pH of 10.00\(\left(K_{\mathrm{b}}\right.\) \(=1.1 \times 10^{-8} )\)

The pH of \(1.0 \times 10^{-8} M\) hydrochloric acid is not \(8.00 .\) The correct pH can be calculated by considering the relationship between the molarities of the three principal ions in the solution \(\left(\mathrm{H}^{+}, \mathrm{Cl}^{-}, \text { and } \mathrm{OH}^{-}\right) .\) These molarities can be calculated from algebraic equations that can be derived from the considerations given below. a. The solution is electrically neutral. b. The hydrochloric acid can be assumed to be 100\(\%\) ionized. c. The product of the molarities of the hydronium ions and the hydroxide ions must equal \(K_{w}\) Calculate the pH of a \(1.0 \times 10^{-8}-M\) HCl solution.
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