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Chapter 7: Problem 34

Write the formulas and names of three common strong acids and strong bases.

Short Answer

Expert verified
Three common strong acids are Hydrochloric acid (\(HCl\)), Nitric acid (\(HNO_3\)), and Sulfuric acid (\(H_2SO_4\)). Three common strong bases are Sodium hydroxide (\(NaOH\)), Potassium hydroxide (\(KOH\)), and Calcium hydroxide (\(Ca(OH)_2\)).

Step by step solution

01

Strong Acids

Here are three common strong acids with their names and chemical formulas: 1. Hydrochloric acid: \(HCl\) 2. Nitric acid: \(HNO_3\) 3. Sulfuric acid: \(H_2SO_4\)
02

Strong Bases

Now, let's list three common strong bases with their names and chemical formulas: 1. Sodium hydroxide: \(NaOH\) 2. Potassium hydroxide: \(KOH\) 3. Calcium hydroxide: \(Ca(OH)_2\)

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Most popular questions from this chapter

Distinguish between what we mean by a singledisplacement reaction and a double-displacement reaction by giving two examples of each type.

Identify each of the following unbalanced reaction equations as belonging to one or more of the following categories: precipitation, acid-base, or oxidation-reduction. a. \(\mathrm{H}_{2} \mathrm{O}_{2}(a q) \rightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{O}_{2}(g)\) b. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Cu}(s) \rightarrow \mathrm{CuSO}_{4}(a q)+\mathrm{H}_{2}(g)\) c. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{NaOH}(a q) \rightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) d. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q) \rightarrow \mathrm{BaSO}_{4}(s)+\mathrm{H}_{2} \mathrm{O}(l)\) e. \(\mathrm{AgNO}_{3}(a q)+\mathrm{CuCl}_{2}(a q) \rightarrow \mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\) \(\mathrm{AgCl}(s)\) f. \(\mathrm{KOH}(a q)+\mathrm{CuSO}_{4}(a q) \rightarrow \mathrm{Cu}(\mathrm{OH})_{2}(s)+\mathrm{K}_{2} \mathrm{SO}_{4}(a q)\) g. \(\mathrm{Cl}_{2}(g)+\mathrm{F}_{2}(g) \rightarrow \operatorname{ClF}(g)\) h. \(\mathrm{NO}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{NO}_{2}(g)\) i. \(\mathrm{Ca}(\mathrm{OH})_{2}(s)+\mathrm{HNO}_{3}(a q) \rightarrow \mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\)

On the basis of the general solubility rules given in Table \(7.1,\) predict which of the following substances are likely to be soluble in water. a. zinc chloride b. lead(II) nitrate c. lead(II) sulfate d. sodium iodide e. cobalt(III) sulfide f. chromium(III) hydroxide g. magnesium carbonate h. ammonium carbonate

Sulfuric acid, \(\mathrm{H}_{2} \mathrm{SO}_{4}\), oxidizes many metallic elements. One of the effects of acid rain is that it produces sulfuric acid in the atmosphere, which then reacts with metals used in construction. Write balanced oxidation-reduction equations for the reaction of sulfuric acid with Fe, \(\mathrm{Zn}, \mathrm{Mg}, \mathrm{Co},\) and \(\mathrm{Ni}\).

What strong acid and what strong base would react in aqueous solution to produce the following salts? a. potassium perchlorate, \(\mathrm{KClO}_{4}\) b. cesium nitrate, \(\mathrm{CSNO}_{3}\) c. potassium chloride, KCl d. sodium sulfate, \(\mathrm{Na}_{2} \mathrm{SO}_{4}\)
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