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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

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. \(\operatorname{Fe}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{Fe}_{3}\left(\mathrm{SO}_{4}\right)_{2}(a q)+\mathrm{H}_{2}(g)\) b. \(\mathrm{HClO}_{4}(a q)+\mathrm{RbOH}(a q) \rightarrow \mathrm{RbClO}_{4}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) \(\overline{\mathrm{c}} . \mathrm{Ca}(s)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CaO}(s)\) d. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{NaOH}(a q) \rightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) e. \(\operatorname{Pb}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{Na}_{2} \mathrm{CO}_{3}(a q) \rightarrow\) \(\mathrm{PbCO}_{3}(s)+\mathrm{NaNO}_{3}(a q)\) f. \(\mathrm{K}_{2} \mathrm{SO}_{4}(a q)+\mathrm{CaCl}_{2}(a q) \rightarrow \mathrm{KCl}(a q)+\mathrm{CaSO}_{4}(s)\) g. \(\mathrm{HNO}_{3}(a q)+\mathrm{KOH}(a q) \rightarrow \mathrm{KNO}_{3}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) h. \(\mathrm{Ni}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}(a q)+\mathrm{Na}_{2} \mathrm{S}(a q) \rightarrow\) \(\mathrm{NiS}(s)+\mathrm{NaC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)\) i. \(\mathrm{Ni}(s)+\mathrm{Cl}_{2}(g) \rightarrow \mathrm{NiCl}_{2}(s)\)

Write balanced net ionic equations for the reactions that occur when the following aqueous solutions are mixed. If no reaction is likely to occur, so indicate. a. sodium sulfate and potassium chloride b. potassium sulfide and calcium nitrate c. sodium hydroxide and silver nitrate d. sodium carbonate and iron(III) chloride e. ammonium phosphate and aluminum chloride f. barium nitrate and potassium chloride

There is much overlapping of the classification schemes for reactions discussed in this chapter. Give an example of a reaction that is, at the same time,an oxidation-reduction reaction, a combustion reaction, and a synthesis reaction.

What is meant by a strong base? Are the strong bases also strong electrolytes? Explain.

For the reaction \(2 \mathrm{Al}(s)+3 \mathrm{Br}_{2}(l) \rightarrow 2 \mathrm{AlBr}_{3}(s),\) show how electrons are gained and lost by the atoms.
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